Quiz for Le Chatelier’s principle

Q1: Le Chatelier’s principle is used to predict the effect of:

A. Change in temperature, pressure, concentration B. Only change in temperature C. Only change in pressure D. Only change in volume

Q2: If concentration of reactants increases, equilibrium will:

A. Shift towards products B. Shift towards reactants C. Remain unchanged D. Reaction stops

Q3: Increasing pressure on gaseous equilibrium favors:

A. Side with fewer moles of gas B. Side with more moles of gas C. No change D. Equilibrium breaks

Q4: Decreasing temperature in an exothermic reaction shifts equilibrium:

A. Towards products B. Towards reactants C. No change D. Equilibrium disappears

Q5: Removing a product at equilibrium causes:

A. Shift towards products B. Shift towards reactants C. No change D. Reaction stops

Q6: Adding a catalyst:

A. Does not shift equilibrium B. Shifts equilibrium to reactants C. Shifts equilibrium to products D. Stops reaction

Q7: Which condition is NOT explained by Le Chatelier’s principle?

A. Adding inert gas at constant volume B. Changing temperature C. Changing pressure D. Changing concentration

Q8: Increase in volume of gaseous system shifts equilibrium:

A. Towards side with more moles B. Towards side with fewer moles C. No change D. Reaction stops

Q9: In an endothermic reaction, increasing temperature shifts equilibrium:

A. Towards products B. Towards reactants C. No change D. Equilibrium destroyed

Q10: Which of the following does NOT change equilibrium position?

A. Adding a catalyst B. Changing concentration C. Changing temperature D. Changing pressure

Q11: If system is at equilibrium and temperature is raised for exothermic reaction, equilibrium:

A. Shifts left towards reactants B. Shifts right towards products C. Remains unchanged D. Reaction stops

Q12: Le Chatelier’s principle applies to:

A. Reversible reactions at equilibrium B. Irreversible reactions C. Physical changes only D. None of the above

Q13: When pressure is decreased in gaseous equilibrium, reaction shifts:

A. Towards side with more moles B. Towards side with fewer moles C. No shift D. Equilibrium breaks

Q14: Removing reactant from equilibrium causes:

A. Shift towards reactants B. Shift towards products C. No change D. Reaction stops

Q15: What happens when an inert gas is added at constant pressure?

A. Volume increases, equilibrium shifts B. No change C. Reaction speeds up D. Equilibrium breaks

Q16: Le Chatelier’s principle helps in:

A. Predicting effect of external changes on equilibrium B. Calculating K value C. Measuring reaction rates D. Determining molecular weight

Q17: Which of the following shifts equilibrium towards reactants?

A. Increase in temperature in exothermic reaction B. Increase in temperature in endothermic reaction C. Increase in concentration of reactants D. Increase in pressure

Q18: Which factor does not affect equilibrium constant?

A. Pressure change B. Temperature change C. Addition of catalyst D. Concentration change

Q19: Which is an example where Le Chatelier’s principle is applied?

A. Haber process for ammonia synthesis B. Combustion of methane C. Freezing of water D. Dissolution of salt in water

Q20: At equilibrium, if temperature is decreased in endothermic reaction:

A. Equilibrium shifts to reactants B. Equilibrium shifts to products C. No change D. Reaction stops