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InterviewSolution
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For the reaction, `2A(g)+B(g) rarr 2D(g)` `DeltaU^(Θ)=-10.5 kJ` and `DeltaS^(Θ)=-44.1 JK^(-1)` Calculate `DeltaG^(Θ)` for the reaction, and predict whether the reaction may occur spontaneously. |
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Answer» Correct Answer - `0.164 kJ,` the reaction is not spontaneous. For the given reaction , `2A_((g))+B_((g))rarr2D_((g))` `Deltan_(g)=2-(3)` 1-mole Substituting the value of `Delta^(theta)` in the expression of `DeltaH:` `DeltaH^(theta)=DeltaU^(theta)+Deltan_(g)RT` `=(-10.5 kJ)-(-1)(8.314xx10^(-3)kJ K^(-1)"mol"^(-1))(298 K)` `=-10.5kJ-2.48 kJ` `DeltaH^(theta)=-12.98 kJ` Subtituting the value of `DeltaH^(theta) and DeltaS^(theta)` in the expression of `DeltaG^(theta):` `DeltaG^(theta)=DeltaH^(theta)-TDeltaS^(theta)` `=-12.98 kJ -(298 K)(-44.1 j K^(-1))` `=-12.98 kJ +13.14 kJ` `DeltaG^(theta)=+0.16 kJ` Since `DeltaG^(theta)` for the reaction is positive, the reaction will not occur spontaneously. |
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