I am stuck on 2 problems and would be grateful if anyone decided to give me a proper explanation as to how to solve them. I am not sure how to use the given information to correctly solve what is being asked. I have included the answers so its not a matter of academic integrity, I am genuinely lost.
- Given the equation: $$\ce{2X^3+ + 3 Y -> 3 Y^2+ + 2X}$$ The standard reduction potential for the X cation is $\pu{0.498 V}$.
The standard reduction potential for the Y cation is $\pu{0.187 V}$.
Using the Nernst equation, calculate the $\log$ of the equilibrium constant $K$ for the above reaction.
The answer is $\log K = 31.52$.
Using the answer, I attempted to work backwards:
$$0.685 = \frac{0.0592}{n} \times 31.52 \implies n = 2.724 ,$$
which I don't understand since $n$ is supposed to be the number of electrons.
- Given the equation:
$$\ce{2 X+ + Y -> Y^2+ + 2 X}$$
The equilibrium constant for the reaction is $5.912 \cdot 10^{13}$.
You measure the concentration of $\ce{Y^2+}$ to be $\pu{0.0674 M}$.
Calculate molar concentration of $\ce{X^+}$.
The answer is $\pu{33.8 nM}$. This one I'm not even sure.