What is the equilibrium constant for the following reaction at 25°C?
Mg(s) + Zn2+(aq) = Mg2+(aq) + Zn(s)

To determine the equilibrium constant for the above chemical reaction is

Given the following data:

The balanced chemical equation for the reaction is:

To determine the equilibrium constant for the above chemical reaction:

Mathematically, the standard cell potential of a galvanic cell is given by the formula:

Now, we can determine the equilibrium constant by using the formula:

Substituting the parameters into the formula, we have;

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2.45×10^54

Explanation:

Mg(s) + Zn2+(aq) = Mg2+(aq) + Zn(s)

From the equation;

n= 2 moles of electrons

E°anode= -2.37 V

E°cathode= -0.76 V

From E°Cell= E°cathode - E°anode

E°Cell= -0.76-(-2.37) = 1.61 V

Recall that E°cell= 0.0592/n log K

1.61= 0.0592/2 log K

log K = 1.61/0.0296

K= Antilog (54.39)

K= 2.45×10^54

the atomic number will stay the same no matter how many electrons it has, so it doesn’t decrease nor increase. it’ll only change with a different number of protons

a pan containing water is placed in a positio n where it is exposed to a 10 mile per hour wind. the pan contains a uniform depth of 1.27 cm of water, is quite wide, and has a length of 2.44 m in the wind direction. the water in the pan is at a constant temperature of 15.5 °c.