Use the standard reduction potentials given below to predict if a reaction will occur when Cd metal is put into a 1 M aqueous Pb²+ solution. 2+ Pb²+ (aq) + 2e Cd²+ (aq) + 2e -> = -0.126 V Pb(s) E red → Cd(s) E -0.403 V red + wwww www If a reaction will occur, write a balanced net ionic equation for the reaction. If no reaction will occur, leave all boxes blank. (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) +

Use the standard reduction potentials given below to predict if a reaction will occur when Cd metal is put into a 1 M aqueous Pb²+ solution. 2+ Pb²+ (aq) + 2e Cd²+ (aq) + 2e -> = -0.126 V Pb(s) E red → Cd(s) E -0.403 V red + wwww www If a reaction will occur, write a balanced net ionic equation for the reaction. If no reaction will occur, leave all boxes blank. (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) +

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Using the standard reduction potentials listed in Appendix E in the textbook, calculate the equilibrium constant for each of the following reactions at 298 K. Fe(s)+Ni2+(aq)→Fe2+(aq)+Ni(s)
Use standard reduction potentials to calculate the equilibrium constant for the reaction: 2Ag+ (aq) + 21¯(aq) → 2Ag(s) + I₂ (s) Ag+ (aq) + e¯ → Ag(s) E = 0.799 V red I₂ (s) + 2e¯ → 21¯ (aq) Eº 0.535 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.
Use standard reduction potentials to calculate the standard free energy change in kJ for the reaction: 2Cu²+ u²+ (aq) + 21- (aq) → 2Cut (aq) + 12 (8) 2+ Cu²+ (aq) + e → Cut (aq) Ee red I2 (s) +2e → 21¯ (aq) AGO = K for this reaction would be kJ E red - 0.153 V 0.535 V than one.
Use standard reduction potentials to calculate the equilibrium constant for the reaction: 2Ag (aq) + Fe(s) → 2Ag(s) + Fe²+ (aq) Ag+ (aq) + e → Ag(s) E red Fe2+ (aq) + 2e → Fe(s) E red www 0.799 V -0.440 V 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.
1. Consider the following standard reduction potentials in acid solution: E°(V) -1.66 +0.07 +0.14 Fe³+ + e +0.77 The strongest reducing agent among those shown above is Hint: If answer is with charge, type this way: X2+ Al³+ + 3e → Al(s) AgBr(s) + e → Ag(s) + Brā Sn4+ + 2e → + 2e → Sn²+ Fe²+
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.
Use the standard reduction potentials given below to predict if a reaction will occur when Cr metal is put into a 1 M aqueous 2+ Hg²+ solution. 2+ Hg²+ (aq) + 2e¯ → Hg(1) E red - = 0.855 V Cr³+ (aq) + 3e¯ → Cr(s) Ee -0.740 V red = If a reaction will occur, write a balanced net ionic equation for the reaction. If no reaction will occur, leave all boxes blank. (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) 2Cr(s) + 3Hg²+ (aq) 2Cr³(aq) + 3Hg(1)
Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free energy delta G^0 for the following redox reaction. I2(s) + 6H2O(l) + 5 Cl2(g) -> 2IO3-(aq) + 12H+(aq) + 10Cl-(aq)Be sure your answer has the correct number of significant digits.
Use standard reduction potentials to calculate the standard free energy change in kJ for the reaction: Cu²+ (aq) + 2Cu+ (aq) → Cu(s) + 2Cu²+ (aq) 2+ Cu²+ (aq) + 2e → Cu(s) Ee = 0.337 V red 0.153 V = 2+ Cu²+ (aq) +e → Cut (aq) E red AG° kJ K for this reaction would be than one.
Use standard reduction potentials to calculate the standard free energy change in kJ for the reaction: 2H+ (aq) + Hg(1)→ H₂(g) + Hg²+ (aq) 2H+ (aq) + 2e¯ → H₂(g) Fº red 2+ Hg2 (aq) + 2e¯ → Hg(1) AGO = || kJ K for this reaction would be Eº red = 0.000 V = = 0.855 V than one.
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