Final answer:
To calculate E°, E, and ΔG for the given cell reaction, we can use the Nernst equation and the formula for ΔG. First, we calculate the concentrations of the reactants and products, then calculate the reaction quotient Q. Using the Nernst equation, we calculate E° and E. Finally, we use the formula for ΔG to calculate the value. Therefore, E° = 0.0143V, E = 0.0135V, and ΔG = -0.0008kJ/mol.
Step-by-step explanation:
The given cell reaction is:
Mg(s) + Sn2+(aq) → Mg2+(aq) + Sn(s)
To calculate E°, E, and ΔG, we can use the formula:
E = E° - (0.0592/n)log(Q)
First, we need to calculate the concentrations of the products and reactants using the given values:
[Mg2+] = 0.045M
[Sn2+] = 0.035M
Next, we can calculate the value of Q, which is the reaction quotient:
Q = [Mg2+]/[Sn2+]
Plugging in the values, we get:
Q = 0.045/0.035 = 1.286
Now we can calculate E° using the Nernst equation:
E° = 0.0592/n * log(Q)
Since there are no coefficients in front of the reactants and products, the value of n is 1.
Plugging in the values, we get:
E° = 0.0592 * log(1.286) = 0.0143V
Finally, we can calculate E using the formula:
E = E° - (0.0592/n)log(Q)
Plugging in the values, we get:
E = 0.0143 - (0.0592/1)log(1.286) = 0.0143 - 0.0008 = 0.0135V
To calculate ΔG, we can use the formula:
ΔG = -nFE
Plugging in the values, we get:
ΔG = -1 * 0.0592 * 0.0135 = -0.0008kJ/mol
Therefore, E° = 0.0143V, E = 0.0135V, and ΔG = -0.0008kJ/mol.