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Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
ISBN: 9781305079243

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BuyFindarrow_forward

Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
ISBN: 9781305079243
Textbook Problem

An unknown diatomic gas has a density of 3.164 g/L at STP. What is the identity of the gas?

Interpretation Introduction

Interpretation:

The diatomic gas having a density of 3.164 g/L at STP should be identified.

Concept introduction:

STP: standard temperature and pressure, it is the condition of 273.2K and 1 atm.

The molar volume of gases at STP condition is similar and it is close to the molar volume of an ideal gas at STP condition. That is, 22.42 L. Hence, at STP the molar volume of a gas is considered as 22.42L.

Equation for density is,

Density=MassVolume

According to ideal gas equation for molecular mass,

Molecularmass=Mass*R*TemperatureVolume*pressure

Explanation

Explanation

The given data’s of the gas are,

  • - Density = 3.164g/L
  • - Temperature = 273.2 K
  • - Pressure = 1 atm
  • - Universal gas constant ‘R’ = 0.08206 L atm

According to ideal gas equation for molecular mass,

Molecularmass=Density*R*Temperaturepressure

Therefore, the molecular mass of given diatomic gas is,

Molecularmassof given diatomic gas=3.164g/L*0.08206Latm/Kmol*273

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