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5 mol of an ideal gas expand reversibly ...

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.

Text Solution

Verified by Experts

For isothermal reversible process `Delta S=2.303 "nR log" (V_(2))/(V_(1))=2.303xx5molxx8.314"J/mol K log"(80)/(8)=95.73JK^(-1)`
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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.

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Knowledge Check

  • 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)`

  • 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)`

  • Two moles of an ideal gas are allowed to expand from a volume of 10 dm^(3) to 2m^(3) at 300 K against a pressure of 101.325 kPa. Calculate the work done.

    A
    `-201.6` kJ
    B
    `13.22` kJ
    C
    `-810` J
    D
    `-18.96` kJ

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