The question is incomplete, the complete question is;
Consider the following reaction at 298K.
2 H+(aq) + 2 Cr2+(aq) =H2(g) + 2 Cr3+(aq)
Which of the following statements are correct?
Choose all that apply.
K > 1
ΔGo < 0
Eocell < 0
n = 2 mol electrons
The reaction is reactant-favored.
Answer:
K > 1
ΔGo < 0
n = 2 mol electrons
Explanation:
If we look at the reaction; 2 H+(aq) + 2 Cr2+(aq) -----> H2(g) + 2 Cr3+(aq), we will notice that the reaction is a spontaneous reaction because E°cell= 0-(-0.41) = 0.41 V
If the reaction is a spontaneous electrochemical process, we expect it to be product favoured with K>1. Also, a spontaneous reaction must have ∆G<0.
Lastly, we can see that two electrons were transferred according to the balanced equation for the electrochemical reaction.
