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13 Dec 2019

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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Jean Keeling
Jean KeelingLv2
17 Dec 2019

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Related questions

Please show all steps!

Calculate the equilibrium constant at 25 ∘C for the reaction

Ni(s)+Sn2+(aq)→Ni2+(aq)+Sn(s)


Standard Reduction Potentials at 25 ∘C

Ni2+(aq)+2e−→Ni(s) E∘= −0.26 V
Sn2+(aq)+2e−→Sn(s)

E∘=−0.14 V

Standard reduction potentials

Reduction half-reaction E∘ (V)
Ag+(aq)+e−→Ag(s) 0.80
Cu2+(aq)+2e−→Cu(s) 0.34
Sn4+(aq)+4e−→Sn(s) 0.15
2H+(aq)+2e−→H2(g) 0
Ni2+(aq)+2e−→Ni(s) −0.26
Fe2+(aq)+2e−→Fe(s) −0.45
Zn2+(aq)+2e−→Zn(s) −0.76
Al3+(aq)+3e−→Al(s) −1.66
Mg2+(aq)+2e−→Mg(s) −2.37

Part A

Use the table of standard reduction potentials given above to calculate the equilibrium constant at standard temperature (25 ∘C) for the following reaction:

Fe(s)+Ni2+(aq)→Fe2+(aq)+Ni(s)

Express your answer numerically.

Part B

Calculate the standard cell potential (E∘) for the reaction

X(s)+Y+(aq)→X+(aq)+Y(s)

if K = 3.04×10−3.

Express your answer to three significant figures and include the appropriate units.

Reduction half-reaction E∘ (V)
Ag+(aq)+e−→Ag(s) 0.80
Cu2+(aq)+2e−→Cu(s) 0.34
Sn4+(aq)+4e−→Sn(s) 0.15
2H+(aq)+2e−→H2(g) 0
Ni2+(aq)+2e−→Ni(s) −0.26
Fe2+(aq)+2e−→Fe(s) −0.45
Zn2+(aq)+2e−→Zn(s) −0.76
Al3+(aq)+3e−→Al(s) −1.66
Mg2+(aq)+2e−→Mg(s) −2.37

1)

Use the table of standard reduction potentials given above to calculate the equilibrium constant at standard temperature (25 ∘C) for the following reaction: Fe(s)+Ni2+(aq)→Fe2+(aq)+Ni(s)

2)

Calculate the standard cell potential (E∘) for the reaction

X(s)+Y+(aq)→X+(aq)+Y(s)

if K = 3.80×10−4.

Express your answer to three significant figures and include the appropriate units.

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