A 2.0-{\ m mol} sample of ideal gas with molar specific heat C_V = {\\textstyle{

Question

A 2.0-{ m mol} sample of ideal gas with molar specific heat C_V = { extstyle{5 over 2}},R is initially at 320 K and 100 { m kPa} pressure.
Part A
Determine the final temperature when 1.7 { m kJ} of heat are added to the gas isothermally.
Express your answer using two significant figures.
ANSWER:
T_f =


{ m K}
Part B
Determine the work done by the gas when 1.7 { m kJ} of heat are added to the gas isothermally.
Express your answer using two significant figures.
ANSWER:
W =


{ m kJ}
Part C
Determine the final temperature when 1.7 { m kJ} of heat are added to the gas at constant volume.
Express your answer using two significant figures.
ANSWER:
T_f =


{ m K}
Part D
Determine the work done by the gas when 1.7 { m kJ} of heat are added to the gas at constant volume.
Express your answer using two significant figures.
ANSWER:
W =


{ m J}
Part E
Determine the final temperature when 1.7 { m kJ} of heat are added to the gas isobarically.
Express your answer using two significant figures.
ANSWER:
T_f =


{ m K}
Part F
Determine the work done by the gas when 1.7 { m kJ} of heat are added to the gas isobarically.
Express your answer using two significant figures.
ANSWER:
W =


{ m J}

Explanation / Answer

part A
as the gas underwent isothermal there is no difference in temperature

final temperature=320K

part B

given T=0,

H=U+W,U=0 since isothermal process

W=H

=1.7 KJ

PART c

V=0,HENCE W=0

nCvdT=1.7

===>dT=1.7/5

=0.34 KJ

PART D

FOR constant volume process

work done is zero

part F

For isobaric process w=H-nCvdT

===>W=1.7-5*dT

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