   Chapter 13, Problem 135AP ### 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
3 views

# f 3 . 2 0  g of nitrogen gas occupies a volume of 1 . 71 L at 0   ° C and a pressure of 1 . 5 0 atm, what would the volume become if 8 . 8 0  g of nitrogen gas were added at constant conditions of temperature and pressure?

Interpretation Introduction

Interpretation:

To calculate the new volume when 8.80 g of nitrogen gas is added at constant temperature and pressure.

Concept Introduction:

The ideal gas equation is;

PV = nRT

• P = pressure.
• T = temperature.
• V = volume.
• R = gas constant = 0.0821 L. atm / K. mole.
• n = number of moles.
• Hence, at constant pressure and temperature, the volume has direct relation with number of moles of gas. The mathematical expression can be written as;

V1n1=V2n2

Explanation

Given information:

Volume of nitrogen gas = V1 = 1.71 L

Mass of nitrogen gas = 3.20 g

At constant pressure and temperature, the volume of gas has direct relation with number of moles of gas.

When 8.80 g of nitrogen gas is added, the mass of gas increases; which also increases the number of moles of gas. As the moles of gas increases, volume of gas also increases at constant temperature and pressure.

Number of moles of nitrogen gas = n1 = 3.20 g28.0 g/mol = 0.114 mole

Number of moles of nitrogen gas on addition of 8.80 g of gas =

n2 = 3.20 +8.80 g28.0 g/mol= 0

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