Please help with this smartwork!! If you could also provide work, that would mea
ID: 978728 • Letter: P
Question
Please help with this smartwork!! If you could also provide work, that would mean a lot!
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_3^-(aq) right arrow 2NO(g) + 3Cu^2+ (aq) + 4H_2O(l) Using the provided standard potentials, calculate E degree_cell for this reaction. Cu^2+ (aq) + 2e^- right arrow Cu(s) E^degree = 0.3419V 4H^+ (aq) + NO^-_3 (aq)_3e^- right arrow NO(g) + 2H_2O(l) E degree = 0.96 V What is the value of Edegree_rxn at 230.00 K when [H^+] = 0.100 M, [NO_3^-] = 0.02500 M, [Cu^2+] = 0.03000 M, and the partial pressure of NO is 0.002200 atm?Explanation / Answer
1) E0cell = E0cathode(red) - E0anode(red) = 0.96 - 0.3419 = 0.6181 V
2) As per Nernst Equation,
Ecell = E0cell - (0.059/n)*logQ = 0.6181 - (0.059/6)*log{[Cu2+]3*PNO2/[NO3-]2*[H+]8} = 0.6051 V