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
    
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