The molar heat capacities of gases are not perfectlyconstant, as we've assumed, but increase slowly withtemperature. An empirical formula for the molar heatcapacity at constant volume of nitrogen isCv = (20.6 - 1.6 × 10¯³T +8.0 × 10¯67²) J/mol K,where T is in K.What is the entropy increase of the gas if 5.0 g of nitrogen in a rigid container are slowly heated from 300°C to 500°C?Express your answer with the appropriate units.

Write the expression for the number of moles and substitute the corresponding values.

The molar heat capacities of gases are not perfectly constant, as we've assumed, but increase slowly with temperature. An empirical formula for the molar heat capacity at constant volume of nitrogen is Cv (20.6 -1.6 x 10-³T+8.0 x 10-67²) J/mol K, where T' is in K. What is the entropy increase of the gas if 5.0 g of nitrogen in a rigid container are slowly heated from 300°C to 500°C? Express your answer with the appropriate units.

The molar heat capacities of gases are not perfectly constant, as we've assumed, but increase slowly with temperature. An empirical formula for the molar heat capacity at constant volume of nitrogen is Cv (20.6 -1.6 x 10-³T+8.0 x 10-67²) J/mol K, where T' is in K. What is the entropy increase of the gas if 5.0 g of nitrogen in a rigid container are slowly heated from 300°C to 500°C? Express your answer with the appropriate units.

Principles of Physics: A Calculus-Based Text

5th Edition

ISBN:9781133104261

Author:Raymond A. Serway, John W. Jewett

Publisher:Raymond A. Serway, John W. Jewett

Chapter18: Heat Engines, Entropy, And The Second Law Of Thermodynamics

Section: Chapter Questions

Problem 36P

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