Indicate whether either an increase or a decrease of presure obtained by changing the volume would increase the amount of product in each of the following reactions.

a. CO(g) + 2H2(g) -> <- CH3OH
b. 2SO2(g) + O2(g) -> <- 2SO3(g)
c. COCl2(g) -> <- CO (g) + Cl2 (g)

a. CO(g) + 2H2(g) ⇌ CH3OH(g)

In this reaction, an increase in pressure obtained by changing the volume would favor the forward reaction (formation of CH3OH). According to Le Chatelier's principle, increasing the pressure will shift the equilibrium towards the side with fewer moles of gas.

As we can see, there are fewer moles of gas on the reactant side (1 mole of CO and 2 moles of H2) compared to the product side (1 mole of CH3OH). Therefore, increasing the pressure will favor the formation of CH3OH, resulting in an increase in the amount of product.

b. 2SO2(g) + O2(g) ⇌ 2SO3(g)

In this reaction, an increase in pressure obtained by changing the volume would favor the forward reaction (formation of SO3). Similar to the previous reaction, increasing the pressure will shift the equilibrium towards the side with fewer moles of gas.

On the reactant side, we have 3 moles of gas (2 moles of SO2 and 1 mole of O2), while on the product side, we have 2 moles of gas (2 moles of SO3). Once again, increasing the pressure will favor the formation of SO3, leading to an increase in the amount of product.

c. COCl2(g) ⇌ CO(g) + Cl2(g)

In this reaction, an increase in pressure obtained by changing the volume would not significantly affect the amount of product. Both the reactant and product sides have 3 moles of gas in this reaction.

Therefore, changing the volume to increase pressure would not have a significant impact on the amount of product formed in this reaction.

To determine whether an increase or decrease in pressure obtained by changing the volume would increase the amount of product in each reaction, we need to analyze the reaction conditions and Le Chatelier's principle.

Le Chatelier's principle states that when a system at equilibrium is subjected to a change in conditions, it will shift to counteract the change and reach a new equilibrium.

a. CO(g) + 2H2(g) ⇌ CH3OH(g)
This reaction represents the synthesis of methanol. According to Le Chatelier's principle, if we increase the pressure, the reaction will shift in the direction that reduces the number of moles of gas. Since there are fewer moles of gas on the right-hand side of the equation (1 molecule of gas), an increase in pressure would favor the forward reaction, resulting in an increase in the amount of product (CH3OH).

b. 2SO2(g) + O2(g) ⇌ 2SO3(g)
This reaction represents the formation of sulfur trioxide. Increasing the pressure in this case would favor the reaction that reduces the number of moles of gas. Since there are fewer moles of gas on the left-hand side of the equation (3 molecules of gas), an increase in pressure would favor the reverse reaction, resulting in a decrease in the amount of product (SO3).

c. COCl2(g) ⇌ CO(g) + Cl2(g)
This reaction represents the decomposition of carbonyl chloride. Increasing the pressure would favor the reaction that reduces the number of moles of gas. In this case, there are the same number of moles of gas on both sides of the equation (2 molecules of gas). Therefore, changing the pressure by altering the volume would not significantly affect the amounts of products.

In summary:
- Increasing pressure (by decreasing volume) would increase the amount of product (CH3OH) in reaction (a) and decrease the amount of product (SO3) in reaction (b).
- Changing the pressure by altering the volume would not significantly affect the amounts of products in reaction (c).