4
Question
2 moles of an ideal gas expanded isothermally and reversibly from 1L to 10 L at 300 K. What is the enthalpy change?
2 moles of an ideal gas expanded isothermally and reversibly from 1L to 10 L at 300 K. What is the enthalpy change?
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Solution
The correct option is C -11.4 kJ
For an isothermal and reversible process
Work done =−pdv=−nRTlnV2V1
Given V1 = 1 L V2 = 10 L , T = 300 K
n = 2 moles
W = -11.4 kJ approximately
we know hat
dU+dW=dq
dU=0 for isothermal process
−∫pdv=∫dq
Work done =−pdv=−nRTlnV2V1
Given V1 = 1 L V2 = 10 L , T = 300 K
n = 2 moles
q=−11.4 kJ approximately
we know that
ΔH=−PΔV=work done=q
q=−11.4 kJ
For an isothermal and reversible process
Work done =−pdv=−nRTlnV2V1
Given V1 = 1 L V2 = 10 L , T = 300 K
n = 2 moles
W = -11.4 kJ approximately
we know hat
dU+dW=dq
dU=0 for isothermal process
−∫pdv=∫dq
Work done =−pdv=−nRTlnV2V1
Given V1 = 1 L V2 = 10 L , T = 300 K
n = 2 moles
q=−11.4 kJ approximately
we know that
ΔH=−PΔV=work done=q
q=−11.4 kJ
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