The first step in the industrial recovery of zinc from zinc sulfide ore is roasting. That is the conversion of ZnS to ZnO by heating: kJ 2ZnS(s) + 302(g) → 2ZnO(s) + 2 SO2 (g) AH=-879 mol Calculate the heat (in kJ) associated with roasting 3.00 grams of zinc sulfide. Be sure your answer has the correct number of significant digits. ☐ kJ x10

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The first step in the industrial recovery of zinc from zinc sulfide ore is roasting. That is the conversion of ZnS to ZnO by heating:
kJ
2ZnS(s) + 302(g) → 2ZnO(s) + 2 SO2 (g) AH=-879
mol
Calculate the heat (in kJ) associated with roasting 3.00 grams of zinc sulfide. Be sure your answer has the correct number of significant digits.
☐ kJ
x10
Transcribed Image Text:The first step in the industrial recovery of zinc from zinc sulfide ore is roasting. That is the conversion of ZnS to ZnO by heating: kJ 2ZnS(s) + 302(g) → 2ZnO(s) + 2 SO2 (g) AH=-879 mol Calculate the heat (in kJ) associated with roasting 3.00 grams of zinc sulfide. Be sure your answer has the correct number of significant digits. ☐ kJ x10
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