Given the reaction at equilibrium: 2CO(g) + O\(_2\)(g) \(\iff\) 2CO\(_2\)(g) When the reaction is subjected...
When the reaction is subjected to stress, a change will occur in the concentration of
- A) reactants, only
- B) products, only
- C) both reactants and products
- D) neither reactants nor products
Correct Answer: C) both reactants and products
Explanation
The given reaction is:
2CO(g) + O\(_2\)(g) \(\iff\) 2CO\(_2\)(g)
This reaction is at equilibrium, which means that the rate of the forward reaction (formation of CO\(_2\) is equal to the rate of the reverse reaction (formation of CO and O\(_2\).
According to Le Chatelier's principle, when a system at equilibrium is subjected to stress (such as change in pressure, temperature, or concentration), the system will adjust itself in order to partially counteract the applied stress and restore a new equilibrium.
In this case, when the reaction is subjected to stress, the system will try to counteract the stress by shifting the equilibrium position either to the right (favoring the forward reaction) or to the left (favoring the reverse reaction). This shifting will cause a change in the concentration of both reactants (CO and O\(_2\) and products (CO\(_2\).
Therefore, the correct answer isOption C: both reactants and products, as their concentrations will change when the system tries to restore equilibrium after being subjected to stress.