The first step in the industrial recovery of zinc from the zinc sulfide ore is roasting, that is, the conversion of ZnS to ZnO by heating. 2 ZnS(s) + 3 O2(g) → 2 ZnO(s) + 2 SO2(g) ΔH = -879 kJ/mol

Question

Calculate the heat evolved (in kJ) per gram of ZnS roasted.

Answer 1

You have 879 kJ/mol and you have 2 mols in the equation so the reaction produces 2 x 879 kJ. How many grams ZnS are there are 2 moles?

Answer 2

-9.06KJ for 1 g

Answer 3

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