   # Measured at a pressure of 1.0 atm and 298 K, gas C has a density of 2.0 g/L. The density of gas D, measured at a pressure of 0.5 atm and 298 K, is 1.3 g/L. Which gas has the larger molar mass? (a) C (b) D (c) Neither. The molar masses are the same. ### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640

#### Solutions

Chapter
Section ### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640
Chapter 10.3, Problem 3RC
Textbook Problem
1 views

## Measured at a pressure of 1.0 atm and 298 K, gas C has a density of 2.0 g/L. The density of gas D, measured at a pressure of 0.5 atm and 298 K, is 1.3 g/L. Which gas has the larger molar mass? (a) C (b) D (c) Neither. The molar masses are the same.

Interpretation Introduction

Interpretation:

The gas with larger molar mass has to be determined under the given conditions.

Concept introduction:

If the density, temperature and pressure values are given then the molar mass of gas can be determined by using the equation,

MolarmassM=dRTPP=pressured=densityT=temperatureinKR=Gasconstant0.082057L.atm/K.mol

This density of gas is expressed in g/mol unit.

### Explanation of Solution

Given, conditions for the gas D is

PressureP=0.5atmTemperature=298KDensity=1.3g/L

Substituting the known quantities in the equation,

MolarmassM=dRTP=1.3g/L×(0.082057L.atm/K.mol×298K0.5atm)=63.57g/mol

Conditions for the gas C is,

PressureP=1

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