Consider the following unbalanced oxidation-reduction reactions in aqueous solution:
Ag⁺(aq) + Li(s) Ag(s) + Li⁺(aq)
Fe(s) + Na⁺(aq) Fe²⁺(aq) + Na(s)
K(s) + H₂O(l) KOH(aq) + H₂(g)
(a) Balance each of the reactions. (b) By using data in Appendix C, calculate ∆H° for each of the reactions. (c) Based on the values you obtain for ∆H°, which of the reactions would you expect to be thermodynamically favored? (d) Use the activity series to predict which of these reactions should occur. (Section 4.4) Are these results in accord with your conclusion in part (c) of this problem?

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Trinidad TremblayLv2

20 May 2020

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Which of these redox reactions do you expect to occur spontaneously in the forward direction?

Standard Electrode Potentials at 25 ?C

Reduction Half-Reaction		E?(V)
Ni2+(aq)+2e?	?Ni(s)	-0.23
Zn2+(aq)+2e?	?Zn(s)	-0.76
Cd2+(aq)+2e?	?Cd(s)	-0.40
Co2+(aq)+2e?	?Co(s)	-0.28
Pb2+(aq)+2e?	?Pb(s)	-0.13
Fe2+(aq)+2e?	?Fe(s)	-0.45
Al3+(aq)+3e?	?Al(s)	-1.66
Ag+(aq)+e?	?Ag(s)	0.80
Cr3+(aq)+3e?	?Cr(s)	-0.73
Mn2+(aq)+2e?	?Mn(s)	-1.18

Consider the following acid-neutralization reactions involving the strong base NaOH(aq):
HNO₃(aq) + NaOH(aq) NaNO₃(aq) + H₂O(l)
HCl(aq) + NaOH(aq) NaCl(aq) + H₂O(l)
NH₄⁺(aq) + NaOH(aq) NH₃(aq) + Na⁺(aq) + H₂O(l)

(a) By using data in Appendix C, calculate ∆H° for each of the reactions. (b) As we saw in Section 4.3, nitric acid and hydrochloric acid are strong acids. Write net ionic equations for the neutralization of these acids. (c) Compare the values of ∆H° for the first two reactions. What can you conclude? (d) In the third equation NH₄⁺ (aq) is acting as an acid. Based on the value of ∆H° for this reaction, do you think it is a strong or a weak acid? Explain.