1
Question
Three moles of an ideal gas initially at 27oC and 40 L volume are compressed isothermally and reversibly till the final volume of the gas is 10 L. Calculate q for the process.
Take:
log(0.25)=0.602
Three moles of an ideal gas initially at 27oC and 40 L volume are compressed isothermally and reversibly till the final volume of the gas is 10 L. Calculate q for the process.
Take:
log(0.25)=0.602
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Solution
The correct option is C −10.37 kJ
Work done in an isothermal reversible process is given as:
w=−2.303nRT(logV2V1)
Here, n=3 mol
T=27+273=300 K
V1=40 L, V2=10 atm
R=8.314 JK−1mol−1
Using the formula we get,
w=−2.303×3×8.314×300×log1040
w=10375 J
For isothermal process, △U=0 (as temperature is constant)
so, from first law
△U=q+w
q=−w=−10375 J
or
q=−10.37 kJ
Work done in an isothermal reversible process is given as:
w=−2.303nRT(logV2V1)
Here, n=3 mol
T=27+273=300 K
V1=40 L, V2=10 atm
R=8.314 JK−1mol−1
Using the formula we get,
w=−2.303×3×8.314×300×log1040
w=10375 J
For isothermal process, △U=0 (as temperature is constant)
so, from first law
△U=q+w
q=−w=−10375 J
or
q=−10.37 kJ
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