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Consider the reaction between NONO and Cl2Cl2 to form NOClNOCl: 2NO(g)+Cl2(g)⇌2NOCl(g)2NO(g)+Cl2(g)⇌2NOCl(g) A reaction mixture at a certain temperature initially contains only [NO]=[NO]= 0.53 MM and [Cl2]=[Cl2]= 0.64 MM. After the reaction comes to equilibrium, the concentration of NOClNOCl is 0.36 MM. Part A Find the value of the equilibrium constant (Kc)(Kc) at this temperature.

Answer :

Answer : The value of equilibrium constant (Kc) is, 9.75

Explanation :

Now we have to calculate the value of equilibrium constant (K).

The given chemical reaction is:

                       [tex]2NO(g)+Cl_2(g)\rightarrow 2NOCl(g)[/tex]

Initial conc.     0.53          0.64              0

At eqm.       (0.53-2x)     (0.64-x)          2x

The expression for equilibrium constant is:

[tex]K_c=\frac{[NOCl]^2}{[NO]^2[Cl_2]}[/tex]

As we are given that:

2x = 0.36 M

x = 0.18 M

Now put all the given values in this expression, we get:

[tex]K_c=\frac{(2x)^2}{(0.53-2x)^2\times (0.64-x)}[/tex]

[tex]K_c=\frac{(2\times 0.18)^2}{(0.53-2\times 0.18)^2\times (0.64-0.18)}[/tex]

[tex]K_c=9.75[/tex]

Thus, the value of equilibrium constant (Kc) is, 9.75

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