Question

When an inert gas, such as helium, is added to a system at equilibrium (1) No cffect on the cquilibrium would occur. (2) The product would be favoured. (3) It would cffect cquilibrium only if it produces changes in concentration (or partial pressurcs) of the reactants or products. (4) It would effcet cquilibrium only if it reacts with onc of the substances involved in the equilibrium.

Short answer

No effect on equilibrium would occur because inert gases do not change concentrations or partial pressures of the reactants or products.

Step-by-step solution

Identify the types of changes that could impact equilibrium

Understand that equilibrium can be affected by changes in concentration, pressure, volume, or temperature of the reactants and products. Determine if the inert gas addition changes any of these parameters.

Consider the role of an inert gas in the system

Inert gases do not react with any substances in the reaction. Thus, they do not directly alter the concentration of reactants or products in equilibrium.

Analyze the effect of inert gas on partial pressure

Adding an inert gas increases the total pressure, but not the partial pressures of the reactants or products assuming volume remains constant. This means there is no shift in equilibrium according to Le Chatelier's principle.

Conclude the specific impacts on the equilibrium

Since the inert gas does not affect the concentration or partial pressure of the reactants or products, it will not influence the equilibrium position.

Key concepts

Le Chatelier's Principle

Le Chatelier's Principle helps predict how a system at equilibrium reacts when disturbed. It states that if a stress, such as a change in concentration, temperature, or pressure, is applied to a system at equilibrium, the system will adjust to counteract the stress and restore a new equilibrium.
For example, if the concentration of a reactant is increased, the system will favor the forward reaction to reduce the concentration of that reactant.
Le Chatelier's Principle is crucial for understanding how chemical reactions respond to external changes and finding the optimal conditions for a desired product.

Effect of Inert Gases

Inert gases, like helium, do not react with substances involved in the chemical equilibrium. When added to a closed system at constant volume, the inert gas increases the total pressure but does not affect the partial pressures of the reactants or products.
Because inert gases do not change the concentration of reactants or products, they do not cause the system to shift its equilibrium position.
In summary, the addition of an inert gas has a negligible effect on the equilibrium, as it doesn't alter the conditions that drive the direction of the reaction.

Partial Pressure

Partial pressure is the pressure exerted by a single type of gas in a mixture of gases. For a gas in a mixture, its partial pressure is proportional to its mole fraction multiplied by the total pressure.
In chemical equilibrium, the partial pressures of reactants and products are vital for determining the direction and extent of the reaction according to the equilibrium constant, Kp.
If partial pressures of reactants or products change, the system will shift its equilibrium position to balance the changes, following Le Chatelier's Principle.

Chemical Equilibrium

Chemical equilibrium occurs when the rates of the forward and reverse reactions are equal, resulting in no net change in the concentrations of reactants and products.
At equilibrium, the reaction quotient, Q, equals the equilibrium constant, K. This indicates a stable state where the proportions of reactants and products remain constant over time, despite ongoing reactions at the molecular level.
Disturbances to the system, such as changes in concentration, temperature, or pressure (excluding inert gases), can shift the equilibrium position, prompting the system to re-establish balance.