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MHT CET · Chemistry · Thermodynamics (C)

Calculate Gibbs energy change for a reaction having \(\Delta \mathrm{H}=31400 \mathrm{~J}, \Delta \mathrm{~S}=32 \mathrm{JK}^{-1}\) at \(1000^{\circ} \mathrm{C}\) ?

  1. A -4668 J
  2. B -9336 J
  3. C -4073 J
  4. D -2334 J
Verified Solution

Answer & Solution

Correct Answer

(B) -9336 J

Step-by-step Solution

Detailed explanation

\(\begin{aligned}
& \mathrm{T}=1000^{\circ} \mathrm{C}=1273 \mathrm{~K} \\
& \Delta \dot{G}=\Delta \mathrm{H}-\mathrm{T} \Delta \mathrm{~S} \\
& =31400 \mathrm{~J}-1273 \mathrm{~K}\left(32 \mathrm{~J} \mathrm{~K}^{-1}\right) \\
& =3.1400 \mathrm{~J}-40736 \mathrm{~J} \\
& \Delta \mathrm{G}=-9336 \mathrm{~J}
\end{aligned}\)