Equilibrium Calculations Quiz

What happens to concentrations when a system is not at equilibrium?

• They decrease to zero.

• They remain constant.

• They increase indefinitely.

• They change until equilibrium is reached.

In the decomposition of ammonia, if nitrogen concentration increases by 0.11 mol, what is the change in hydrogen concentration?

• 0.33 mol

• 0.22 mol

• 0.44 mol

• 0.11 mol

What does the ICE in ICE box stand for?

• Initial, Change, Equilibrium

• Initial, Concentration, End

• Increase, Change, End

• Increase, Concentration, Equilibrium

How do you calculate the equilibrium constant (K) if you know all equilibrium concentrations?

• Add all concentrations together.

• Multiply all concentrations together.

• Plug them into the equilibrium constant expression.

• Divide the largest concentration by the smallest.

If you know the equilibrium constant (K) and some equilibrium concentrations, how can you find an unknown concentration?

• Guess the value.

• Use the reaction quotient expression.

• Use the stoichiometric coefficients.

• Use the ICE box method.

What is the first step in calculating equilibrium concentrations from non-equilibrium concentrations?

• Determine the direction of the reaction.

• Measure the initial concentrations.

• Find the equilibrium constant (K).

• Calculate the reaction quotient (Q).

How do you determine the direction in which a reaction will proceed to reach equilibrium?

• By observing the color change.

• By measuring the temperature.

• By comparing Q to K.

• By checking the pressure.

What happens if Q is smaller than K?

• The reaction will move to generate products.

• The reaction will move to generate reactants.

• The reaction will reverse.

• The reaction will stop.

What is the purpose of using an ICE box in equilibrium calculations?

• To store chemicals safely.

• To organize initial, change, and equilibrium data.

• To cool down the reaction.

• To increase the reaction rate.

Why is it important to check your arithmetic after calculating equilibrium concentrations?

• To make sure the concentrations are equal.

• To verify the reaction has stopped.

• To confirm the calculated K matches the expected K.

• To ensure the values are positive.