The standard emf for the cell using the overall cell reaction below is +2.20 V:
2 Al(s) + (s) → (aq) + (aq)
The emf generated by the cell when [ ] = 5.0 × Mol L^-1 and [ ] = 0.10 mol L^-1 is

Question

The standard emf for the cell using the overall cell reaction below is +2.20 V:
2 Al(s) +

(s) →

(aq) +

(aq)
The emf generated by the cell when [ The standard emf for the cell using the overall cell reaction below is +2.20 V: 2 Al(s) + (s) → (aq) + (aq) The emf generated by the cell when [ ] = 5.0 × Mol L-1 and [ ] = 0.10 mol L-1 is A) 2.20 B) 2.30 C) 2.10 D) 2.41 E) 2.23

] = 5.0 ×

Mol L^-1 and [ The standard emf for the cell using the overall cell reaction below is +2.20 V: 2 Al(s) + (s) → (aq) + (aq) The emf generated by the cell when [ ] = 5.0 × Mol L-1 and [ ] = 0.10 mol L-1 is A) 2.20 B) 2.30 C) 2.10 D) 2.41 E) 2.23

] = 0.10 mol L^-1 is The standard emf for the cell using the overall cell reaction below is +2.20 V: 2 Al(s) + (s) → (aq) + (aq) The emf generated by the cell when [ ] = 5.0 × Mol L-1 and [ ] = 0.10 mol L-1 is A) 2.20 B) 2.30 C) 2.10 D) 2.41 E) 2.23

Quizplus · Accepted Answer

Using the Nernst equation: 
E = E°- (RT/nF) ln(Q), where 
E° = +2.20 V 
T = 298 K 
n = 6 (from the balanced equation) 
F = 96,485 C/mol 
Q = (0.10 mol/5.0 mol)*[Hg2+]/[Cl-]^2 = 0.02*[Hg2+]/[Cl-]^2

Plugging in the values: 
E = 2.20 V - [(8.314 J/mol*K)*(298 K)/(6*96,485 C/mol)]*ln(0.02*[Hg2+]/[Cl-]^2) 
E = 2.30 V

Therefore, the answer is B)2.30.

The Standard Emf for the Cell Using the Overall Cell