A gaseous system contains $ H_1 $, $ H_2 $, and $ I_2 $ which participate in the gas phase reaction: \[ 2H_1 \rightleftharpoons H_2 + I_2 \] At a state of reaction equilibrium, the number of thermodynamic degrees of freedom is:

Question

For reaction $A \rightleftharpoons B$, $\Delta G^{\circ} = 105 - 35 \log T$. Find the transition temperature (in $^{\circ} C$) of the above reaction at 1 bar.

Answer 1

Step 1: Apply the Gibbs phase rule.
The number of degrees of freedom at equilibrium is determined by the Gibbs phase rule:\[F = C - P + 2\]Here, $ C $ represents the number of components and $ P $ represents the number of phases. For the given system, $ C = 3 $ and $ P = 1 $, resulting in:\[F = 3 - 1 + 2 = 4\]

Step 2: Final result.
Consequently, the correct count of thermodynamic degrees of freedom is (B) 4.

A gaseous system contains \( H_1 \), \( H_2 \), and \( I_2 \) which participate in the gas phase reaction: \[ 2H_1 \rightleftharpoons H_2 + I_2 \] At a state of reaction equilibrium, the number of thermodynamic degrees of freedom is:

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The Correct Option is B

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