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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: 2ZnS (s) + 30₂(g) → 2ZnO(s) + 2SO₂ (g) kJ mol Calculate the heat (in kJ) associated with roasting 2.00 grams of zinc sulfide. Be sure your answer has the correct number of significant digits. kJ 0x10 ΔΗ= - 879

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: 2ZnS (s) + 30₂(g) → 2ZnO(s) + 2SO₂ (g) kJ mol Calculate the heat (in kJ) associated with roasting 2.00 grams of zinc sulfide. Be sure your answer has the correct number of significant digits. kJ 0x10 ΔΗ= - 879

Introductory Chemistry: A Foundation
Introductory Chemistry: A Foundation
9th Edition
ISBN:9781337399425
Author:Steven S. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Donald J. DeCoste
Chapter10: Energy
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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: 2 ZnS (s) + 30₂(g) → 2ZnO(s) + 2SO₂ (g) kJ mol Calculate the heat (in kJ) associated with roasting 2.00 grams of zinc sulfide. Be sure your answer has the correct number of significant digits. kJ 0x10 X ΔΗ= - 879
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: 2 ZnS (s) + 30₂(g) → 2ZnO(s) + 2SO₂ (g) kJ mol Calculate the heat (in kJ) associated with roasting 2.00 grams of zinc sulfide. Be sure your answer has the correct number of significant digits. kJ 0x10 X ΔΗ= - 879
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