Equilibrium Shifts in Chemical Reactions

This video tutorial explains how changes in volume and pressure affect chemical equilibrium, focusing on the inverse relationship between these two factors. It discusses how to predict the direction of equilibrium shifts by examining the moles of gas on each side of a reaction. The video also covers the effects of catalysts and inert gases, emphasizing that they do not alter equilibrium. Finally, it provides practice questions to reinforce understanding of these concepts.

What happens to the volume of a system when the pressure is increased?

• The volume increases.

• The volume decreases.

• The volume remains the same.

• The volume fluctuates.

When the volume of a container is increased, to which side does the equilibrium shift?

• To the side with more liquids.

• To the side with more solids.

• To the side with more moles of gas.

• To the side with fewer moles of gas.

If the volume of a container is decreased, what happens to the equilibrium?

• It shifts to the side with fewer moles of gas.

• It shifts to the side with more moles of gas.

• It shifts to the side with more liquids.

• It shifts to the side with more solids.

In the reaction N2O4 decomposing into 2NO2, what happens if the volume is increased?

• The reaction stops.

• The reaction shifts to the left.

• The reaction shifts to the right.

• The reaction remains unchanged.

For the reaction H2 + Cl2 → 2HCl, what happens to the equilibrium when volume changes?

• It shifts to the left.

• It shifts to the right.

• It depends on the temperature.

• There is no shift.

What is the effect of adding a catalyst to a system already at equilibrium?

• It shifts the equilibrium to the left.

• It increases the pressure.

• It has no effect on the equilibrium.

• It shifts the equilibrium to the right.

What happens when an inert gas is added to a system at equilibrium?

• The equilibrium shifts to the left.

• The reaction rate increases.

• The equilibrium remains unchanged.

• The equilibrium shifts to the right.

If the temperature is increased in an endothermic reaction, which way does the equilibrium shift?

• To the left.

• It remains unchanged.

• It depends on the pressure.

• To the right.

When the volume is increased in a reaction with 4 moles of reactant gas and 5 moles of product gas, which way does the equilibrium shift?

• To the right.

• It depends on the temperature.

• To the left.

• It remains unchanged.

What happens to the equilibrium if HCl is added to the reaction H2 + Cl2 → 2HCl?

• It depends on the volume.

• It remains unchanged.

• It shifts to the left.

• It shifts to the right.