A copper penny dropped into a solution of nitric acid produces a mixture of nitr

Question

A copper penny dropped into a solution of nitric acid produces a mixture of nitrogen oxides. The following reaction describes the formation of NO, one of the products.

3Cu(s) + 8H+(aq) + 2NO3-(aq) -----> 2NO(g) + 3Cu^2+(aq) + 4H2O(l)

E cell for this reaction is 0.620 V.

What is the value of E rxn at 228 K. when [H+] = 0.100 M, [NO3-] = 0.0350 M, [Cu2+] = 0.0300 M, and the partial pressure of NO is 0.0014 atm?

A copper penny dropped into a solution of nitric acid produces a mixture of nitrogen oxides. The following reaction describes the formation of NO, one of the products 3Cu(s) + 8H+(aq) + 2NO, (aq) 2NO(g) + 3Cu2 + (aq) + 4H20(1) E cell for this reaction is 0.620 V What is the value of Erxn at 228 K, when [H+] = 0.100 M, [NO3-1-0.0350 M, [Cu2+] = 0.0300 M, and the partial pressure of NO is 0.0014 atm?

Explanation / Answer

E cell for the reaction is 0.62V

E= Eo- 0.0592/n logQ

Q= [Cu+2]3 [ PNO]2/ [NO3-]2 [H+]8 = (0.030)3*(0.0014)2/ (0.0350)2*(0.1)8 = 4.32

logQ= 0.635

E= 0.62-(0.0592/6)*0.635 =0.613V

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