Question

because \\(q = 0.016\\) is less than \\(k = 25.0\\), the reaction proceeds toward the product. complete the
ice\ table below to find \x\.

\\(\

$$\begin{array}{|c|c|c|c|}\\hline \\text{r(eaction)} & \\text{h}_2\\text{(g)} + & \\text{br}_2\\text{(g)} & \ ightleftharpoons 2\\text{ hbr(g)} \\\\ \\hline \\text{i(nitial)} & 0.40 & 0.40 & 0.05 \\\\ \\hline \\text{c(hange)} & & & \\\\ \\hline \\text{e(quilibrium)} & & & \\\\ \\hline \\end{array}$$

\\)

what is the value of \x\ from the
ice\ table?

Explanation:

Set up the RICE table expressions

Using the RICE Table Calculations knowledge point

$$
LATEXBLOCK0
$$

Write the equilibrium constant expression

Using the Equilibrium Constant knowledge point

$$ K = \frac{[\text{HBr}]^2}{[\text{H}_2][\text{Br}_2]} = 25.0 $$

Substitute equilibrium concentrations into the expression

Using the Equilibrium Constant and RICE Table Calculations knowledge points

$$ \frac{(0.05 + 2x)^2}{(0.40 - x)^2} = 25.0 $$

Solve for x by taking the square root

Using the RICE Table Calculations knowledge point

$$
LATEXBLOCK1
$$

Answer:

\(x \approx 0.28\)