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Consider the following reaction at 298K.
I2 (s) + 2 Cr2+ (aq) 2 I- (aq) + 2 Cr3+ (aq)

Which of the following statements are correct?

Choose all that apply.
n = 4 mol electrons
Eo cell < 0
delta G^o < 0
The reaction is reactant-favored.
K > 1

Consider The Following Reaction At 298K I2 S 2 Cr2 Aq 2 I Aq 2 Cr3 Aq Which Of The Following Statements Are Correct Choose All That Apply N 4 Mol Electrons Eo C class=

Sagot :

pstnonsonjoku

The true statements are;

  • ΔG  < 0
  • K  > 1

What are the correct statements?

Now we can see that the reaction here is a redox reaction. Thus;

Eocell = cell potential = 0.54 - (-0.41) = 0.95 V

K = equilibrium constant = ?

n = number of moles of electrons = 2

ΔG = change in free energy = ?

Hence;

Eocell = 0.0592/n log K

0.95 = 0.0592/2 log K

K = 0.95 * 2/0.0592

K = 1.2 * 10^32

Now

ΔG = -nFEcell

ΔG = - (2 * 96500 *  0.95)

ΔG = -183.3kJ

Learn more about Ecell:https://brainly.com/question/3807566

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