X^2+ + 2e- -> X(s) E=1.73V
Y^2+ + 2e- -> Y(s) E=0.40v
Which pair of species would react under standard conditions?
X^2+ and Y^2+
X and Y^2+
X and Y
X^2+ and Y
Would it be X and Y because the E is positive?
I don't think X + Y will be positive. In fact they won't react at all.
X^2+ + Y ==> X + Y^2+ 1.73-0.40 = +?
So would it be X^2+ and Y^2+?
No. How do you get a reaction out of X^2 + Y^2?
X^2+ + 2e ==> X
Y^2+ + 2e = Y
Both of them are being reduced. In a reaction an oxidation is ALWAYS accompanied with a reduction.
So X and Y won't react.
X^2+ + Y^2+ won't react.
The only possibilities are the second and fourth choices and I gave you the right choice in my first response.
To determine which pair of species would react under standard conditions, we need to compare the standard reduction potentials (E°) of the half-cell reactions. The half-cell reaction with a more positive E° value will tend to occur in the forward direction.
In this case, the reduction potential for X^2+ + 2e- -> X(s) is given as E=1.73V, and the reduction potential for Y^2+ + 2e- -> Y(s) is given as E=0.40V.
Comparing the values, we see that the reduction potential for X^2+ is higher (more positive) than that for Y^2+. This means that X^2+ has a greater tendency to gain electrons and be reduced, compared to Y^2+. Therefore, X^2+ and Y would be the pair of species that would react under standard conditions.
It's important to note that the sign of the reduction potential (positive or negative) alone does not determine whether a reaction will occur under standard conditions. The magnitude and relative values of the reduction potentials are what determine the feasibility of the reaction.