Calculate the equilibrium constant for the reaction between Ni2+(aq) and Zn(s) under standard conditions at 25∘C.

Expert Solution

queen_honey_blossom answered 5 months ago

Part A Calculate the equilibrium constant at 25 ∘C for the reaction Ni(s)+2Ag+(aq)→Ni2+(aq)+2Ag(s), if Ni2+(aq)+2e−→Ni(s), E∘...

Part A Calculate the equilibrium constant at 25 ∘C for the reaction Ni(s)+2Ag+(aq)→Ni2+(aq)+2Ag(s), if Ni2+(aq)+2e−→Ni(s), E∘ = -0.26 V, Al+(aq)+e−→Al(s), E∘ = 0.80 V Express your answer using one significant figure. Part B Calculate the equilibrium constant at 25 ∘C for the reaction Hg2+2(aq)→Hg(l)+Hg2+(aq) See Appendix D for standard reduction potentials. Express your answer using one significant figure.

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4. Calculate the equilibrium constant at standard temperature, 25oC, for the redox reaction between Pb2+(aq) and...

4. Calculate the equilibrium constant at standard temperature, 25oC, for the redox reaction between Pb2+(aq) and Zn(s). HINT: Write a balanced chemical reaction first. a) 1.17x1030 b) 1.92x1021 c) 4.38x1010 d) 1.08x1015 e) 1.75x109

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Under standard conditions, Consider the following standard reduction potentials, Ni2+(aq) + 2 e- → Ni(s) E°...

Under standard conditions, Consider the following standard reduction potentials, Ni2+(aq) + 2 e- → Ni(s) E° = -0.26 V I2(s) + 2 e- → 2 I-(aq) E° = +0.54 V Under standard conditions, a)Ni2+(aq) is a stronger oxidizing agent than I2(s) and I-(aq) is a stronger reducing agent than Ni(s). b)I2(s) is a stronger oxidizing agent than Ni2+(aq) and Ni(s) is a stronger reducing agent than I-(aq). c)I-(aq) is a stronger oxidizing agent than Ni(s) and I2(s) is a stronger...

Calculate ΔG° for the following reaction as written Ni2+ (aq) + Sn (s) → Ni (s)...

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The reaction F + G = H is at equilibrium, under standard conditions. (a) Calculate ∆Go’...

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Calculate the equilibrium constant for each of the reactions at 25∘C. Standard Electrode Potentials at 25...

Calculate the equilibrium constant for each of the reactions at 25∘C. Standard Electrode Potentials at 25 ∘C Reduction Half-Reaction E∘(V) Fe3+(aq)+3e− →Fe(s) -0.036 Sn2+(aq)+2e− →Sn(s) -0.14 Ni2+(aq)+2e− →Ni(s) -0.23 O2(g)+2H2O(l)+4e− →4OH−(aq) 0.40 Br2(l)+2e− →2Br− 1.09 I2(s)+2e− →2I− 0.54 Part A 2Fe3+(aq)+3Sn(s)→2Fe(s)+3Sn2+(aq) Express your answer using two significant figures. Part B O2(g)+2H2O(l)+2Ni(s)→4OH−(aq)+2Ni2+(aq) Express your answer using two significant figures. Part C Br2(l)+2I−(aq)→2Br−(aq)+I2(s) Express your answer using two significant figures.

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