Question

Following method of extracting Zn is based on thermodynamics
A: \(2\text{ZnS} + 3\text{O}_2 \rightarrow 2\text{ZnO} + 2\text{SO}_2\)
B: \(\text{ZnO} + \text{C} \rightarrow \text{Zn} + \text{CO}\)
If \(\Delta G_f^{\circ}\) (standard free energies of formation, in kJ mol\(^{-1}\)) of ZnS = -205.4, ZnO = -318.0, SO\(_2\) = -300.4, and CO = -137.3. Free energy changes of the above reaction A and B (respectively) will be:

• A. -826.4 kJ, +180.9 kJ
• B. +826.4 kJ, -180.9 kJ
• C. -826.4 kJ, -180.9 kJ
• D. +826.4 kJ, +180.9 kJ

Hint:

Negative \(\Delta G\) = spontaneous. Reaction B is non-spontaneous at standard conditions.

Answer 1

The Correct Option is A