Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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A sample of nitrous oxide (N2O) gas at 298.15 K is heated to 373.15 K and also allowed to expand from 1.50 L to 2.75 L. What is the final pressure of this gas in atm if the original pressure was 725 mmHg?
Expert Solution
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Step 1
For the phase change of the ideal gas the temperature, pressure, and volume of the initial state and the final state are given by the following equation:
Where
P1 = initial pressure of gas = 725 mmHg
V1 = initial volume of gas = 1.50 L
T1 = initial temperature of gas = 298.15 K
P2 = final pressure of gas =?
V2 = final volume of gas = 2.75 L
T2 = final temperature of gas = 373.15 K
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Step 2
By rearranging the above equation, we get:
Let’s put the above values into this equation to get the final volume of the gas:
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