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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

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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Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter6: Thermochemistry
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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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