Chapter 9, Problem 9.115CHP

(a)

Interpretation Introduction

Interpretation:

The number of moles present in the gas has to be calculated.

Concept Introduction:

Ideal gas equation is an equation that is describing the state of an imaginary ideal gas.

$\text{PV}\text{=}\text{n RT}$

Where,

P is the pressure of the gas

V is the volume

n is the number of moles of gas

R is the universal gas constant $\text{(R=0}{\text{.0821LatmK}}^{\text{-1}}{\text{mol}}^{\text{-1}})$

T is the temperature

(b)

Interpretation Introduction

Interpretation:

The number of moles of $\text{B}$ present in the gas has to be calculated.

Concept Introduction:

Ideal gas equation is an equation that is describing the state of an imaginary ideal gas.

$\text{PV}\text{=}\text{n RT}$

Where,

P is the pressure of the gas

V is the volume

n is the number of moles of gas

R is the universal gas constant $\text{(R=0}{\text{.0821LatmK}}^{\text{-1}}{\text{mol}}^{\text{-1}})$

T is the temperature

(c)

Interpretation Introduction

Interpretation:

The density of $\text{B}$ gas has to be calculated.

Concept Introduction:

Density = an amount of substance per unit volume is known as density.

$\begin{array}{l}\text{ ρ = }\frac{\text{M}}{\text{V}}\\ \text{Where,}\\ \text{ρ=density}\\ \text{M=mass}\\ \text{V=Volume}\end{array}$

(d)

Interpretation Introduction

Interpretation:

The molecular weight of $\text{B}$ collected and its formula have to be calculated.

Concept Introduction:

Molecular mass:

It is a physical property, which is defined as the mass of a given substance divided by the amount of substance. Unit of the molecular mass is $\text{Kg/mol}$

$\text{molecular}\text{mass}\text{=}\frac{\text{amount}\text{of}\text{mass}}{\text{molar}\text{mass}}$

(e)

Interpretation Introduction

Interpretation:

The balanced equation for the reaction of $\text{mercury}\left(\text{I}\right)\text{carbonate with nitric acid}$ has to be written.

Concept Introduction:

Balancing equations:

In a reaction, the number of molecules before and after the reaction should be equal. That means the number of moles of particular compound on either side of the reaction should be equal, this can be done by multiplication with the number of molecules required to make them equal in a reaction.