91影视

Rewrite the reaction as follows:

$2{\mathrm{NOBr}}_{\left(\mathrm{g}\right)}鈻�2{\mathrm{NO}}_{\left(\mathrm{g}\right)}+{\mathrm{Br}}_{2\left(\mathrm{g}\right)}$

The expression for the reaction quotient is the ratio of partial pressure of products to partial pressure of reactants, with each partial pressure term raised to a power equal to its stoichiometric coefficient.

The expression for the reaction quotient ${\mathrm{Q}}_{\mathrm{P}}\mathrm{is},$

${\mathrm{Q}}_{\mathrm{P}}=\frac{{\mathrm{P}}^2{}_{\mathrm{NO}}{\mathrm{P}}_{{\mathrm{Br}}_2}}{{\mathrm{P}}^2{}_{\mathrm{NOBr}}}$

The partial pressure of each gas in the reaction is 0.10 atm. That is

role="math" localid="1654920434762" $$\begin{gathered} {\mathrm{P}}_{\mathrm{NO}}={\mathrm{P}}_{{\mathrm{Br}}_2} \\ ={\mathrm{P}}_{\mathrm{NOBr}} \\ =0.10\mathrm{atm} \end{gathered}$$

The value of ${\mathrm{K}}_{\mathrm{P}}$for the reaction at 373 K is 60.6.

If the value of ${\mathrm{Q}}_{\mathrm{P}}$is equal to ${\mathrm{K}}_{\mathrm{P}}$, the reaction will be at equilibrium. Here, ${\mathrm{Q}}_{\mathrm{P}}$is less

than ${\mathrm{K}}_{\mathrm{P}}$.

Thus, the reaction is not at equilibrium.

If the value of ${\mathrm{Q}}_{\mathrm{P}}$is less than ${\mathrm{K}}_{\mathrm{P}}$, the reaction proceeds toward the product鈥檚 side to

attain equilibrium. Here ${\mathrm{Q}}_{\mathrm{P}}$is less than ${\mathrm{K}}_{\mathrm{P}}$.

Thus, the reaction shifts towards products.