   Chapter 13, Problem 132AP ### Introductory Chemistry: A Foundati...

9th Edition
Steven S. Zumdahl + 1 other
ISBN: 9781337399425

#### Solutions

Chapter
Section ### Introductory Chemistry: A Foundati...

9th Edition
Steven S. Zumdahl + 1 other
ISBN: 9781337399425
Textbook Problem
1 views

# uppose two separate 1 00.0 − L tanks are to be filled, one with helium and one with hydrogen. What mass of each gas is needed to produce a pressure of 2 . 7 0 atm in its respective lank at 24  ° C ?

Interpretation Introduction

Interpretation:

To calculate the mass of gas in each tank with given conditions of pressure, volume and temperature.

Concept Introduction:

To calculate the mass of gases, we can apply the ideal gas equation which purposed the relation between moles, pressure, volume and temperature of ideal gas.

The ideal equation is: PV = nRT.

Explanation

Given information:

Pressure = 2.70 atm

Temperature = 24 °C = 273 + 24 = 297 K

Volume = 100.0 L

We have to apply ideal gas equation to calculate the moles of gases. Since the pressure, volume and temperature are same for both tanks so number of moles will be same for both gases. The mass of gas depends on the molar mass of gas hence the mass will be different for both the gases as the molar mass of different.

Plug the values in ideal gas equation;

PV = nRT

2.70 atm × 100.0 L = n × 0.0821 L.atm / K

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