In order to determine the identity of a particular transition metal (M) ,a voltaic cell is constructed at 25°C with the anode consisting of the transition metal as the electrode immersed in a solution of 0.0977 M M(NO3) 2,and the cathode consisting of a copper electrode immersed in a 0.0724M Cu(NO3) 2 solution.The two half-reactions are as follows:
M(s)
M2+(aq) + 2e-
Cu2+(aq) + 2e-
Cu(s)
The potential measured across the cell is 1.13 V.What is the identity of the metal M?
Reduction Half-Reaction
E° (V)
Cu2+(aq) + 2e-
Cu(s) +0.34
Ni2+(aq) + 2e-
Ni(s) -0.23
Cd2+(aq) + 2e-
Cd(s) - 0.40
Zn2+(aq) + 2e-
Zn(s) -0.76
Mn2+(aq) + 2e-
Mn(s) -1.18
A) Zn
B) Ni
C) Cu
D) Cd
E) Mn
Correct Answer:
Verified
Q85: Given: Q86: Which of the following statements about batteries Q87: Molten magnesium chloride is electrolyzed using inert Q88: In order to determine the identity of Q89: What is the copper(II)-ion concentration at 25°C Q91: What half-reaction occurs at the cathode during Q92: Cathodic protection results when Q93: A piece of iron half-immersed in a Q94: A cell consists of a magnesium electrode Q95: What is the value of the reaction
Zn2+(aq)+ 2e- ![]()
A)iron is amalgamated with
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