951 mol of N2 gas is in a constant volume 235.6 L turbine at 25 °C. If 11.36 MJ of heat energy is added the gas will heat up to 600 °C. a. calculate CP,m= ΔH/ΔT/n. b. If we Google the heat capacity we find CP,m = 29.135 J/K/mol at room temperature. The result from pt. a is slightly higher! Can you explain the discrepancy?
951 mol of N2 gas is in a constant volume 235.6 L turbine at 25 °C. If 11.36 MJ of heat energy is added the gas will heat up to 600 °C. a. calculate CP,m= ΔH/ΔT/n. b. If we Google the heat capacity we find CP,m = 29.135 J/K/mol at room temperature. The result from pt. a is slightly higher! Can you explain the discrepancy?
Elements Of Electromagnetics
7th Edition
ISBN:9780190698614
Author:Sadiku, Matthew N. O.
Publisher:Sadiku, Matthew N. O.
ChapterMA: Math Assessment
Section: Chapter Questions
Problem 1.1MA
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Let’s say 951 mol of N2 gas is in a constant volume 235.6 L turbine at 25 °C. If 11.36 MJ of heat energy is added the gas will heat up to 600 °C.
a. calculate CP,m= ΔH/ΔT/n.
b. If we Google the heat capacity we find CP,m = 29.135 J/K/mol at room temperature. The result from pt. a is slightly higher! Can you explain the discrepancy?
Expert Solution
Step 1
Given:
No. of moles of N2, n = 951 mol
heat added , ΔH = 11.36 MJ
T1 = 25 °C
T2 = 600 °C
To find:
(a) CP,m
(b) reason for discrepancy
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