Consider the reaction below. CO (g) + Cl2 (g) " COCl2 (g) What is the most likely effect to the forward reaction if there is an increase in pressure on this reaction? The reactant surface area increases. The reaction rate decreases. The reaction is not affected at all. The reaction stops completely.

Answer: the reaction rate of the forward reaction increases (although it is not among the options shown).

Explanation:

1) The equation given is:

CO (g) + Cl₂ (g) ⇄ COCl₂ (g)

2) The forward reaction is:

CO (g) + Cl₂ (g) → COCl₂ (g)

3) The stoichiometry is 1 mole + 1 mole → 1 mole

4) Analysis and conclusion:

The effect of change in the conditions of an equilibrium is foreseen using Le Chatelier's principle.

Le Chatelier's principle states that a system in equilibrium will act trying to compensate the distress applied to the system.

In this case, the distress is increase in pressure.

To compensate the increase in pressure the system must act by reducing the number of moles in the system. Since the forward reaction implies the conversion of two moles of reagents into one mole of product, the more the forward reaction progress the less the number of moles will be present in the system and so the more the compensation of the increase in pressure. So the forward raction is favored by the increase in pressure.

Favoring the forwar reaction means that its rate will incrase,