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 1 year 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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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...

A voltaic cell is constructed that uses the following reaction and operates at 298 K: Zn(s)+Ni2+(aq)→Zn2+(aq)+Ni(s)....

A voltaic cell is constructed that uses the following reaction and operates at 298 K: Zn(s)+Ni2+(aq)→Zn2+(aq)+Ni(s). a. What is the emf of this cell when [Ni2+]= 2.10 M and [Zn2+]= 0.160 M ? b. What is the emf of the cell when [Ni2+]= 0.100 M and [Zn2+]= 0.860 M ? Thanks!

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calculate E cell at 298 K (25 c) for Zn (s) + Cu 2+ (aq) --> Zn 2+ (aq) + Cu (s) when [Zn 2+]=.0010 M and [Cu 2+]=.10 M

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