Percent yield of HSiCl 3 is to be calculated. Concept introduction: The expression to determine number of moles is as follows: Number of moles = Given Mass Molar mass The formula to calculate moles as per ideal gas law is as follows: n = P V R T Where, R is gas constant. V denotes the volume. n denotes number of moles. T denotes temperature. P denotes pressure.

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Answer 1

Question

Chapter 5, Problem 68E

(a)

Interpretation Introduction

Interpretation:Percent yield of $HSiCl3$ is to be calculated.

Concept introduction: The expression to determine number of moles is as follows:

$Number of moles=Given MassMolar mass$

The formula to calculate moles as per ideal gas law is as follows:

$n=PVRT$

Where,

$R$ is gas constant.

$V$ denotes the volume.

$n$ denotes number of moles.

$T$ denotes temperature.

$P$ denotes pressure.

(a)

Expert Solution

Answer to Problem 68E

Percent yield of $HSiCl3$ is $78.017 %$ .

Explanation of Solution

Given Information:

Density of $HSiCl3$ is $0.850 g/mL$ .

Pressure of $HCl$ is $10 atm$ .

Volume of $HCl$ is $15.0 L$ .

Temperature in Celsius is $35 °C$ .

The formula to convert degree Celsius to kelvin is as follows:

$T(K)=T(°C)+273 K$

Temperature in Celsius is $35 °C$ .

Substitute the value in the above formula.

$T(K)=T(°C)+273 K=35 °C+273 K=308 K$

The formula to calculate mass from density is as follows:

$Mass=(Volume)(Density)$

For $HSiCl3$

Volume is $156 mL$ .

Density is $1.34 g/mL$ .

Substitute the value in above formula.

$Mass=(Volume)(Density)=(156 mL)(1.34 g/mL)=209.04 g$

The expression to determine number of moles is as follows:

$Number of moles=Mass of HSiCl3Molar mass of HSiCl3$

Mass of $HSiCl3$ is $209.04 g$ .

Molar mass of $HSiCl3$ is $135.45 g/mol$ .

Substitute the value in above formula.

$Number of moles= Mass of HSiCl3 Molar mass of HSiCl3=209.04 g135.45 g/mol=1.3264 mol$

The balanced equation for formation of $HSiCl3$ is as follows:

$Si(s)+3HCl(g)→HSiCl3+H2(g)$

The formula to calculate moles as per ideal gas law is as follows:

$n=PVRT$

The value of $P$ is $10 atm$ .

The value of $V$ is $15.0 L$ .

The value of $T$ is $308 K$ .

The value of $R$ is $0.08206 L⋅atm/mol⋅K$ .

Substitute the value in above equation.

$n=PVRT=( 10 atm)( 15.0 L)( 0.08206 L⋅atm/mol⋅K)( 308 K)=5.9348 mol$

In accordance with balanced equation, $3 mol HCl$ forms $1 mol HSiCl3$ , thus moles of $HSiCl3$ formed from $5.9348 mol HCl$ is calculated as follows:

$Moles of HSiCl3=(5.9348 mol HCl)( 1 mol HSiCl 3 3 mol HCl)=1.9782 mol HSiCl3$

The formula to calculate mass from moles is given as follows:

$Mass=(Number of moles)(Molar mass)$

Number of moles is $1.9782 mol$ .

Molar mass is $135.45 g/mol$ .

Substitute the values in above formula.

$Mass=(Number of moles)(Molar mass)=(1.9782 mol)(135.45 g/mol)=267.94 g$

Thus, theoretical yield of $HSiCl3$ expected $267.94 g$ .

The formula to calculate percent yield is as follows:

$Percent yield=(Observed yieldTheoretical yield)(100 %)$

Observed yield is $209.04 g$ .

Theoretical yield is $267.94 g$ .

Substitute the value in above formula.

$Percent yield=( Observed yield Theoretical yield)(100 %)=( 209.04 g 267.94 g)(100 %)=78.017 %$

(b)

Interpretation Introduction

Interpretation:Volume of $SiH4$ when percent yield of $HSiCl3$ is $93.1 %$ isto be calculated.

Concept introduction: The expression to determine number of moles is as follows:

$Number of moles=Given MassMolar mass$

The formula to calculate moles as per ideal gas law is as follows:

$n=PVRT$

Where,

$R$ is gas constant.

$V$ denotes the volume.

$n$ denotes number of moles.

$T$ denotes temperature.

$P$ denotes pressure.

(b)

Expert Solution

Answer to Problem 68E

Volume of $SiH4$ is $907.87 mL$ .

Explanation of Solution

The formula to convert degree Celsius to kelvin is as follows:

$T(K)=T(°C)+273 K$

Temperature in Celsius is $35 °C$ .

Substitute the value in the above formula.

$T(K)=T(°C)+273 K=35 °C+273 K=308 K$

The formula to calculate mass from density is as follows:

$Mass=(Volume)(Density)$

For $HSiCl3$

Volume is $156 mL$ .

Density is $1.34 g/mL$ .

Substitute the value in above formula.

$Mass=(Volume)(Density)=(156 mL)(1.34 g/mL)=209.04 g$

The expression to determine number of moles is as follows:

$Number of moles=Mass of HSiCl3Molar mass of HSiCl3$

Mass of $HSiCl3$ is $209.04 g$ .

Molar mass of $HSiCl3$ is $135.45 g/mol$ .

Substitute the value in above formula.

$Number of moles= Mass of HSiCl3 Molar mass of HSiCl3=209.04 g135.45 g/mol=1.5433 mol$

The balanced equation for formation of $HSiCl3$ is as follows:

$4HSiCl3(l)→SiH4+3SiCl4(l)$

The formula to calculate moles as per ideal gas law is as follows:

$n=PVRT$

The value of $P$ is $10 atm$ .

The value of $V$ is $15.0 L$ .

The value of $T$ is $308 K$ .

The value of $R$ is $0.08206 L⋅atm/mol⋅K$ .

Substitute the value in above equation.

$n=PVRT=( 10 atm)( 15.0 L)( 0.08206 L⋅atm/mol⋅K)( 308 K)=5.9348 mol$

In accordance with balanced equation, $4 mol HSiCl3$ forms $1 mol SiH4$ , thus moles of $SiH4$ formed from $1.5433 mol HSiCl3$ is calculated as follows:

$Moles of SiH4=(1.5433 mol HSiCl3)( 1 mol SiH 4 4 mol HSiCl 3 )=0.385825 mol SiH4$

The formula to calculate mass from moles is given as follows:

$Mass=(Number of moles)(Molar mass)$

Number of moles is $0.385825 mol$ .

Molar mass is $32.12 g/mol$ .

Substitute the values in above formula.

$Mass=(0.385825 mol)(32.12 g/mol)=12.3929 g$

The formula to calculate percent yield is as follows:

$Percent yield=(Observed yieldTheoretical yield)(100 %)$

Percent yield is $93.1 %$ .

Theoretical yield is $12.3929 g$ .

Substitute the value in above formula.

$Percent yield=( Observed yield Theoretical yield)(100 %)93.1 %=( Observed yield 12.3929 g)(100 %)$

Rearrange to obtain the observed yield.

$Observed yield=( 93.1 % 100 %)(12.3929 g)=11.5377 g$

The formula to calculate volume as per ideal gas law is as follows:

$V=mRTMP$

The value of $P$ is $10 atm$ .

The value of $m$ is $11.5377 g$ .

The value of $M$ is $32.12 g/mol$ .

The value of $T$ is $308 K$ .

The value of $R$ is $0.08206 L⋅atm/mol⋅K$ .

Substitute the values in above equation.

$V=mRTMP=( 11.5377 g)( 0.08206 L⋅atm/mol⋅K)( 308 K)( 32.12 g/mol)( 10 atm)=0.90787 L$

The conversion factor to convert liters to milliliters is as follows:

$1 L=1000 mL$

Hence convert $0.90787 L$ to $mL$ as follows:

$Volume=(0.90787 L)( 1000 mL 1 L)=907.87 mL$

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Answer 2

Question

Chapter 5, Problem 68E

(a)

Interpretation Introduction

Interpretation:Percent yield of $HSiCl3$ is to be calculated.

Concept introduction: The expression to determine number of moles is as follows:

$Number of moles=Given MassMolar mass$

The formula to calculate moles as per ideal gas law is as follows:

$n=PVRT$

Where,

$R$ is gas constant.

$V$ denotes the volume.

$n$ denotes number of moles.

$T$ denotes temperature.

$P$ denotes pressure.

(a)

Expert Solution

Answer to Problem 68E

Percent yield of $HSiCl3$ is $78.017 %$ .

Explanation of Solution

Given Information:

Density of $HSiCl3$ is $0.850 g/mL$ .

Pressure of $HCl$ is $10 atm$ .

Volume of $HCl$ is $15.0 L$ .

Temperature in Celsius is $35 °C$ .

The formula to convert degree Celsius to kelvin is as follows:

$T(K)=T(°C)+273 K$

Temperature in Celsius is $35 °C$ .

Substitute the value in the above formula.

$T(K)=T(°C)+273 K=35 °C+273 K=308 K$

The formula to calculate mass from density is as follows:

$Mass=(Volume)(Density)$

For $HSiCl3$

Volume is $156 mL$ .

Density is $1.34 g/mL$ .

Substitute the value in above formula.

$Mass=(Volume)(Density)=(156 mL)(1.34 g/mL)=209.04 g$

The expression to determine number of moles is as follows:

$Number of moles=Mass of HSiCl3Molar mass of HSiCl3$

Mass of $HSiCl3$ is $209.04 g$ .

Molar mass of $HSiCl3$ is $135.45 g/mol$ .

Substitute the value in above formula.

$Number of moles= Mass of HSiCl3 Molar mass of HSiCl3=209.04 g135.45 g/mol=1.3264 mol$

The balanced equation for formation of $HSiCl3$ is as follows:

$Si(s)+3HCl(g)→HSiCl3+H2(g)$

The formula to calculate moles as per ideal gas law is as follows:

$n=PVRT$

The value of $P$ is $10 atm$ .

The value of $V$ is $15.0 L$ .

The value of $T$ is $308 K$ .

The value of $R$ is $0.08206 L⋅atm/mol⋅K$ .

Substitute the value in above equation.

$n=PVRT=( 10 atm)( 15.0 L)( 0.08206 L⋅atm/mol⋅K)( 308 K)=5.9348 mol$

In accordance with balanced equation, $3 mol HCl$ forms $1 mol HSiCl3$ , thus moles of $HSiCl3$ formed from $5.9348 mol HCl$ is calculated as follows:

$Moles of HSiCl3=(5.9348 mol HCl)( 1 mol HSiCl 3 3 mol HCl)=1.9782 mol HSiCl3$

The formula to calculate mass from moles is given as follows:

$Mass=(Number of moles)(Molar mass)$

Number of moles is $1.9782 mol$ .

Molar mass is $135.45 g/mol$ .

Substitute the values in above formula.

$Mass=(Number of moles)(Molar mass)=(1.9782 mol)(135.45 g/mol)=267.94 g$

Thus, theoretical yield of $HSiCl3$ expected $267.94 g$ .

The formula to calculate percent yield is as follows:

$Percent yield=(Observed yieldTheoretical yield)(100 %)$

Observed yield is $209.04 g$ .

Theoretical yield is $267.94 g$ .

Substitute the value in above formula.

$Percent yield=( Observed yield Theoretical yield)(100 %)=( 209.04 g 267.94 g)(100 %)=78.017 %$

(b)

Interpretation Introduction

Interpretation:Volume of $SiH4$ when percent yield of $HSiCl3$ is $93.1 %$ isto be calculated.

Concept introduction: The expression to determine number of moles is as follows:

$Number of moles=Given MassMolar mass$

The formula to calculate moles as per ideal gas law is as follows:

$n=PVRT$

Where,

$R$ is gas constant.

$V$ denotes the volume.

$n$ denotes number of moles.

$T$ denotes temperature.

$P$ denotes pressure.

(b)

Expert Solution

Answer to Problem 68E

Volume of $SiH4$ is $907.87 mL$ .

Explanation of Solution

The formula to convert degree Celsius to kelvin is as follows:

$T(K)=T(°C)+273 K$

Temperature in Celsius is $35 °C$ .

Substitute the value in the above formula.

$T(K)=T(°C)+273 K=35 °C+273 K=308 K$

The formula to calculate mass from density is as follows:

$Mass=(Volume)(Density)$

For $HSiCl3$

Volume is $156 mL$ .

Density is $1.34 g/mL$ .

Substitute the value in above formula.

$Mass=(Volume)(Density)=(156 mL)(1.34 g/mL)=209.04 g$

The expression to determine number of moles is as follows:

$Number of moles=Mass of HSiCl3Molar mass of HSiCl3$

Mass of $HSiCl3$ is $209.04 g$ .

Molar mass of $HSiCl3$ is $135.45 g/mol$ .

Substitute the value in above formula.

$Number of moles= Mass of HSiCl3 Molar mass of HSiCl3=209.04 g135.45 g/mol=1.5433 mol$

The balanced equation for formation of $HSiCl3$ is as follows:

$4HSiCl3(l)→SiH4+3SiCl4(l)$

The formula to calculate moles as per ideal gas law is as follows:

$n=PVRT$

The value of $P$ is $10 atm$ .

The value of $V$ is $15.0 L$ .

The value of $T$ is $308 K$ .

The value of $R$ is $0.08206 L⋅atm/mol⋅K$ .

Substitute the value in above equation.

$n=PVRT=( 10 atm)( 15.0 L)( 0.08206 L⋅atm/mol⋅K)( 308 K)=5.9348 mol$

In accordance with balanced equation, $4 mol HSiCl3$ forms $1 mol SiH4$ , thus moles of $SiH4$ formed from $1.5433 mol HSiCl3$ is calculated as follows:

$Moles of SiH4=(1.5433 mol HSiCl3)( 1 mol SiH 4 4 mol HSiCl 3 )=0.385825 mol SiH4$

The formula to calculate mass from moles is given as follows:

$Mass=(Number of moles)(Molar mass)$

Number of moles is $0.385825 mol$ .

Molar mass is $32.12 g/mol$ .

Substitute the values in above formula.

$Mass=(0.385825 mol)(32.12 g/mol)=12.3929 g$

The formula to calculate percent yield is as follows:

$Percent yield=(Observed yieldTheoretical yield)(100 %)$

Percent yield is $93.1 %$ .

Theoretical yield is $12.3929 g$ .

Substitute the value in above formula.

$Percent yield=( Observed yield Theoretical yield)(100 %)93.1 %=( Observed yield 12.3929 g)(100 %)$

Rearrange to obtain the observed yield.

$Observed yield=( 93.1 % 100 %)(12.3929 g)=11.5377 g$

The formula to calculate volume as per ideal gas law is as follows:

$V=mRTMP$

The value of $P$ is $10 atm$ .

The value of $m$ is $11.5377 g$ .

The value of $M$ is $32.12 g/mol$ .

The value of $T$ is $308 K$ .

The value of $R$ is $0.08206 L⋅atm/mol⋅K$ .

Substitute the values in above equation.

$V=mRTMP=( 11.5377 g)( 0.08206 L⋅atm/mol⋅K)( 308 K)( 32.12 g/mol)( 10 atm)=0.90787 L$

The conversion factor to convert liters to milliliters is as follows:

$1 L=1000 mL$

Hence convert $0.90787 L$ to $mL$ as follows:

$Volume=(0.90787 L)( 1000 mL 1 L)=907.87 mL$

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Answer 3

Question

Chapter 5, Problem 68E

(a)

Interpretation Introduction

Interpretation:Percent yield of $HSiCl3$ is to be calculated.

Concept introduction: The expression to determine number of moles is as follows:

$Number of moles=Given MassMolar mass$

The formula to calculate moles as per ideal gas law is as follows:

$n=PVRT$

Where,

$R$ is gas constant.

$V$ denotes the volume.

$n$ denotes number of moles.

$T$ denotes temperature.

$P$ denotes pressure.

(a)

Expert Solution

Answer to Problem 68E

Percent yield of $HSiCl3$ is $78.017 %$ .

Explanation of Solution

Given Information:

Density of $HSiCl3$ is $0.850 g/mL$ .

Pressure of $HCl$ is $10 atm$ .

Volume of $HCl$ is $15.0 L$ .

Temperature in Celsius is $35 °C$ .

The formula to convert degree Celsius to kelvin is as follows:

$T(K)=T(°C)+273 K$

Temperature in Celsius is $35 °C$ .

Substitute the value in the above formula.

$T(K)=T(°C)+273 K=35 °C+273 K=308 K$

The formula to calculate mass from density is as follows:

$Mass=(Volume)(Density)$

For $HSiCl3$

Volume is $156 mL$ .

Density is $1.34 g/mL$ .

Substitute the value in above formula.

$Mass=(Volume)(Density)=(156 mL)(1.34 g/mL)=209.04 g$

The expression to determine number of moles is as follows:

$Number of moles=Mass of HSiCl3Molar mass of HSiCl3$

Mass of $HSiCl3$ is $209.04 g$ .

Molar mass of $HSiCl3$ is $135.45 g/mol$ .

Substitute the value in above formula.

$Number of moles= Mass of HSiCl3 Molar mass of HSiCl3=209.04 g135.45 g/mol=1.3264 mol$

The balanced equation for formation of $HSiCl3$ is as follows:

$Si(s)+3HCl(g)→HSiCl3+H2(g)$

The formula to calculate moles as per ideal gas law is as follows:

$n=PVRT$

The value of $P$ is $10 atm$ .

The value of $V$ is $15.0 L$ .

The value of $T$ is $308 K$ .

The value of $R$ is $0.08206 L⋅atm/mol⋅K$ .

Substitute the value in above equation.

$n=PVRT=( 10 atm)( 15.0 L)( 0.08206 L⋅atm/mol⋅K)( 308 K)=5.9348 mol$

In accordance with balanced equation, $3 mol HCl$ forms $1 mol HSiCl3$ , thus moles of $HSiCl3$ formed from $5.9348 mol HCl$ is calculated as follows:

$Moles of HSiCl3=(5.9348 mol HCl)( 1 mol HSiCl 3 3 mol HCl)=1.9782 mol HSiCl3$

The formula to calculate mass from moles is given as follows:

$Mass=(Number of moles)(Molar mass)$

Number of moles is $1.9782 mol$ .

Molar mass is $135.45 g/mol$ .

Substitute the values in above formula.

$Mass=(Number of moles)(Molar mass)=(1.9782 mol)(135.45 g/mol)=267.94 g$

Thus, theoretical yield of $HSiCl3$ expected $267.94 g$ .

The formula to calculate percent yield is as follows:

$Percent yield=(Observed yieldTheoretical yield)(100 %)$

Observed yield is $209.04 g$ .

Theoretical yield is $267.94 g$ .

Substitute the value in above formula.

$Percent yield=( Observed yield Theoretical yield)(100 %)=( 209.04 g 267.94 g)(100 %)=78.017 %$

(b)

Interpretation Introduction

Interpretation:Volume of $SiH4$ when percent yield of $HSiCl3$ is $93.1 %$ isto be calculated.

Concept introduction: The expression to determine number of moles is as follows:

$Number of moles=Given MassMolar mass$

The formula to calculate moles as per ideal gas law is as follows:

$n=PVRT$

Where,

$R$ is gas constant.

$V$ denotes the volume.

$n$ denotes number of moles.

$T$ denotes temperature.

$P$ denotes pressure.

(b)

Expert Solution

Answer to Problem 68E

Volume of $SiH4$ is $907.87 mL$ .

Explanation of Solution

The formula to convert degree Celsius to kelvin is as follows:

$T(K)=T(°C)+273 K$

Temperature in Celsius is $35 °C$ .

Substitute the value in the above formula.

$T(K)=T(°C)+273 K=35 °C+273 K=308 K$

The formula to calculate mass from density is as follows:

$Mass=(Volume)(Density)$

For $HSiCl3$

Volume is $156 mL$ .

Density is $1.34 g/mL$ .

Substitute the value in above formula.

$Mass=(Volume)(Density)=(156 mL)(1.34 g/mL)=209.04 g$

The expression to determine number of moles is as follows:

$Number of moles=Mass of HSiCl3Molar mass of HSiCl3$

Mass of $HSiCl3$ is $209.04 g$ .

Molar mass of $HSiCl3$ is $135.45 g/mol$ .

Substitute the value in above formula.

$Number of moles= Mass of HSiCl3 Molar mass of HSiCl3=209.04 g135.45 g/mol=1.5433 mol$

The balanced equation for formation of $HSiCl3$ is as follows:

$4HSiCl3(l)→SiH4+3SiCl4(l)$

The formula to calculate moles as per ideal gas law is as follows:

$n=PVRT$

The value of $P$ is $10 atm$ .

The value of $V$ is $15.0 L$ .

The value of $T$ is $308 K$ .

The value of $R$ is $0.08206 L⋅atm/mol⋅K$ .

Substitute the value in above equation.

$n=PVRT=( 10 atm)( 15.0 L)( 0.08206 L⋅atm/mol⋅K)( 308 K)=5.9348 mol$

In accordance with balanced equation, $4 mol HSiCl3$ forms $1 mol SiH4$ , thus moles of $SiH4$ formed from $1.5433 mol HSiCl3$ is calculated as follows:

$Moles of SiH4=(1.5433 mol HSiCl3)( 1 mol SiH 4 4 mol HSiCl 3 )=0.385825 mol SiH4$

The formula to calculate mass from moles is given as follows:

$Mass=(Number of moles)(Molar mass)$

Number of moles is $0.385825 mol$ .

Molar mass is $32.12 g/mol$ .

Substitute the values in above formula.

$Mass=(0.385825 mol)(32.12 g/mol)=12.3929 g$

The formula to calculate percent yield is as follows:

$Percent yield=(Observed yieldTheoretical yield)(100 %)$

Percent yield is $93.1 %$ .

Theoretical yield is $12.3929 g$ .

Substitute the value in above formula.

$Percent yield=( Observed yield Theoretical yield)(100 %)93.1 %=( Observed yield 12.3929 g)(100 %)$

Rearrange to obtain the observed yield.

$Observed yield=( 93.1 % 100 %)(12.3929 g)=11.5377 g$

The formula to calculate volume as per ideal gas law is as follows:

$V=mRTMP$

The value of $P$ is $10 atm$ .

The value of $m$ is $11.5377 g$ .

The value of $M$ is $32.12 g/mol$ .

The value of $T$ is $308 K$ .

The value of $R$ is $0.08206 L⋅atm/mol⋅K$ .

Substitute the values in above equation.

$V=mRTMP=( 11.5377 g)( 0.08206 L⋅atm/mol⋅K)( 308 K)( 32.12 g/mol)( 10 atm)=0.90787 L$

The conversion factor to convert liters to milliliters is as follows:

$1 L=1000 mL$

Hence convert $0.90787 L$ to $mL$ as follows:

$Volume=(0.90787 L)( 1000 mL 1 L)=907.87 mL$

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Answer 4

Question

Chapter 5, Problem 68E

(a)

Interpretation Introduction

Interpretation:Percent yield of $HSiCl3$ is to be calculated.

Concept introduction: The expression to determine number of moles is as follows:

$Number of moles=Given MassMolar mass$

The formula to calculate moles as per ideal gas law is as follows:

$n=PVRT$

Where,

$R$ is gas constant.

$V$ denotes the volume.

$n$ denotes number of moles.

$T$ denotes temperature.

$P$ denotes pressure.

(a)

Expert Solution

Answer to Problem 68E

Percent yield of $HSiCl3$ is $78.017 %$ .

Explanation of Solution

Given Information:

Density of $HSiCl3$ is $0.850 g/mL$ .

Pressure of $HCl$ is $10 atm$ .

Volume of $HCl$ is $15.0 L$ .

Temperature in Celsius is $35 °C$ .

The formula to convert degree Celsius to kelvin is as follows:

$T(K)=T(°C)+273 K$

Temperature in Celsius is $35 °C$ .

Substitute the value in the above formula.

$T(K)=T(°C)+273 K=35 °C+273 K=308 K$

The formula to calculate mass from density is as follows:

$Mass=(Volume)(Density)$

For $HSiCl3$

Volume is $156 mL$ .

Density is $1.34 g/mL$ .

Substitute the value in above formula.

$Mass=(Volume)(Density)=(156 mL)(1.34 g/mL)=209.04 g$

The expression to determine number of moles is as follows:

$Number of moles=Mass of HSiCl3Molar mass of HSiCl3$

Mass of $HSiCl3$ is $209.04 g$ .

Molar mass of $HSiCl3$ is $135.45 g/mol$ .

Substitute the value in above formula.

$Number of moles= Mass of HSiCl3 Molar mass of HSiCl3=209.04 g135.45 g/mol=1.3264 mol$

The balanced equation for formation of $HSiCl3$ is as follows:

$Si(s)+3HCl(g)→HSiCl3+H2(g)$

The formula to calculate moles as per ideal gas law is as follows:

$n=PVRT$

The value of $P$ is $10 atm$ .

The value of $V$ is $15.0 L$ .

The value of $T$ is $308 K$ .

The value of $R$ is $0.08206 L⋅atm/mol⋅K$ .

Substitute the value in above equation.

$n=PVRT=( 10 atm)( 15.0 L)( 0.08206 L⋅atm/mol⋅K)( 308 K)=5.9348 mol$

In accordance with balanced equation, $3 mol HCl$ forms $1 mol HSiCl3$ , thus moles of $HSiCl3$ formed from $5.9348 mol HCl$ is calculated as follows:

$Moles of HSiCl3=(5.9348 mol HCl)( 1 mol HSiCl 3 3 mol HCl)=1.9782 mol HSiCl3$

The formula to calculate mass from moles is given as follows:

$Mass=(Number of moles)(Molar mass)$

Number of moles is $1.9782 mol$ .

Molar mass is $135.45 g/mol$ .

Substitute the values in above formula.

$Mass=(Number of moles)(Molar mass)=(1.9782 mol)(135.45 g/mol)=267.94 g$

Thus, theoretical yield of $HSiCl3$ expected $267.94 g$ .

The formula to calculate percent yield is as follows:

$Percent yield=(Observed yieldTheoretical yield)(100 %)$

Observed yield is $209.04 g$ .

Theoretical yield is $267.94 g$ .

Substitute the value in above formula.

$Percent yield=( Observed yield Theoretical yield)(100 %)=( 209.04 g 267.94 g)(100 %)=78.017 %$

(b)

Interpretation Introduction

Interpretation:Volume of $SiH4$ when percent yield of $HSiCl3$ is $93.1 %$ isto be calculated.

Concept introduction: The expression to determine number of moles is as follows:

$Number of moles=Given MassMolar mass$

The formula to calculate moles as per ideal gas law is as follows:

$n=PVRT$

Where,

$R$ is gas constant.

$V$ denotes the volume.

$n$ denotes number of moles.

$T$ denotes temperature.

$P$ denotes pressure.

(b)

Expert Solution

Answer to Problem 68E

Volume of $SiH4$ is $907.87 mL$ .

Explanation of Solution

The formula to convert degree Celsius to kelvin is as follows:

$T(K)=T(°C)+273 K$

Temperature in Celsius is $35 °C$ .

Substitute the value in the above formula.

$T(K)=T(°C)+273 K=35 °C+273 K=308 K$

The formula to calculate mass from density is as follows:

$Mass=(Volume)(Density)$

For $HSiCl3$

Volume is $156 mL$ .

Density is $1.34 g/mL$ .

Substitute the value in above formula.

$Mass=(Volume)(Density)=(156 mL)(1.34 g/mL)=209.04 g$

The expression to determine number of moles is as follows:

$Number of moles=Mass of HSiCl3Molar mass of HSiCl3$

Mass of $HSiCl3$ is $209.04 g$ .

Molar mass of $HSiCl3$ is $135.45 g/mol$ .

Substitute the value in above formula.

$Number of moles= Mass of HSiCl3 Molar mass of HSiCl3=209.04 g135.45 g/mol=1.5433 mol$

The balanced equation for formation of $HSiCl3$ is as follows:

$4HSiCl3(l)→SiH4+3SiCl4(l)$

The formula to calculate moles as per ideal gas law is as follows:

$n=PVRT$

The value of $P$ is $10 atm$ .

The value of $V$ is $15.0 L$ .

The value of $T$ is $308 K$ .

The value of $R$ is $0.08206 L⋅atm/mol⋅K$ .

Substitute the value in above equation.

$n=PVRT=( 10 atm)( 15.0 L)( 0.08206 L⋅atm/mol⋅K)( 308 K)=5.9348 mol$

In accordance with balanced equation, $4 mol HSiCl3$ forms $1 mol SiH4$ , thus moles of $SiH4$ formed from $1.5433 mol HSiCl3$ is calculated as follows:

$Moles of SiH4=(1.5433 mol HSiCl3)( 1 mol SiH 4 4 mol HSiCl 3 )=0.385825 mol SiH4$

The formula to calculate mass from moles is given as follows:

$Mass=(Number of moles)(Molar mass)$

Number of moles is $0.385825 mol$ .

Molar mass is $32.12 g/mol$ .

Substitute the values in above formula.

$Mass=(0.385825 mol)(32.12 g/mol)=12.3929 g$

The formula to calculate percent yield is as follows:

$Percent yield=(Observed yieldTheoretical yield)(100 %)$

Percent yield is $93.1 %$ .

Theoretical yield is $12.3929 g$ .

Substitute the value in above formula.

$Percent yield=( Observed yield Theoretical yield)(100 %)93.1 %=( Observed yield 12.3929 g)(100 %)$

Rearrange to obtain the observed yield.

$Observed yield=( 93.1 % 100 %)(12.3929 g)=11.5377 g$

The formula to calculate volume as per ideal gas law is as follows:

$V=mRTMP$

The value of $P$ is $10 atm$ .

The value of $m$ is $11.5377 g$ .

The value of $M$ is $32.12 g/mol$ .

The value of $T$ is $308 K$ .

The value of $R$ is $0.08206 L⋅atm/mol⋅K$ .

Substitute the values in above equation.

$V=mRTMP=( 11.5377 g)( 0.08206 L⋅atm/mol⋅K)( 308 K)( 32.12 g/mol)( 10 atm)=0.90787 L$

The conversion factor to convert liters to milliliters is as follows:

$1 L=1000 mL$

Hence convert $0.90787 L$ to $mL$ as follows:

$Volume=(0.90787 L)( 1000 mL 1 L)=907.87 mL$

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Answer 5

Chapter 5, Problem 68E

(a)

Interpretation Introduction

Interpretation:Percent yield of $HSiCl3$ is to be calculated.

Concept introduction: The expression to determine number of moles is as follows:

$Number of moles=Given MassMolar mass$

The formula to calculate moles as per ideal gas law is as follows:

$n=PVRT$

Where,

$R$ is gas constant.

$V$ denotes the volume.

$n$ denotes number of moles.

$T$ denotes temperature.

$P$ denotes pressure.

(a)

Expert Solution

Answer to Problem 68E

Percent yield of $HSiCl3$ is $78.017 %$ .

Explanation of Solution

Given Information:

Density of $HSiCl3$ is $0.850 g/mL$ .

Pressure of $HCl$ is $10 atm$ .

Volume of $HCl$ is $15.0 L$ .

Temperature in Celsius is $35 °C$ .

The formula to convert degree Celsius to kelvin is as follows:

$T(K)=T(°C)+273 K$

Temperature in Celsius is $35 °C$ .

Substitute the value in the above formula.

$T(K)=T(°C)+273 K=35 °C+273 K=308 K$

The formula to calculate mass from density is as follows:

$Mass=(Volume)(Density)$

For $HSiCl3$

Volume is $156 mL$ .

Density is $1.34 g/mL$ .

Substitute the value in above formula.

$Mass=(Volume)(Density)=(156 mL)(1.34 g/mL)=209.04 g$

The expression to determine number of moles is as follows:

$Number of moles=Mass of HSiCl3Molar mass of HSiCl3$

Mass of $HSiCl3$ is $209.04 g$ .

Molar mass of $HSiCl3$ is $135.45 g/mol$ .

Substitute the value in above formula.

$Number of moles= Mass of HSiCl3 Molar mass of HSiCl3=209.04 g135.45 g/mol=1.3264 mol$

The balanced equation for formation of $HSiCl3$ is as follows:

$Si(s)+3HCl(g)→HSiCl3+H2(g)$

The formula to calculate moles as per ideal gas law is as follows:

$n=PVRT$

The value of $P$ is $10 atm$ .

The value of $V$ is $15.0 L$ .

The value of $T$ is $308 K$ .

The value of $R$ is $0.08206 L⋅atm/mol⋅K$ .

Substitute the value in above equation.

$n=PVRT=( 10 atm)( 15.0 L)( 0.08206 L⋅atm/mol⋅K)( 308 K)=5.9348 mol$

In accordance with balanced equation, $3 mol HCl$ forms $1 mol HSiCl3$ , thus moles of $HSiCl3$ formed from $5.9348 mol HCl$ is calculated as follows:

$Moles of HSiCl3=(5.9348 mol HCl)( 1 mol HSiCl 3 3 mol HCl)=1.9782 mol HSiCl3$

The formula to calculate mass from moles is given as follows:

$Mass=(Number of moles)(Molar mass)$

Number of moles is $1.9782 mol$ .

Molar mass is $135.45 g/mol$ .

Substitute the values in above formula.

$Mass=(Number of moles)(Molar mass)=(1.9782 mol)(135.45 g/mol)=267.94 g$

Thus, theoretical yield of $HSiCl3$ expected $267.94 g$ .

The formula to calculate percent yield is as follows:

$Percent yield=(Observed yieldTheoretical yield)(100 %)$

Observed yield is $209.04 g$ .

Theoretical yield is $267.94 g$ .

Substitute the value in above formula.

$Percent yield=( Observed yield Theoretical yield)(100 %)=( 209.04 g 267.94 g)(100 %)=78.017 %$

(b)

Interpretation Introduction

Interpretation:Volume of $SiH4$ when percent yield of $HSiCl3$ is $93.1 %$ isto be calculated.

Concept introduction: The expression to determine number of moles is as follows:

$Number of moles=Given MassMolar mass$

The formula to calculate moles as per ideal gas law is as follows:

$n=PVRT$

Where,

$R$ is gas constant.

$V$ denotes the volume.

$n$ denotes number of moles.

$T$ denotes temperature.

$P$ denotes pressure.

(b)

Expert Solution

Answer to Problem 68E

Volume of $SiH4$ is $907.87 mL$ .

Explanation of Solution

The formula to convert degree Celsius to kelvin is as follows:

$T(K)=T(°C)+273 K$

Temperature in Celsius is $35 °C$ .

Substitute the value in the above formula.

$T(K)=T(°C)+273 K=35 °C+273 K=308 K$

The formula to calculate mass from density is as follows:

$Mass=(Volume)(Density)$

For $HSiCl3$

Volume is $156 mL$ .

Density is $1.34 g/mL$ .

Substitute the value in above formula.

$Mass=(Volume)(Density)=(156 mL)(1.34 g/mL)=209.04 g$

The expression to determine number of moles is as follows:

$Number of moles=Mass of HSiCl3Molar mass of HSiCl3$

Mass of $HSiCl3$ is $209.04 g$ .

Molar mass of $HSiCl3$ is $135.45 g/mol$ .

Substitute the value in above formula.

$Number of moles= Mass of HSiCl3 Molar mass of HSiCl3=209.04 g135.45 g/mol=1.5433 mol$

The balanced equation for formation of $HSiCl3$ is as follows:

$4HSiCl3(l)→SiH4+3SiCl4(l)$

The formula to calculate moles as per ideal gas law is as follows:

$n=PVRT$

The value of $P$ is $10 atm$ .

The value of $V$ is $15.0 L$ .

The value of $T$ is $308 K$ .

The value of $R$ is $0.08206 L⋅atm/mol⋅K$ .

Substitute the value in above equation.

$n=PVRT=( 10 atm)( 15.0 L)( 0.08206 L⋅atm/mol⋅K)( 308 K)=5.9348 mol$

In accordance with balanced equation, $4 mol HSiCl3$ forms $1 mol SiH4$ , thus moles of $SiH4$ formed from $1.5433 mol HSiCl3$ is calculated as follows:

$Moles of SiH4=(1.5433 mol HSiCl3)( 1 mol SiH 4 4 mol HSiCl 3 )=0.385825 mol SiH4$

The formula to calculate mass from moles is given as follows:

$Mass=(Number of moles)(Molar mass)$

Number of moles is $0.385825 mol$ .

Molar mass is $32.12 g/mol$ .

Substitute the values in above formula.

$Mass=(0.385825 mol)(32.12 g/mol)=12.3929 g$

The formula to calculate percent yield is as follows:

$Percent yield=(Observed yieldTheoretical yield)(100 %)$

Percent yield is $93.1 %$ .

Theoretical yield is $12.3929 g$ .

Substitute the value in above formula.

$Percent yield=( Observed yield Theoretical yield)(100 %)93.1 %=( Observed yield 12.3929 g)(100 %)$

Rearrange to obtain the observed yield.

$Observed yield=( 93.1 % 100 %)(12.3929 g)=11.5377 g$

The formula to calculate volume as per ideal gas law is as follows:

$V=mRTMP$

The value of $P$ is $10 atm$ .

The value of $m$ is $11.5377 g$ .

The value of $M$ is $32.12 g/mol$ .

The value of $T$ is $308 K$ .

The value of $R$ is $0.08206 L⋅atm/mol⋅K$ .

Substitute the values in above equation.

$V=mRTMP=( 11.5377 g)( 0.08206 L⋅atm/mol⋅K)( 308 K)( 32.12 g/mol)( 10 atm)=0.90787 L$

The conversion factor to convert liters to milliliters is as follows:

$1 L=1000 mL$

Hence convert $0.90787 L$ to $mL$ as follows:

$Volume=(0.90787 L)( 1000 mL 1 L)=907.87 mL$

Answer 6

Chapter 5, Problem 68E

(a)

Interpretation Introduction

Interpretation:Percent yield of $HSiCl3$ is to be calculated.

Concept introduction: The expression to determine number of moles is as follows:

$Number of moles=Given MassMolar mass$

The formula to calculate moles as per ideal gas law is as follows:

$n=PVRT$

Where,

$R$ is gas constant.

$V$ denotes the volume.

$n$ denotes number of moles.

$T$ denotes temperature.

$P$ denotes pressure.

(a)

Expert Solution

Answer to Problem 68E

Percent yield of $HSiCl3$ is $78.017 %$ .

Explanation of Solution

Given Information:

Density of $HSiCl3$ is $0.850 g/mL$ .

Pressure of $HCl$ is $10 atm$ .

Volume of $HCl$ is $15.0 L$ .

Temperature in Celsius is $35 °C$ .

The formula to convert degree Celsius to kelvin is as follows:

$T(K)=T(°C)+273 K$

Temperature in Celsius is $35 °C$ .

Substitute the value in the above formula.

$T(K)=T(°C)+273 K=35 °C+273 K=308 K$

The formula to calculate mass from density is as follows:

$Mass=(Volume)(Density)$

For $HSiCl3$

Volume is $156 mL$ .

Density is $1.34 g/mL$ .

Substitute the value in above formula.

$Mass=(Volume)(Density)=(156 mL)(1.34 g/mL)=209.04 g$

The expression to determine number of moles is as follows:

$Number of moles=Mass of HSiCl3Molar mass of HSiCl3$

Mass of $HSiCl3$ is $209.04 g$ .

Molar mass of $HSiCl3$ is $135.45 g/mol$ .

Substitute the value in above formula.

$Number of moles= Mass of HSiCl3 Molar mass of HSiCl3=209.04 g135.45 g/mol=1.3264 mol$

The balanced equation for formation of $HSiCl3$ is as follows:

$Si(s)+3HCl(g)→HSiCl3+H2(g)$

The formula to calculate moles as per ideal gas law is as follows:

$n=PVRT$

The value of $P$ is $10 atm$ .

The value of $V$ is $15.0 L$ .

The value of $T$ is $308 K$ .

The value of $R$ is $0.08206 L⋅atm/mol⋅K$ .

Substitute the value in above equation.

$n=PVRT=( 10 atm)( 15.0 L)( 0.08206 L⋅atm/mol⋅K)( 308 K)=5.9348 mol$

In accordance with balanced equation, $3 mol HCl$ forms $1 mol HSiCl3$ , thus moles of $HSiCl3$ formed from $5.9348 mol HCl$ is calculated as follows:

$Moles of HSiCl3=(5.9348 mol HCl)( 1 mol HSiCl 3 3 mol HCl)=1.9782 mol HSiCl3$

The formula to calculate mass from moles is given as follows:

$Mass=(Number of moles)(Molar mass)$

Number of moles is $1.9782 mol$ .

Molar mass is $135.45 g/mol$ .

Substitute the values in above formula.

$Mass=(Number of moles)(Molar mass)=(1.9782 mol)(135.45 g/mol)=267.94 g$

Thus, theoretical yield of $HSiCl3$ expected $267.94 g$ .

The formula to calculate percent yield is as follows:

$Percent yield=(Observed yieldTheoretical yield)(100 %)$

Observed yield is $209.04 g$ .

Theoretical yield is $267.94 g$ .

Substitute the value in above formula.

$Percent yield=( Observed yield Theoretical yield)(100 %)=( 209.04 g 267.94 g)(100 %)=78.017 %$

Answer 7

Chapter 5, Problem 68E

(a)

Interpretation Introduction

Interpretation:Percent yield of $HSiCl3$ is to be calculated.

Concept introduction: The expression to determine number of moles is as follows:

$Number of moles=Given MassMolar mass$

The formula to calculate moles as per ideal gas law is as follows:

$n=PVRT$

Where,

$R$ is gas constant.

$V$ denotes the volume.

$n$ denotes number of moles.

$T$ denotes temperature.

$P$ denotes pressure.

Answer 8

(a)

Expert Solution

Answer to Problem 68E

Percent yield of $HSiCl3$ is $78.017 %$ .

Answer 9

(a)

Expert Solution

Answer 10

(a)

Expert Solution

Answer 11

Expert Solution

Answer 12

Explanation of Solution

Given Information:

Density of $HSiCl3$ is $0.850 g/mL$ .

Pressure of $HCl$ is $10 atm$ .

Volume of $HCl$ is $15.0 L$ .

Temperature in Celsius is $35 °C$ .

The formula to convert degree Celsius to kelvin is as follows:

$T(K)=T(°C)+273 K$

Temperature in Celsius is $35 °C$ .

Substitute the value in the above formula.

$T(K)=T(°C)+273 K=35 °C+273 K=308 K$

The formula to calculate mass from density is as follows:

$Mass=(Volume)(Density)$

For $HSiCl3$

Volume is $156 mL$ .

Density is $1.34 g/mL$ .

Substitute the value in above formula.

$Mass=(Volume)(Density)=(156 mL)(1.34 g/mL)=209.04 g$

The expression to determine number of moles is as follows:

$Number of moles=Mass of HSiCl3Molar mass of HSiCl3$

Mass of $HSiCl3$ is $209.04 g$ .

Molar mass of $HSiCl3$ is $135.45 g/mol$ .

Substitute the value in above formula.

$Number of moles= Mass of HSiCl3 Molar mass of HSiCl3=209.04 g135.45 g/mol=1.3264 mol$

The balanced equation for formation of $HSiCl3$ is as follows:

$Si(s)+3HCl(g)→HSiCl3+H2(g)$

The formula to calculate moles as per ideal gas law is as follows:

$n=PVRT$

The value of $P$ is $10 atm$ .

The value of $V$ is $15.0 L$ .

The value of $T$ is $308 K$ .

The value of $R$ is $0.08206 L⋅atm/mol⋅K$ .

Substitute the value in above equation.

$n=PVRT=( 10 atm)( 15.0 L)( 0.08206 L⋅atm/mol⋅K)( 308 K)=5.9348 mol$

In accordance with balanced equation, $3 mol HCl$ forms $1 mol HSiCl3$ , thus moles of $HSiCl3$ formed from $5.9348 mol HCl$ is calculated as follows:

$Moles of HSiCl3=(5.9348 mol HCl)( 1 mol HSiCl 3 3 mol HCl)=1.9782 mol HSiCl3$

The formula to calculate mass from moles is given as follows:

$Mass=(Number of moles)(Molar mass)$

Number of moles is $1.9782 mol$ .

Molar mass is $135.45 g/mol$ .

Substitute the values in above formula.

$Mass=(Number of moles)(Molar mass)=(1.9782 mol)(135.45 g/mol)=267.94 g$

Thus, theoretical yield of $HSiCl3$ expected $267.94 g$ .

The formula to calculate percent yield is as follows:

$Percent yield=(Observed yieldTheoretical yield)(100 %)$

Observed yield is $209.04 g$ .

Theoretical yield is $267.94 g$ .

Substitute the value in above formula.

$Percent yield=( Observed yield Theoretical yield)(100 %)=( 209.04 g 267.94 g)(100 %)=78.017 %$

Answer 13

(b)

Interpretation Introduction

Interpretation:Volume of $SiH4$ when percent yield of $HSiCl3$ is $93.1 %$ isto be calculated.

Concept introduction: The expression to determine number of moles is as follows:

$Number of moles=Given MassMolar mass$

The formula to calculate moles as per ideal gas law is as follows:

$n=PVRT$

Where,

$R$ is gas constant.

$V$ denotes the volume.

$n$ denotes number of moles.

$T$ denotes temperature.

$P$ denotes pressure.

(b)

Expert Solution

Answer to Problem 68E

Volume of $SiH4$ is $907.87 mL$ .

Explanation of Solution

The formula to convert degree Celsius to kelvin is as follows:

$T(K)=T(°C)+273 K$

Temperature in Celsius is $35 °C$ .

Substitute the value in the above formula.

$T(K)=T(°C)+273 K=35 °C+273 K=308 K$

The formula to calculate mass from density is as follows:

$Mass=(Volume)(Density)$

For $HSiCl3$

Volume is $156 mL$ .

Density is $1.34 g/mL$ .

Substitute the value in above formula.

$Mass=(Volume)(Density)=(156 mL)(1.34 g/mL)=209.04 g$

The expression to determine number of moles is as follows:

$Number of moles=Mass of HSiCl3Molar mass of HSiCl3$

Mass of $HSiCl3$ is $209.04 g$ .

Molar mass of $HSiCl3$ is $135.45 g/mol$ .

Substitute the value in above formula.

$Number of moles= Mass of HSiCl3 Molar mass of HSiCl3=209.04 g135.45 g/mol=1.5433 mol$

The balanced equation for formation of $HSiCl3$ is as follows:

$4HSiCl3(l)→SiH4+3SiCl4(l)$

The formula to calculate moles as per ideal gas law is as follows:

$n=PVRT$

The value of $P$ is $10 atm$ .

The value of $V$ is $15.0 L$ .

The value of $T$ is $308 K$ .

The value of $R$ is $0.08206 L⋅atm/mol⋅K$ .

Substitute the value in above equation.

$n=PVRT=( 10 atm)( 15.0 L)( 0.08206 L⋅atm/mol⋅K)( 308 K)=5.9348 mol$

In accordance with balanced equation, $4 mol HSiCl3$ forms $1 mol SiH4$ , thus moles of $SiH4$ formed from $1.5433 mol HSiCl3$ is calculated as follows:

$Moles of SiH4=(1.5433 mol HSiCl3)( 1 mol SiH 4 4 mol HSiCl 3 )=0.385825 mol SiH4$

The formula to calculate mass from moles is given as follows:

$Mass=(Number of moles)(Molar mass)$

Number of moles is $0.385825 mol$ .

Molar mass is $32.12 g/mol$ .

Substitute the values in above formula.

$Mass=(0.385825 mol)(32.12 g/mol)=12.3929 g$

The formula to calculate percent yield is as follows:

$Percent yield=(Observed yieldTheoretical yield)(100 %)$

Percent yield is $93.1 %$ .

Theoretical yield is $12.3929 g$ .

Substitute the value in above formula.

$Percent yield=( Observed yield Theoretical yield)(100 %)93.1 %=( Observed yield 12.3929 g)(100 %)$

Rearrange to obtain the observed yield.

$Observed yield=( 93.1 % 100 %)(12.3929 g)=11.5377 g$

The formula to calculate volume as per ideal gas law is as follows:

$V=mRTMP$

The value of $P$ is $10 atm$ .

The value of $m$ is $11.5377 g$ .

The value of $M$ is $32.12 g/mol$ .

The value of $T$ is $308 K$ .

The value of $R$ is $0.08206 L⋅atm/mol⋅K$ .

Substitute the values in above equation.

$V=mRTMP=( 11.5377 g)( 0.08206 L⋅atm/mol⋅K)( 308 K)( 32.12 g/mol)( 10 atm)=0.90787 L$

The conversion factor to convert liters to milliliters is as follows:

$1 L=1000 mL$

Hence convert $0.90787 L$ to $mL$ as follows:

$Volume=(0.90787 L)( 1000 mL 1 L)=907.87 mL$

Answer 14

(b)

Interpretation Introduction

Interpretation:Volume of $SiH4$ when percent yield of $HSiCl3$ is $93.1 %$ isto be calculated.

Concept introduction: The expression to determine number of moles is as follows:

$Number of moles=Given MassMolar mass$

The formula to calculate moles as per ideal gas law is as follows:

$n=PVRT$

Where,

$R$ is gas constant.

$V$ denotes the volume.

$n$ denotes number of moles.

$T$ denotes temperature.

$P$ denotes pressure.

Answer 15

(b)

Expert Solution

Answer to Problem 68E

Volume of $SiH4$ is $907.87 mL$ .

Answer 16

(b)

Expert Solution

Answer 17

(b)

Expert Solution

Answer 18

Expert Solution

Answer 19

Explanation of Solution

The formula to convert degree Celsius to kelvin is as follows:

$T(K)=T(°C)+273 K$

Temperature in Celsius is $35 °C$ .

Substitute the value in the above formula.

$T(K)=T(°C)+273 K=35 °C+273 K=308 K$

The formula to calculate mass from density is as follows:

$Mass=(Volume)(Density)$

For $HSiCl3$

Volume is $156 mL$ .

Density is $1.34 g/mL$ .

Substitute the value in above formula.

$Mass=(Volume)(Density)=(156 mL)(1.34 g/mL)=209.04 g$

The expression to determine number of moles is as follows:

$Number of moles=Mass of HSiCl3Molar mass of HSiCl3$

Mass of $HSiCl3$ is $209.04 g$ .

Molar mass of $HSiCl3$ is $135.45 g/mol$ .

Substitute the value in above formula.

$Number of moles= Mass of HSiCl3 Molar mass of HSiCl3=209.04 g135.45 g/mol=1.5433 mol$

The balanced equation for formation of $HSiCl3$ is as follows:

$4HSiCl3(l)→SiH4+3SiCl4(l)$

The formula to calculate moles as per ideal gas law is as follows:

$n=PVRT$

The value of $P$ is $10 atm$ .

The value of $V$ is $15.0 L$ .

The value of $T$ is $308 K$ .

The value of $R$ is $0.08206 L⋅atm/mol⋅K$ .

Substitute the value in above equation.

$n=PVRT=( 10 atm)( 15.0 L)( 0.08206 L⋅atm/mol⋅K)( 308 K)=5.9348 mol$

In accordance with balanced equation, $4 mol HSiCl3$ forms $1 mol SiH4$ , thus moles of $SiH4$ formed from $1.5433 mol HSiCl3$ is calculated as follows: