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The following reactions have the indicated equilibrium constants at a particular temperature: N2(g) + O2(g) ⇌ 2NO(g)Kc = 4.3 × 10−25 2NO(g) + O2(g) ⇌ 2NO2(g)Kc = 6.4 × 109 Determine the value of the equilibrium constant for the following equation at the same temperature: N2(g) + 2O2(g) ⇌ 2NO2(g) Kc = × 10 (Enter your answer in scientific notation.)

Respuesta :

Answer:

[tex]K_c=2.752\times 10^{-15}[/tex]

Explanation:

The given equilibrium reaction is:

[tex]N_2_{(g)}+O_2_{(g)}\rightleftharpoons 2NO_{(g)}[/tex]

The expression for the equilibrium constant is:

[tex]K_c_1=\frac {[NO]^2}{[N_2][O_2]}=4.3\times 10^{-25}[/tex]

The another given equilibrium reaction is:

[tex]2NO{(g)}+O_2_{(g)}\rightleftharpoons 2NO_2_{(g)}[/tex]

The expression for the equilibrium constant is:

[tex]K_c_2=\frac {[NO_2]^2}{[NO]^2[O_2]}=6.4\times 10^{9}[/tex]

To find,

For the equilibrium which is:

[tex]N_2_{(g)}+2O_2_{(g)}\rightleftharpoons 2NO_2_{(g)}[/tex]

The expression for the equilibrium constant is:

[tex]K_c=\frac {[NO_2]^2}{[N_2][O_2]^2}[/tex]

Multiplying and dividing by [tex][NO]^2[/tex] and rearranging in the above equation as:

[tex]K_c=\frac {[NO_2]^2}{[NO]^2[O_2]}\times \frac {[NO]^2}{[N_2][O_2]}[/tex]

[tex]K_c=K_c_2\times K_c_1=6.4\times 10^{9}\times 4.3\times 10^{-25}=2.752\times 10^{-15}[/tex]

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