a)A half-cell that consists of a copper wire in 1.00 M CuNO 3 solution is connec
ID: 797459 • Letter: A
Question
a)A half-cell that consists of a copper wire in 1.00 M CuNO3 solution is connected by a salt bridge to a half cell containing a 1.00 M X(II) acetate solution and an electrode of metal X. The voltage of the cell is 1.77 V, with metal X as the positive electrode. Calculate the standard reduction potential for the X half-reaction. The standard reduction potential of the copper half-reaction is 0.52 V. (Hint, write the half-reactions and the overall chemical equation for the spontaneous reaction.)
b)
Calculate ?Go (in J) for 1 moles of electron(s) in each half-reaction and a standard potential of 0.35 V.
c)Calculate ?Go (in J) for 2 moles of electron(s) in each half-reaction and a standard potential of (-0.21) V.
d)Calculate Keq for 1 moles of electron(s) in each half-reaction and a standard potential of 0.54 V.
e)Calculate Keq for 2 moles of electron(s) in each half-reaction and a standard potential of (-0.54) V.
Explanation / Answer
1) E CELL= E CATHODE -E ANODE
1.77= E CATHODE - 0.52
E CATHODE= 1.77 + 0.52
= 2.29 V
2)
A) DELTA G= -nF E CELL
= -1* 96500 * 0.35 = - 33775 V
B) DELTA G= nF E CELL
=- 2*96500*(-0.24) = 46320 J
C) log K=n*E CELL/0.059
log K=1*0.54/0.059
K= 1.4*10^-9
D) log k= n*E CELL/0.059
log k= 2*(-0.54)/0.059
k= 1.9*10^-19
Related Questions
drjack9650@gmail.com
Navigate
Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.