The standard emf for the cell using the overall cell reaction below is +0.48 V:
Zn(s) + (aq) → (aq) + Ni(s)
The emf generated by the cell when [ ] = 2.50 mol L^-1 and [ ] = 0.100 mol L^-1 is

Question

The standard emf for the cell using the overall cell reaction below is +0.48 V:
Zn(s) +

(aq) →

(aq) + Ni(s)
The emf generated by the cell when [ The standard emf for the cell using the overall cell reaction below is +0.48 V: Zn(s) + (aq) → (aq) + Ni(s) The emf generated by the cell when [ ] = 2.50 mol L-1 and [ ] = 0.100 mol L-1 is A) 0.40 B) 0.50 C) 0.52 D) 0.56 E) 0.44

] = 2.50 mol L^-1 and [ The standard emf for the cell using the overall cell reaction below is +0.48 V: Zn(s) + (aq) → (aq) + Ni(s) The emf generated by the cell when [ ] = 2.50 mol L-1 and [ ] = 0.100 mol L-1 is A) 0.40 B) 0.50 C) 0.52 D) 0.56 E) 0.44

] = 0.100 mol L^-1 is The standard emf for the cell using the overall cell reaction below is +0.48 V: Zn(s) + (aq) → (aq) + Ni(s) The emf generated by the cell when [ ] = 2.50 mol L-1 and [ ] = 0.100 mol L-1 is A) 0.40 B) 0.50 C) 0.52 D) 0.56 E) 0.44

Quizplus · Accepted Answer

The emf of the cell can be calculated using the Nernst equation: Ecell = E°cell - (RT/nF)ln(Q) where E°cell is the standard emf, R is the gas constant, T is the temperature, n is the number of electrons involved in the reaction, F is Faraday's constant, and Q is the reaction quotient. The reaction quotient can be calculated using the concentrations of the species involved in the reaction: Q = ([Ni2+]/[Zn2+][L^-1]^11) Plugging in the given values, we get: Q = (0.100)/(2.50^11) = 5.12 x 10^-15 Substituting this into the Nernst equation and solving for Ecell, we get: Ecell = 0.48 - (0.0257/2)*ln(5.12 x 10^-15) = 0.52 V Therefore, the correct answer is C, 0.52.

The Standard Emf for the Cell Using the Overall Cell