Question

Consider the following equilibrium: H2O(g) + CO(g) H2(g) + CO2(g) A closed container is initially filled with H2O and CO. Which of the following correctly describes the reaction as it proceeds towards equilibrium?

A.The [CO] and [CO2] both increase.

B.The [CO] decreases and [CO2] increases.

C.The [CO] increases and [CO2] decreases.

D.The [CO] and [CO2] both decrease.

Answer 1

The answer is b. The H2O and CO have to decrease in order to produce the CO2 and H2

Answer 2

Answer : The correct option is, (B) The
`[CO]` decreases and
`[CO_2]` increases.

Explanation :

According to the Le-Chatelier's principle, if any changes occurs in the variables of the reaction then the equilibrium will be shift in that direction where the effect is minimum.

When the concentration of the reactant increases then the equilibrium will be shift in the forward direction and when the concentration of the reactant decreases then the equilibrium will be shift in the backward or reverse direction.

As per question, when a closed container is initially filled with
`H_2O` and CO then the concentration of reactants
`(H_2O\text{ and }CO)` would decreases and concentration of
`(H_2\text{ and }CO_2)` would increases.

Hence, the correct option is, (B) The
`[CO]` decreases and
`[CO_2]` increases.