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 6 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.

Calculate the equilibrium constant K of the reaction Sn(s)|Sn2+(aq)||Ag+(aq)|Ag(s) at 25 °C.

Calculate E at 25° C for a galvanic cell based on the reaction: Zn(s) + Cu2+(aq)→Zn...

Calculate E at 25° C for a galvanic cell based on the reaction: Zn(s) + Cu2+(aq)→Zn 2+(aq) + Cu (s) in which [Zn2+]=0.55M and [Cu2+]=1.02M

Calculate the equilibrium constant for each of the reactions at 25 ∘C . A.) 2Fe3+(aq)+3Sn(s)→2Fe(s)+3Sn2+(aq) B.)...

Calculate the equilibrium constant for each of the reactions at 25 ∘C . A.) 2Fe3+(aq)+3Sn(s)→2Fe(s)+3Sn2+(aq) B.) O2(g)+2H2O(l)+2Cu(s)→4OH−(aq)+2Cu2+(aq) C.) Br2(l)+2I−(aq)→2Br−(aq)+I2(s)

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

What is the value of the equilibrium constant for the reaction of Na(s)with Pb2+ (aq)at 25°...

What is the value of the equilibrium constant for the reaction of Na(s)with Pb2+ (aq)at 25° C? Eº cell = 2.58 V 2Na(s) + Pb2+(aq) ↔ Pb(s) + 2Na+(aq) 3.0 x 1043 6.0 x 10200 6.0 x 10 43 1.8 x 1087

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)...

Calculate ΔG° for the following reaction as written Ni2+ (aq) + Sn (s) → Ni (s) + Sn2+ (aq) given the following reduction half-reactions and standard reduction potentials. Sn2+ (aq) + 2 e- → Sn (s) E° = -0.15V Ni2+ (aq) + 2 e- → Ni (s) E° = -0.25V

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

The reaction F + G = H is at equilibrium, under standard conditions. (a) Calculate ∆Go’ if [F] = 2mM, [G] = 3 mM, and [H] = 9 mM (b) What happens to ∆Go’ if the solution is at equilibrium at twice this concentration of F? (c) What happens to ∆Go’ if the solution is at equilibrium at twice this concentration of H? (d) Does this violate LeChatelier’s Principle?

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.

Question