Question #170714

Initially, 1.0 mol of NO(g) and 1 mol of Cl₂(g) were added to a 1 L container. As a result of the reaction the equilibrium concentration of NOCl(g) became 0.96 M. Using the ICE table methodology determine the value of the equilibrium constant KC for this reaction. . 2NO(g) + Cl₂(g) ⇋2NOCl(g)

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2NO(g) + Cl_{2}(g) "\\leftrightarrow" 2NOCl

1mol/L____1mol/L____0mol/L

-2x______-x_________+2x

[NOCl]_{eq }= 2x = 0.96M

x = 0.48 M

Kc = "\\frac{[NOCl]^2}{[NO]^2[Cl]}" = "\\frac{[0.48]^2}{[1-2x]^2[1-x]}"

Kc = "\\frac{0.2304}{[1-0.96]^2[1-0.48]}" = "\\frac{0.2304}{[0.04]^2[0.52]}"

Kc = "\\frac{0.2304}{(0.0016)\u00d70.52}" = "\\frac{0.2304}{0.000832}" = 276.92

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