Which of the following relationship is incorrect?

\frac{Δ H - Δ E}{Δ n T} =

constant

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Δ G = Δ H - T Δ S

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q = Δ U + W

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Δ G^{o} = - R T l n K

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Solution

The correct option is C $q = Δ U + W$
The First Law of Thermodynamics states that energy can be converted from one form to another with the interaction of heat, work and internal energy, but it cannot be created nor destroyed, under any circumstances.
Mathematically, this is represented as:
$Δ U = q + W$
$q = W - Δ U$
So, statement C is wrong.
Hence option C is correct.

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