We are being asked to calculate the equilibrium constant, K_{c} for the given equilibrium reaction:

**2 ONCl(g) ⇌ 2 NO(g) + Cl _{2}(g)**

**When dealing with equilibrium and K _{c}:**

• **K _{c} **→ equilibrium units are in molarity

•

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

▪ **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:**

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) + Cl_{2}(g)

Determine the value of K_{c}:

A. 4.4 × 10^{–4 }

B. 2.2 × 10^{2 }

C. 1.1 × 10^{2}

D. 2.2 × 10^{–4}

E. 9.1 × 10^{–1}

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Equilibrium Expressions concept. If you need more Equilibrium Expressions practice, you can also practice Equilibrium Expressions practice problems.

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