The entropy change involved in the isothermal reversible expansion of 2 moles of an ideal gas from a volume of `10 dm^(3)` to a volume of `100dm^(3)` at `27^(@)C` isA. `38.3 J mol^(-1) K^(-1)`B. `35.8 J mol^(-1) K^(-1)`C. `32.3 J mol^(-1) K^(-1)`D. `42.3 J mol^(-1) K^(-1)`

The entropy change involved in the isothermal reversible expansion of

1.	The entropy change involved in the isothermal reversible expansion of 2 moles of an ideal gas from a volume of `10 dm^(3)` to a volume of `100dm^(3)` at `27^(@)C` isA. `38.3 J mol^(-1) K^(-1)`B. `35.8 J mol^(-1) K^(-1)`C. `32.3 J mol^(-1) K^(-1)`D. `42.3 J mol^(-1) K^(-1)`
Answer» Correct Answer - a Entropy change for an isothermal process is `DeltaS=2.303R log((V_(2))/(V_(1)))` `DeltaS=2.303xx2xx8.314xxlog(100/10)` `=38.294 J mol^(-1) K^(-1)`

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The entropy change involved in the isothermal reversible expansion of 2 moles of an ideal gas from a volume of `10 dm^(3)` to a volume of `100dm^(3)` at `27^(@)C` isA. `38.3 J mol^(-1) K^(-1)`B. `35.8 J mol^(-1) K^(-1)`C. `32.3 J mol^(-1) K^(-1)`D. `42.3 J mol^(-1) K^(-1)`

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