Question

Base your answer on the information below and your knowledge of chemistry. Methanol can be manufactured by a reaction that is reversible. In the reaction, carbon monoxide gas and hydrogen gas react using a catalyst. The equation below represents this system at equilibrium. CO(g) 2H2(g) CH3OH(g) energy. Explain, in terms of collision theory, why increasing the concentration of H2(g) in this system will increase the concentration of CH3OH(g).

Answer 1

Step-by-step explanation:

For the given reaction:

Rate law says that rate of a reaction is directly proportional to the concentration of the reactants each raised to a stoichiometric coefficient determined experimentally called as order.

`CO(g)+2H_2(g)\rightarrow CH_3OH(g)`

`Rate=k[CO]^x[H_2]^y`

where x and y are order wrt to
`CO` and
`H_2`

According to collision theory , the molecules must collide for a reaction to take place. According to collision theory , the rate of a reaction is proportional to rate of collision of reactants.

Thus with an increase in concentration of reactants , the rate of reaction also increases. This is because if the concentration of reactants increases , the chances of collision between molecules also increases and thus more products wil be formed which in turn increases the rate of reaction.