Asked by Tanisha

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

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

Answers

Answered by DrBob222
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?
Answered by fide
-9.06KJ for 1 g
Answered by Berhanu Mamo
Thank You

Related Questions