The equilibrium charge-exchange reaction between hydrogen and deuterium is given by:
H2 + 2D+ (arrows) D2 + 2H+
Using the standard reduction potentials for each half reaction given below, determine which isoptope of hydrogen (H or D) prefers to be in the +1 state in aquesous solution under standard conditions.
2D+ + 2e- (right arrow) D2 E^o(red)=-0.044
2H+ + 2e- (right arrow) H2 E^o(red)=+0.000
I know that the D isotope is preferred; however, I don't know why. Please provide me with an explanation.
For this question you have to look qualitatively at the two potentials for the reactions. The hydrogen one is great because it is zero, both in the forward direction and the ...
The solution explains why the D isotope is preferred in the positive +1 state under standard conditions. This is shown through looking at the chemical properties and states behind the two chemicals, and how they react normally.