Consider the following reaction at equilibrium:

$2C{O}_2(g)2CO(g)+O_2(g),H=-514kJ$

Fill in the blanks in the statements below with a preceding bolded term. If the reaction equilibrium is not affected by the change described, enter neither.

When more $C{O}_2$ is added, the reaction will proceed $($left$,$ right, neither$)$ to re$-$establish equilibrium.

When the partial pressure of $CO$ is decreased, the reaction will proceed $($left$,$ right, neither$)$ to re$-$establish equilibrium.

When the volume of the container is decreased, the reaction will proceed $($left$,$ right, neither$)$ to re$-$establish equilibrium.

When the temperature is increased, the reaction will proceed $($left$,$ right, neither$)$ to re$-$establish equilibrium.