Predict whether the following reactions are spontaneous or not Pd + 2 + H_2 doub

Question

Predict whether the following reactions are spontaneous or not Pd + 2 + H_2 doubleheadarrow Pd + 2H^+; S_n + 4 + H_2 doubleheadarrow S_n^+ 2 + 2H^+; Ni^+2 + H_2 doubleheadarrow Ni + 2H^+; Cd^+2 + H_2 doubleheadarrow Cd + 2H^+; Pd^+2 + 2e^-1 doubleheadarrow Pd Sn^+4 + 2e^1 doubleheadarrow Sn Ni^+2 + 2e^-1 doubleheadarrow Ni Cd^+ 2 + 2e^-1 doubleheadarrow Cd E degree = 0.987 V E degree = 0.154 V E degree = -0.250 V E degree = - 0.250 V E degree = - 0.403 V Which of the above metals or metal could be oxidized in a solution containing hydrogen ions? Mark all of the ionic reactions shown above spontaneous and then identify the oxidizing and reducing agents in each. b. List the metals or metal ions according to increasing activity.

Explanation / Answer

1. Spontaneous reactions are those whose Eo values are positive. A negative Eo value suggest the reaction is non-sponatneous in the forward direction.

So,

First and second reactions are spontaneous

Third and fourth reactions are non-sponatneous

2. Of the metals, Ni and Cd can be oxidized in a solution containing hydrogen ions.

3. a.

spontaneous reactions

First reaction, Pd2+ = oxidizing agent ; H2 = reducign agent

Second reaction, Sn4+ = oxidizing agent ; H2 = reducing agent

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