© Macmillan Learning E = Consider the reactions. Zn2++ 4 NH3 Zn(NH₂)²+ = 5.01 × 108 E°=-0.762 V Zn2+ + 2eZn(s) Assuming there is negligible current and nearly all Zn² + is in the form Zn(NH3)²+, what cathode potential (vs. S.H.E.) would be required to reduce 99.99% of the Zn² + from a solution containing 0.12 M Zn² + in 1.0 M of ammonia? Assume T = 298 K. V
© Macmillan Learning E = Consider the reactions. Zn2++ 4 NH3 Zn(NH₂)²+ = 5.01 × 108 E°=-0.762 V Zn2+ + 2eZn(s) Assuming there is negligible current and nearly all Zn² + is in the form Zn(NH3)²+, what cathode potential (vs. S.H.E.) would be required to reduce 99.99% of the Zn² + from a solution containing 0.12 M Zn² + in 1.0 M of ammonia? Assume T = 298 K. V
Chapter18: Introduction To Electrochemistry
Section: Chapter Questions
Problem 18.2QAP
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