For the following balanced reaction occurring at a constant temperature,what will be the change in the concentration of $CO$ if the volume of the system is decreased?
$2CO_{(g)} \rightleftharpoons O_{2(g)} + 2CO_{2(g)}$

Consider the following reaction:
$N_{2}O_{4(g)} \rightleftharpoons 2NO_{2(g)} ; \Delta H^{0} = +58 \ kJ$
For each of the following cases $(a, b)$,determine the direction in which the equilibrium shifts:
$(a)$ Temperature is decreased
$(b)$ Pressure is increased by adding $N_{2}$ at constant $T$ and constant $V$

In which of the following reactions will a change in pressure not affect the rate of reaction?

In a reversible reaction,a catalyst:

$H_{2(g)} + I_{2(g)} \rightleftharpoons 2HI_{(g)}$. In this reaction,when pressure increases,the reaction direction:

The rate of reaction of which of the following is not affected by pressure?