# Problem: At 500.0 K, 1.0 mole of gaseous ONCl is placed in a 1.0-liter container. At equilibrium, it is 9.0% dissociated according to the equation:2 ONCl(g) ⇌ 2 NO(g) + Cl2(g)Determine the value of Kc:A. 4.4 × 10–4 B. 2.2 × 102 C. 1.1 × 102 D. 2.2 × 10–4E. 9.1 × 10–1

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###### FREE Expert Solution

We are being asked to calculate the equilibrium constant, Kc for the given equilibrium reaction:

2 ONCl(g) ⇌ 2 NO(g) + Cl2(g)

When dealing with equilibrium and Kc:

Kc → equilibrium units are in molarity
Kc is an equilibrium expression:

$\overline{){{\mathbf{K}}}_{{\mathbf{c}}}{\mathbf{=}}\frac{\mathbf{products}}{\mathbf{reactants}}}$

only aqueous and gaseous species are included in the equilibrium expression
▪ the coefficient of each compound in the reaction equation will be the exponent of the concentrations in the equilibrium expression

We need to calculate for the initial amount of the reactant ONCl. Recall molarity:

###### Problem Details

At 500.0 K, 1.0 mole of gaseous ONCl is placed in a 1.0-liter container. At equilibrium, it is 9.0% dissociated according to the equation:

2 ONCl(g) ⇌ 2 NO(g) + Cl2(g)

Determine the value of Kc:

A. 4.4 × 10–4

B. 2.2 × 10

C. 1.1 × 102

D. 2.2 × 10–4

E. 9.1 × 10–1