Question

\text{h}_2 = 0.40\text{ m}, \text{br}_2 = 0.40\text{ m}, \text{ and } \text{hbr} = 0.05\text{ m} \text{ are the initial concentrations added to a flask at } 25\text{ }^{\circ}\text{c}.

k = 25.0

what is the value of the reaction quotient, q?

\text{h}_2(g) + \text{br}_2(g) \
ightleftharpoons 2\text{hbr}(g)

q = ?

Explanation:

Write the reaction quotient expression

Using the Chemical Equilibrium and Equilibrium Constant knowledge points

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

Substitute the initial concentrations

Using the Chemical Equilibrium knowledge point

$$
LATEXBLOCK0
$$

Calculate the numerical value of Q

Using the Chemical Equilibrium knowledge point

$$
LATEXBLOCK1
$$

Answer:

What is the value of the reaction quotient, Q?
\( \text{H}_2(g) + \text{Br}_2(g)
ightleftharpoons 2\text{HBr}(g) \)
\( Q = \) <blank>\(0.016\)</blank>