Consider the following reaction: SO2Cl2(g)⇌SO2(g)+Cl2(g) A reaction mixture is made containing an initial [SO2Cl2] of 2.2×10−2M . At equilibrium, [Cl2]= 1.3×10−2M . Calculate the value of the equilibrium constant (Kc).

The value of equilibrium constant is equal to the quotient of the products raised to its stoichiometric coefficient over the reaction's reactants raised to its respective stoichiometric coeff. The equation is Kc=[SO2][Cl2]/[SO2Cl2]= [1.3*10^-2][1.3*10^-2]/[2.2*10^-2-1.3*10^-2]=0.0188. The final answer is Kc=0.0188.

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throwdolbeau throwdolbeau · Answer 2 · 2022-02-01T15:00:33+01:00

The value of equilibrium constant (Kc) will be 0.0188.

Equilibrium constant :

The equilibrium constant of a chemical reaction is the value of its reaction quotient at chemical equilibrium, a state approached by a dynamic chemical system after sufficient time has elapsed at which its composition has no measurable tendency towards further change.

Given reaction:

SO₂Cl₂(g)⇌SO₂(g)+Cl₂(g)

To find:

Kc=?

The equation that represents kc for the given reaction will be:

[tex]k_c=\frac{[SO_2][Cl_2]}{[SO_2Cl_2]}[/tex]

On substituting the initial concentration:

[tex]k_c=\frac{[SO_2][Cl_2]}{[SO_2Cl_2]}\\\\k_c=\frac{[1.3*10^{-2}][1.3*10^{-2}]}{[2.2*10^{-2}-1.3*10^{-2}]} \\\\k_c=0.0188[/tex]

Thus, the value of equilibrium constant (Kc) will be 0.0188.

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