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In the reaction, A(s)+B(g) to C(g)+D(g),...

In the reaction, `A(s)+B(g) to C(g)+D(g),DeltaH=31kJ and DeltaS=+35J*K^(-1)`. State whether the reaction will be spontaneous at `100^(@)C and 1100^(@)C` or not? Consider `Delta H and DeltaS` are independent of temperature.

Text Solution

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We know, `DeltaG=DeltaH-TDeltaS`. Now at `100^(@)C`,
`DeltaG=DeltaH-TDeltaS=31xx10^(3)-(273+100)xx35=+17945J`
`therefore`AT `1100^(@)C,=31xx10^(3)-(273+1100)xx35=-17055J`
AT `100^(@)C,DeltaG` for the given reaction is positive, so the reaction will be non-spontaneous. on the contrary, at `1100^(@)C,DeltaG` for the given reaction is negative, so it will be spontaneous.
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