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4) A sample consisting of 2.00 mol of an ideal gas initially at P 111.0 kPa and T1 277.0 K is heated reversibly to 356.0 K at constant volume. The molar heat capacity at constant volume of the gas is Cy : (5/2) R. Calculate the final pressure, the change in internal energy AU of the gas, and the heat q and work w exchanged between the gas and its surroundings for the process.

4) A sample consisting of 2.00 mol of an ideal gas initially at P 111.0 kPa and T1 277.0 K is heated reversibly to 356.0 K at constant volume. The molar heat capacity at constant volume of the gas is Cy : (5/2) R. Calculate the final pressure, the change in internal energy AU of the gas, and the heat q and work w exchanged between the gas and its surroundings for the process.

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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4) A sample consisting of 2.00 mol of an ideal gas initially at P 111.0 kPa and T1 277.0 K is heated reversibly to 356.0 K at constant volume. The molar heat capacity at constant volume of the gas is Cy : (5/2) R. Calculate the final pressure, the change in internal energy AU of the gas, and the heat q and work w exchanged between the gas and its surroundings for the process.
Transcribed Image Text:4) A sample consisting of 2.00 mol of an ideal gas initially at P 111.0 kPa and T1 277.0 K is heated reversibly to 356.0 K at constant volume. The molar heat capacity at constant volume of the gas is Cy : (5/2) R. Calculate the final pressure, the change in internal energy AU of the gas, and the heat q and work w exchanged between the gas and its surroundings for the process.
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