MyQuestionIcon

2

You visited us 2 times! Enjoying our articles? Unlock Full Access!

Heat of Reaction

Two moles of ...

Question

Two moles of an ideal gas is expanded isothermally and reversibly from 1 litre to 10 litre at 300K. 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

Temperature remains constant, so enthalpy change for an isothermal process is equal to zero.

Suggest Corrections

thumbs-up

7

Similar questions

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 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 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

Thermochemistry

CHEMISTRY

Watch in App

explore_more_icon

Explore more

Heat of Reaction

Standard XII Chemistry

Join BYJU'S Learning Program

CrossIcon