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Balance redox reactions using the half-reaction method. Balance the redox reaction below using the half-reaction method. Ir³+ (aq) + Co(s) Ir(s) + Co²+ (aq) (a) To show your method, write the balanced half reactions below. Use the smallest integer coefficients possible and show electrons as e. If a box is not needed, leave it blank. (Coefficients of 1 are not needed). Oxidation half-reaction: + Reduction half-reaction: + - Ir³+ (aq) + + (b) To show your balanced equation, enter an integer in each of the boxes. If the integer is "1," do enter it. even though you would normally not show that in the equation. Use the smallest integer coefficients possible. Co(s)→ + Ir(s) + Co2+ (aq)

Balance redox reactions using the half-reaction method. Balance the redox reaction below using the half-reaction method. Ir³+ (aq) + Co(s) Ir(s) + Co²+ (aq) (a) To show your method, write the balanced half reactions below. Use the smallest integer coefficients possible and show electrons as e. If a box is not needed, leave it blank. (Coefficients of 1 are not needed). Oxidation half-reaction: + Reduction half-reaction: + - Ir³+ (aq) + + (b) To show your balanced equation, enter an integer in each of the boxes. If the integer is "1," do enter it. even though you would normally not show that in the equation. Use the smallest integer coefficients possible. Co(s)→ + Ir(s) + Co2+ (aq)

Chemistry: The Molecular Science
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter17: Electrochemistry And Its Applications
Section17.5: Using Standard Half-cell Potentials
Problem 17.9CE
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Balance redox reactions using the half-reaction method. Balance the redox reaction below using the half-reaction method. Ir³+ (aq) + Co(s) Ir(s) + Co²+ (aq) (a) To show your method, write the balanced half reactions below. Use the smallest integer coefficients possible and show electrons as e. If a box is not needed, leave it blank. (Coefficients of 1 are not needed). Oxidation half-reaction: + Reduction half-reaction: + - Ir³+ (aq) + → + (b) To show your balanced equation, enter an integer in each of the boxes. If the integer is "1," do enter it even though you would normally not show that in the equation. Use the smallest integer coefficients possible. Co(s)→ + Ir(s) + Co2+ (aq)
Transcribed Image Text:Balance redox reactions using the half-reaction method. Balance the redox reaction below using the half-reaction method. Ir³+ (aq) + Co(s) Ir(s) + Co²+ (aq) (a) To show your method, write the balanced half reactions below. Use the smallest integer coefficients possible and show electrons as e. If a box is not needed, leave it blank. (Coefficients of 1 are not needed). Oxidation half-reaction: + Reduction half-reaction: + - Ir³+ (aq) + → + (b) To show your balanced equation, enter an integer in each of the boxes. If the integer is "1," do enter it even though you would normally not show that in the equation. Use the smallest integer coefficients possible. Co(s)→ + Ir(s) + Co2+ (aq)
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