Chemistry for Engineering Students
Chemistry for Engineering Students
4th Edition
ISBN: 9781337398909
Author: Lawrence S. Brown, Tom Holme
Publisher: Cengage Learning
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Chapter 5, Problem 5.29PAE

5.29 What are the densities of the following gases at STP?

(a) CF2Cl2, (b)CO2, (c) HCl

Expert Solution & Answer
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Interpretation Introduction

Interpretation:

The densities of the following gases at STP have to be calculated.

Concept Introduction:

  • An ideal gas has is a hypothetical gas that is formed by a few molecules so that, its density is low, and the intermolecular forces are null. The model of gas facilitates mathematical calculations to study gases.
  • The molar mass is mass expressed in grams of a mol of substance. The molar mass can be expressed is the following way,

M=niAi

Where ni are the atoms number of element i that form the gas molecule gas and Ai is the atomic weight of element i.

  • The ideal gas law can be expressed in the following way,

P x V= n x R x TP x V= mM x R x TP = mV x R x TMP=δ x R x TM

Where P is the gas pressure (atm), V is the gas volume (L), T is the gas absolute temperature (K), n is the moles number of the gas , R is the ideal gas constant ( R=0.082 atm LK mol ), m is the mass (g) of the gas, ࢐ is the density of the gas and M (g/mol) is the molar mass of the gas.

In the STP conditions, the temperature is 273 K and the pressure is 1 atm.

Answer to Problem 5.29PAE

Solution: a) δCF2Cl2=5.4 gL

b) δCO2=1.96 gL

c) δHCl=1.63 gL

Explanation of Solution

Given Information:

The following gases,a) CF2Cl2b) CO2c) HCl

a)

1-Calculate the molar mass (M) of CF2Cl2,M= 1 x 12 gmol+2 x 19gmol + 2 x 35.5 gmol=121 gmol

2-Calculate the density of CF2Cl2 at STP1 atm  = δ CF2 Cl20.082 atm L K molx 273 K121 g mol1 atm x 121 gmol=δ CF2 Cl2 x 0.082atm LK molx 273 Kδ CF2 Cl2=1 atm x ;121 g m o l 0.082 a t m L K ; m o l x 273 K=5.4 gL

b)

1-Calculate the molar mass (M) of CO2,M= 1 x 12 gmol+2 x 16gmol = 44 gmol

2-Calculate the density of CF2Cl2 at STP1 atm  = δ CO20.082 atm L K molx 273 K44 g mol1 atm x 44 gmol=δ CO2 x 0.082atm LK molx 273 Kδ CO2=1 atm x 44 g m o l 0.082 a t m L K ; m o l x 273 K=1.96 gL

c)

1-Calculate the molar mass (M) of HCl,M= 1 x 1 gmol+1 x 35.5gmol = 36.5 gmol

2-Calculate the density of CF2Cl2 at STP1 atm  = δHCl0.082 atm L K molx 273 K36.5 g mol1 atm x 36.5 gmol=δHCl x 0.082atm LK molx 273 KδHCl=1 atm x 36.5 g m o l 0.082 a t m L K ; m o l x 273 K=1.63 gL

Conclusion

a) The density of CF2Cl2at STP is 5.4 gL.

b) The density of CO2at STP is 1.96 gL.

c) The density of HCl at STP is 1.63 gL.

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Chapter 5 Solutions

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