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Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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Question
Calculate the equilibrium constant for the following reaction at 298 K.
Cu(s) + 2 Ag+(aq) → Cu2+(aq) + 2 Ag(s)
Cu2+(aq) + 2 e → Cu(s) Eored = +0.34 V
Ag+(aq) + 1 e → Ag(s) Eored = +0.80 V
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- Use standard reduction potentials to calculate the equilibrium constant for the reaction: Cu²+ (aq) + Pb(s) → Cu(s) + Pb²+ (aq) 2+ Cu²+ (aq) + 2e Pb²+ (aq) + 2e → Cu(s) Fre 0.337 V → Pb(s) Fe -0.126 V red = Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm. Equilibrium constant at 298 K: AGO for this reaction would be | than zero.arrow_forwardBalance the redox reaction in acidic solution. Y(s) + XO, (aq)→ YO(s) + XH3(aq)arrow_forwardBalance the following redox reaction in basic solution: Cu(s) + HNO3(aq) ---> Cu2+(aq) + NO(g) Oxidation half reaction: Reduction half reaction: Overall balanced equation:arrow_forward
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