MyQuestionIcon

1

You visited us 1 times! Enjoying our articles? Unlock Full Access!

Work done in Isothermal Irreversible Process

Two moles of ...

Question

Two moles of an ideal gas is expanded isothermally and reversibly from 1 litre to 10 litre at 300 K. The enthalpy change ( in kJ) for the process is

A

11.4 kJ

No worries! We‘ve got your back. Try BYJU‘S free classes today!

B

−11.4 kJ

No worries! We‘ve got your back. Try BYJU‘S free classes today!

C

0 kJ

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses

D

4.8 kJ

No worries! We‘ve got your back. Try BYJU‘S free classes today!

Open in App

Solution

The correct option is C
0 kJ

$△ H = n C_{p} △ T s o l u t i o n; s i n c e △ T = 0$

so, $△ H = 0$

Suggest Corrections

thumbs-up

41

Similar questions

Q. Two moles of an ideal gas are expanded isothermally and reversibly from

1

10

300 K

. The enthalpy change (in

k J

) for the process is:

Q. Two moles of an ideal gas is expanded isothermally and reversibly from 1 litre to 10 litre at 300 K. The enthalpy change ( in kJ) for the process is

Q. Two moles of an ideal gas is expanded isothermally and reversibly from 1 litre to 10 litre at 300 K. The internal energy change (in kJ) for the process is

Q. Two moles of an ideal gas expended isothermally and reversibly from 1 litre to 10 litre at 300 K. The enthalpy change (in kJ) for the process is:

Q. Calculate entropy change when

10

moles of an ideal gas expands reversibly and isothermally from an initial volume of

10

100

300 K

View More

Join BYJU'S Learning Program

similar_icon

Related Videos

lock

First Law of Thermodynamics

CHEMISTRY

Watch in App

explore_more_icon

Explore more

Work done in Isothermal Irreversible Process

Standard XII Chemistry

Join BYJU'S Learning Program

CrossIcon