Effect of inert gas on chemical equilibrium

The video tutorial explains an experiment involving a piston-fitted chamber and inert gas. It focuses on a catalytic methanation reaction at constant volume and temperature. The addition of helium gas increases molecular collisions and total pressure but does not affect the partial pressures of individual gases, maintaining chemical equilibrium. The conclusion is that adding inert gas does not alter the equilibrium state.

What is the role of the piston-fitted chamber in the experiment?

• To measure the temperature of the reaction

• To maintain constant volume during the reaction

• To add reactants to the reaction

• To remove products from the reaction

How does the addition of helium gas affect the total pressure in the container?

• It decreases the partial pressure of reactants

• It has no effect on the total pressure

• It increases the total pressure

• It decreases the total pressure

Why do the partial pressures of individual gases remain constant when helium is added?

• Because the volume of the container increases

• Because the temperature of the reaction decreases

• Because the molar fraction of gases remains unchanged

• Because the reaction rate increases

What remains unchanged in the reaction when inert gas is added?

• The concentration of reactants and products

• The total volume of the container

• The temperature of the reaction

• The catalyst used in the reaction

What conclusion can be drawn about the effect of inert gas on chemical equilibrium?

• Inert gas shifts the equilibrium towards the products

• Inert gas shifts the equilibrium towards the reactants

• Inert gas increases the rate of reaction

• Inert gas has no effect on chemical equilibrium