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Use the standard reduction potentials located in the 'Tables' linked above to calculate the equilibrium constant for the reaction: 1₂(s) + 2Ag(s)→→→→→→21 (aq) + 2Ag (aq) Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm. You may use the OWL references to find the values you may need in this question. Equilibrium constant: AGO for this reaction would be ✓than zero. Use the standard reduction potentials located in the Tables' linked above to calculate the equilibrium constant for the reaction: Ni²+ (aq) + 21 (aq) →→→→ Ni(s) + 1₂(s) Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm. You may use the OWL references to find the values you may need in this question. Equilibrium constant: AG for this reaction would be than zero.

Use the standard reduction potentials located in the 'Tables' linked above to calculate the equilibrium constant for the reaction: 1₂(s) + 2Ag(s)→→→→→→21 (aq) + 2Ag (aq) Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm. You may use the OWL references to find the values you may need in this question. Equilibrium constant: AGO for this reaction would be ✓than zero. Use the standard reduction potentials located in the Tables' linked above to calculate the equilibrium constant for the reaction: Ni²+ (aq) + 21 (aq) →→→→ Ni(s) + 1₂(s) Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm. You may use the OWL references to find the values you may need in this question. Equilibrium constant: AG for this reaction would be than zero.

Chemistry
Chemistry
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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
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Calculate K (both parts of the question)

Standard Reduction (Electrode) Potentials at 25 °C Half-Cell Reaction 2 F (aq) F₂(g) + 2 e Ce¹(aq) + e MnO₂ (aq) +8 Cl₂(g) + 2 e Cr₂0₂² (aq) + 14 H(aq) + 6 e —> 2 Cr³(aq) + 7 H₂0 (1) 0₂(g) + 4 H (aq) + 4e → 2 H₂0 (1) Br₂ (1) + 2 e 2 Br (aq) NO₂ (aq) + 4 H*(aq) + 3 e° ——» NO(g) + 2 H₂0 (1) 2 Hg2+ (aq) + 2 eHg₂² (aq) Ce³+ (aq) H*(aq) +5 e 2 Cl'(aq) Hg2+ (aq) + 2e Hg(1) Ag (aq)+eAg(s) Hg₂² (aq) +2 e →→→>2 Hg(!) Fe³+(aq) +e →→→Fe²+ (aq) 1₂ (s) + 2 e →21 (aq) Fe(CN),(aq) + e > Fe(CN),* (aq) Cu²+ (aq) +2 e Cu²+ (aq) + S(s) + 2 H* (aq) + 2 H₂S(aq) 2 H*(aq) + 2e Pb²+ (aq) + 2 e Sn²(aq) + 2 e Ni²+(aq) +2 e Co²+ (aq) + 2 Cd²+ (aq) +2 e Cr²³(aq) + e Fe²+ (aq) + 2 e Cr²³(aq) + 3 e Zn²2(aq) + 2 e 2 H₂O(1) + 2 e Cu(s) Cu(aq) H₂(g) > Pb(s) Sn(s) →→Ni(s) Mn²* (aq) + 4 H₂0 (1) Co(s) Cd (s) Cr²2 (aq) →→Fe(s) →→Cr(s) Zn(s) > H₂(g) + 2 OH(aq) Mn²(aq) + 2e →→Mn(s) A1³+ (aq) + 3 e →→→→Al(s) Mg2+ (aq) + 2 e Mg(s) Na (aq) +eNa(s) K* (aq) +e →→→K(s) Li (aq) +eLi(s) Eº (volts) 2.87 1.61 1.51 1.36 1.33 1.229 1.08 0.96 0.920 0.855 0.799 0.789 0.771 0.535 0.48 0.337 0.153 0.14 0.0000 -0.126 -0.14 -0.25 -0.28 -0.403 -0.41 -0.44 -0.74 -0.763 -0.83 -1.18 -1.66 -2.37 -2.714 -2.925 -3.045
Transcribed Image Text:Standard Reduction (Electrode) Potentials at 25 °C Half-Cell Reaction 2 F (aq) F₂(g) + 2 e Ce¹(aq) + e MnO₂ (aq) +8 Cl₂(g) + 2 e Cr₂0₂² (aq) + 14 H(aq) + 6 e —> 2 Cr³(aq) + 7 H₂0 (1) 0₂(g) + 4 H (aq) + 4e → 2 H₂0 (1) Br₂ (1) + 2 e 2 Br (aq) NO₂ (aq) + 4 H*(aq) + 3 e° ——» NO(g) + 2 H₂0 (1) 2 Hg2+ (aq) + 2 eHg₂² (aq) Ce³+ (aq) H*(aq) +5 e 2 Cl'(aq) Hg2+ (aq) + 2e Hg(1) Ag (aq)+eAg(s) Hg₂² (aq) +2 e →→→>2 Hg(!) Fe³+(aq) +e →→→Fe²+ (aq) 1₂ (s) + 2 e →21 (aq) Fe(CN),(aq) + e > Fe(CN),* (aq) Cu²+ (aq) +2 e Cu²+ (aq) + S(s) + 2 H* (aq) + 2 H₂S(aq) 2 H*(aq) + 2e Pb²+ (aq) + 2 e Sn²(aq) + 2 e Ni²+(aq) +2 e Co²+ (aq) + 2 Cd²+ (aq) +2 e Cr²³(aq) + e Fe²+ (aq) + 2 e Cr²³(aq) + 3 e Zn²2(aq) + 2 e 2 H₂O(1) + 2 e Cu(s) Cu(aq) H₂(g) > Pb(s) Sn(s) →→Ni(s) Mn²* (aq) + 4 H₂0 (1) Co(s) Cd (s) Cr²2 (aq) →→Fe(s) →→Cr(s) Zn(s) > H₂(g) + 2 OH(aq) Mn²(aq) + 2e →→Mn(s) A1³+ (aq) + 3 e →→→→Al(s) Mg2+ (aq) + 2 e Mg(s) Na (aq) +eNa(s) K* (aq) +e →→→K(s) Li (aq) +eLi(s) Eº (volts) 2.87 1.61 1.51 1.36 1.33 1.229 1.08 0.96 0.920 0.855 0.799 0.789 0.771 0.535 0.48 0.337 0.153 0.14 0.0000 -0.126 -0.14 -0.25 -0.28 -0.403 -0.41 -0.44 -0.74 -0.763 -0.83 -1.18 -1.66 -2.37 -2.714 -2.925 -3.045
Use the standard reduction potentials located in the 'Tables' linked above to calculate the equilibrium constant for the reaction: 1₂(s) + 2Ag(s)→→→→→21 (aq) + 2Ag+ (aq) Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm. You may use the OWL references to find the values you may need in this question. Equilibrium constant: AGO for this reaction would be ✓than zero. Use the standard reduction potentials located in the 'Tables' linked above to calculate the equilibrium constant for the reaction: Ni²+ (aq) + 21 (aq) →→→ Ni(s) + 1₂(s) Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm. You may use the OWL references to find the values you may need in this question. Equilibrium constant: AG for this reaction would be ✓than zero.
Transcribed Image Text:Use the standard reduction potentials located in the 'Tables' linked above to calculate the equilibrium constant for the reaction: 1₂(s) + 2Ag(s)→→→→→21 (aq) + 2Ag+ (aq) Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm. You may use the OWL references to find the values you may need in this question. Equilibrium constant: AGO for this reaction would be ✓than zero. Use the standard reduction potentials located in the 'Tables' linked above to calculate the equilibrium constant for the reaction: Ni²+ (aq) + 21 (aq) →→→ Ni(s) + 1₂(s) Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm. You may use the OWL references to find the values you may need in this question. Equilibrium constant: AG for this reaction would be ✓than zero.
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