Using the equation for Cp as a function of T for CH4(g), calculate the entropy change (J/K), which results from heating 2 moles of the gas from 300 K to 600 K at constant pressure. Cp = 3.422 + 17.845x10-3 T – 41.65x10-7 T2 cal/mol-K Assuming that for CH4, Cp – Cv = R, find the entropy change (J/K) resulting from heating 2 moles of the gas from 300 K to 600 K at constant volume.
Using the equation for Cp as a function of T for CH4(g), calculate the entropy change (J/K), which results from heating 2 moles of the gas from 300 K to 600 K at constant pressure. Cp = 3.422 + 17.845x10-3 T – 41.65x10-7 T2 cal/mol-K Assuming that for CH4, Cp – Cv = R, find the entropy change (J/K) resulting from heating 2 moles of the gas from 300 K to 600 K at constant volume.
Introduction to Chemical Engineering Thermodynamics
8th Edition
ISBN:9781259696527
Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Chapter1: Introduction
Section: Chapter Questions
Problem 1.1P
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Using the equation for Cp as a function of T for CH4(g), calculate the entropy change (J/K), which results from heating 2 moles of the gas from 300 K to 600 K at constant pressure.
Cp = 3.422 + 17.845x10-3 T – 41.65x10-7 T2 cal/mol-K
Assuming that for CH4, Cp – Cv = R, find the entropy change (J/K) resulting from heating 2 moles of the gas from 300 K to 600 K at constant volume.
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