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.
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