Home
Class 11
CHEMISTRY
Two mole of an ideal gas is expanded irr...

Two mole of an ideal gas is expanded irreversibly and isothermally at `37^(@)C` until its volume is doubled and 3.41 kJ heat is absorbed from surroundings. `Delta S_("total")` (system + surroundings) is

A

`-0.52J//K`

B

`0.52J//K`

C

`22.52J//K`

D

0

Text Solution

Verified by Experts

The correct Answer is:
B
`DeltaS_("system")="nR ln"(V_(2))/(V_(1))`
`=2xxRxx"ln 2"`
= 11.52 J/K
`DeltaS_("surrounding")=-(3.41xx1000)/(310)`
`=-11J//K`
`DeltaS_("total")=+11.52-11`
`=+0.52J//K`
Promotional Banner

Topper's Solved these Questions

  • THERMODYNAMICS

    NARENDRA AWASTHI|Exercise Level 1 (Q.1 To Q.30)|6 Videos

  • THERMODYNAMICS

    NARENDRA AWASTHI|Exercise Level 1 (Q.31 To Q.60)|2 Videos

  • STOICHIOMETRY

    NARENDRA AWASTHI|Exercise Level 3 - Subjective Problems|20 Videos

Similar Questions

Explore conceptually related problems

Find the work done by a gas when it expands isothermally at 37^@C to four times its initial volume

One mole of ideal gas expands isothermally to double its volume at 27^(@)C . Then the work done by the gas is nearly

Two litres of an ideal gas at a pressure of 10 atm expands isothermally into a vacuum until its total volume is 20 litres. How much heat is absorbed and how much work is done in the expansion?

0.14kg of nitrogen at 300K is expanded isothermally and reversibly until its volume becomes doubled. Calculate the work done by the gas.

One mole of an ideal gas undergoes an isothermal change at temperature "T" so that its volume v is doubled. R is the molar gas constant. Work done by the gas during this change is

2 mole of an ideal gas at 27^(@)C expands isothermally and reversibly from a volume of 4 litre to 40 litre. The work done (in kJ) by the gas is