Equilibrium Expressions and ICE Tables

This video tutorial explains how to solve an ICE table problem to find the equilibrium constant for a reaction involving nitrogen, hydrogen, and ammonia. It covers the initial conditions, the process of determining equilibrium concentrations, and the calculation of the equilibrium constant using the ICE table method. The tutorial emphasizes the importance of understanding initial concentrations and changes in concentration to solve for the equilibrium constant accurately.

What are the initial concentrations of nitrogen and ammonia in the reaction?

• 0.75 molar nitrogen and 0.45 molar ammonia

• 0.45 molar nitrogen and 0.75 molar ammonia

• 0.30 molar nitrogen and 0.75 molar ammonia

• 0.75 molar nitrogen and 0.30 molar ammonia

Why is it possible for the reaction to proceed even without initial hydrogen?

• Because the reaction is spontaneous

• Because the system will reach equilibrium regardless of initial conditions

• Because hydrogen is not needed for the reaction

• Because ammonia decomposes to form hydrogen

What is the significance of the squiggly line under the arrows in the ICE table?

• It indicates the direction of the reaction

• It helps in visualizing the change in concentrations

• It separates reactants from products

• It denotes the equilibrium state

How do the coefficients in the balanced equation affect the change in concentrations?

• They dictate the ratio of change in concentrations

• They are used to calculate the equilibrium constant

• They have no effect on the change in concentrations

• They determine the initial concentrations

What is the value of x in the ICE table calculations?

• 0.30 molar

• 0.10 molar

• 0.15 molar

• 0.20 molar

What is the equilibrium concentration of nitrogen after solving the ICE table?

• 0.95 molar

• 0.85 molar

• 0.65 molar

• 0.75 molar

What is the equilibrium concentration of ammonia after solving the ICE table?

• 0.15 molar

• 0.35 molar

• 0.45 molar

• 0.25 molar

What is the purpose of writing the equilibrium expression?

• To find the equilibrium constant (Kc)

• To determine the initial concentrations

• To balance the chemical equation

• To calculate the change in concentrations

What is the final equilibrium constant (Kc) for the reaction?

• 2.0

• 1.8

• 3.5

• 2.7

Why are the coefficients used as exponents in the equilibrium expression?

• To represent the stoichiometry of the reaction

• To balance the equation

• To simplify the calculation

• To adjust the units of concentration