Calculate the equilibrium constant for the following reaction: co2+ (aq) + zn(s> co (s) + zn2+ (aq)

The of the reaction is

Explanation:

For the given half reactions:

Oxidation half reaction:

Reduction half reaction:

Net reaction:

Oxidation reaction occurs at anode and reduction reaction occurs at cathode.

To calculate the of the reaction, we use the equation:

Putting values in above equation, we get:

To calculate equilibrium constant, we use the relation between Gibbs free energy, which is:

and,

Equating these two equations, we get:

where,

n = number of electrons transferred = 2

F = Faraday's constant = 96500 C

= standard electrode potential of the cell = 0.48 V

R = Gas constant = 8.314 J/K.mol

T = temperature of the reaction =

= equilibrium constant of the reaction = ?

Putting values in above equation, we get:

Hence, the of the reaction is

the answer to your question is c.

if you read the house of usher you should know that the house was haunted

i think it's c. i'm not sure but i think so.