Methanol has the formula CH₃OH and can be produced by the reaction of carbon monoxide with hydrogen gas.
CO + 2 H₂ ? CH₃OH + heat
Using the above chemical reaction, determine how each of the following actions would affect the equilibrium of the system.
a. heating the mixture
b. adding an excess of carbon monoxide
c. removing the methanol as it is formed
d. adding a substance that reacts with carbon monoxide

Answer in explanation

Explanation:

A. Heating the mixture

Before we can explain the effect of a temperature increase, we need to know the type of reaction it is on temperature basis. As heat is produced, this type of reaction is an exothermic reaction. An exothermic reaction is one in which heat is released into the environment. As such, increasing the temperature of an exothermic reaction leads to more reactants being formed. The equilibrium will thus favor the backward reaction

B. Adding an excess of carbon monoxide

This means we are adding more reactants to the mix. This causes an increase in the available reactants necessary for the reaction to take place making it possible for more product to be formed. This thus favors the forward reaction

C. Removing the methanol as it is formed also favors the forward reaction. This favors the forward reaction as there is allocation for more product to be formed

D. Adding a substance that reacts with carbon ii oxide means less reactant availability which makes it possible for the equilibrium to favor the backward reaction as less reactant is available to give more product.

5.6⋅10−^19  j

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