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5 mol of an ideal gas expands reversibly...

`5 mol` of an ideal gas expands reversibly from a volume of `8 dm^(3)` at a temperature of `27^(@)C`. Calculate the chngae in entropy.

A

`70.26 J K^(-1)`

B

`80.55 J K^(-1)`

C

`95.73 J K^(-1)`

D

`107.11 J K^(-1)`

Text Solution

Verified by Experts

Entropy change `(DeltaS) = 2.303 nRT "log"(V_(2))/(V_(1))`
`= 2.303 xx5xx 8.314 xx "log"(80)/(8)`
`= 95.73 J K^(-1)`
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5 mol of an ideal gas expand reversibly from a volume of 8 dm^(3) to 80 dm^(3) at an temperature of 27^(@)C . Calculate the change in entropy.

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Knowledge Check

  • Five moles of anideal gas expends reversily from a volume of 8dm^(3) at a temperature of 27^(@)C Calculate the change in entropy.

    A
    `70.26JK^(-1)`
    B
    `82.55JK^(-1)`
    C
    `95.73JK^(-1)`
    D
    `107.11JK^(-1)`

  • 5 mole of an ideal gas expands reversible from a volume of 8 dm^(3) to 80 dm^(3) at a temperature of 27^(@) C. Calculate the change in entropy.

    A
    `70.26 JK^(-1)`
    B
    `82.55 JK^(-1)`
    C
    `95.73 JK^(-1)`
    D
    `107.11 JK^(-1)`

  • 6 moles of an ideal gas expand isothermally and reversibly from a volume of 1 litre to a volume of 10 litres at 27^(@)C . What is the maximum work done

    A
    47 kJ
    B
    100 kJ
    C
    0
    D
    34.465 kJ

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