6. Chemical Quantities & Aqueous Reactions
Redox Reactions
6. Chemical Quantities & Aqueous Reactions Redox Reactions
103PRACTICE PROBLEM
Iron can reduce sulfuric acid to produce solid sulfur. It can also reduce sulfuric acid to produce sulfur dioxide:
(i) 3 Fe(s) + SO42−(aq) + 8 H+(aq) → S(s) + 4 H2O(l) + 3 Fe2+(aq) E° = 0.49 V
(ii) Fe(s) + SO42−(aq) + 4 H+(aq) → SO2(g) + 2 H2O(l) + Fe2+(aq) E° = 0.28 V
What is the potential for reaction (i) if there are 0.15 M Fe2+ and 0.20 M H2SO4? What is the potential for reaction (ii) if there are 0.15 M Fe2+, 0.20 M H2SO4, and 1.0 atm SO2 gas? Which of the two reactions has a greater thermodynamic tendency if the concentration of H2SO4 is 0.15 M? (Assume that H2SO4 fully dissociates.)
Iron can reduce sulfuric acid to produce solid sulfur. It can also reduce sulfuric acid to produce sulfur dioxide:
(i) 3 Fe(s) + SO42−(aq) + 8 H+(aq) → S(s) + 4 H2O(l) + 3 Fe2+(aq) E° = 0.49 V
(ii) Fe(s) + SO42−(aq) + 4 H+(aq) → SO2(g) + 2 H2O(l) + Fe2+(aq) E° = 0.28 V
What is the potential for reaction (i) if there are 0.15 M Fe2+ and 0.20 M H2SO4? What is the potential for reaction (ii) if there are 0.15 M Fe2+, 0.20 M H2SO4, and 1.0 atm SO2 gas? Which of the two reactions has a greater thermodynamic tendency if the concentration of H2SO4 is 0.15 M? (Assume that H2SO4 fully dissociates.)