The values of Δ G are very important in metallurgy. The Δ G values for the following reactions at 1000 K are given as: (s) + 2(g) - 2(g); Δ G = -544 kJ; 2Zn(s) + (s) - 2ZnS(s); Δ G = -293 kJ; 2Zn(s)

Question

The values of Δ G are very important in metallurgy. The Δ G values for the following reactions at 1000 K are given as: $S_2$(s) + 2$O_2$(g) -> 2$SO_2$(g); Δ G = -544 kJ; 2Zn(s) + $S_2$(s) -> 2ZnS(s); Δ G = -293 kJ; 2Zn(s) + $O_2$(g) -> 2ZnO(s); Δ G = -480 kJ. The Δ G for the reaction: 2ZnS(s) + 3$O_2$(g) -> 2ZnO(s) + 2$SO_2$(g) will be

Prashant Kotian · Accepted Answer

Correct answer: B. We can get the desired reaction by: Reversing reaction (2): 2ZnS -> 2Zn + ; Δ G = +293 kJ. Adding reaction (3): 2Zn + -> 2ZnO; Δ G = -480 kJ. Adding reaction (1): + 2 -> 2; Δ G = -544 kJ. Summing gives 2ZnS + 3 -> 2ZnO + 2. Total Δ G = +293 - 480 - 544 = -731 kJ.

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