3. Use the following balanced oxidation-reduction equation for questions A and B. K2Cr2O7 3 H2S + 4 H2SO4 A. The oxidizing agent is a. K2Cr2O7 B. The substance oxidized → K2SO4 + Cr2(SO4)3 + 3 S + 7 H₂O b. H₂S c. H2SO4 a. K2Cr2O7 b. H₂S 4. In the reaction C6H1006 + 602 a. increases by 2 c. decreases by 2 c. H2SO4 d. S d. S → 6 CO4 + 5 H2O the oxidation number of C b. increases by 4 d. decreases by 4
3. Use the following balanced oxidation-reduction equation for questions A and B. K2Cr2O7 3 H2S + 4 H2SO4 A. The oxidizing agent is a. K2Cr2O7 B. The substance oxidized → K2SO4 + Cr2(SO4)3 + 3 S + 7 H₂O b. H₂S c. H2SO4 a. K2Cr2O7 b. H₂S 4. In the reaction C6H1006 + 602 a. increases by 2 c. decreases by 2 c. H2SO4 d. S d. S → 6 CO4 + 5 H2O the oxidation number of C b. increases by 4 d. decreases by 4
World of Chemistry, 3rd edition
3rd Edition
ISBN:9781133109655
Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste
Chapter18: Oxidation–reduction Reactions And Electrochemistry
Section: Chapter Questions
Problem 46A
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