Question

\\(\text{i}_2 = 0.350\text{ m}\\), \\(\text{cl}_2 = 0.350\text{ m}\\), and \\(\text{icl} = 0.100\text{ m}\\) are the initial concentrations added to a flask at \\(25\text{ }^{\circ}\text{c}\\).

\\(k = 12.25\\)

what is the value of the reaction quotient, q?

\\\text{i}_2(\text{g}) + \text{cl}_2(\text{g}) \
ightleftharpoons 2\text{icl}(\text{g})\\

\\(q = ?\\)

Explanation:

Write the reaction quotient expression

Using the Reaction Quotient knowledge point

$$ Q = \frac{[\text{ICl}]^2}{[\text{I}_2][\text{Cl}_2]} $$

Substitute the initial concentrations

Using the Initial Concentrations knowledge point

$$
LATEXBLOCK0
$$

Calculate the value of Q

Using the Reaction Quotient knowledge point

$$ Q = \frac{(0.100)^2}{(0.350)(0.350)} = \frac{0.0100}{0.1225} \approx 0.0816 $$

Answer:

\([\text{I}_2] = 0.350\text{ M}\), \([\text{Cl}_2] = 0.350\text{ M}\), and \([\text{ICl}] = 0.100\text{ M}\) are the initial concentrations added to a flask at \(25\text{ }^{\circ}\text{C}\).

\(K = 12.25\)

What is the value of the reaction quotient, Q?

\(\text{I}_2(g) + \text{Cl}_2(g)
ightleftharpoons 2\text{ICl}(g)\)

\(Q =\) <blank>\(0.0816\)</blank>