Consider the following reaction at 298K. 2 H+(aq) + 2 Cr2+(aq) =H2(g) + 2 Cr3+(aq)
Which of the following statements are correct?
a) K > 1
b) ΔGo < 0
c) Eocell < 0
d) n = 2 mol electrons

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.

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.

the answer would be b i believe

the correct answer is b. a strong acid completely dissociates to its ions when dissolved in water. completely dissociates to and ions. a is incorrect because does not fully ionize to and ions and some remain as the compound . c and d are incorrect because, and do not fall into the category of bronsted lowry acids. a bronsted lowry acid is a proton donor and since both molecules do not have a proton to donate they are not bronsted lowry acids. likewise,   if we use the lewis acid definition, they cannot be acids. a lewis acid is an electron pair acceptor. both and have a complete octet so can not accept any electrons which disqualifies them as acids.