Practice Problem: Calculating Equilibrium Concentrations

Professor Dave explains how to calculate equilibrium concentrations using a chemical reaction involving nitrogen and hydrogen to form ammonia. He sets up the problem by providing the concentrations of nitrogen and hydrogen and the equilibrium constant. He then explains how to form the equilibrium constant expression and solve for the unknown ammonia concentration using arithmetic.

What are the given concentrations of nitrogen and hydrogen in the equilibrium problem?

• Nitrogen: 1.50 M, Hydrogen: 3.00 M

• Nitrogen: 4.26 M, Hydrogen: 2.09 M

• Nitrogen: 3.00 M, Hydrogen: 1.50 M

• Nitrogen: 2.09 M, Hydrogen: 4.26 M

What is the equilibrium constant for the given reaction?

• 6.000

• 0.0060

• 0.6000

• 0.0600

How is the equilibrium constant expression set up for this reaction?

• Concentration of NH3 squared over concentration of N2 times concentration of H2 cubed

• Concentration of N2 squared over concentration of NH3 times concentration of H2 cubed

• Concentration of NH3 cubed over concentration of N2 squared times concentration of H2

• Concentration of H2 cubed over concentration of NH3 squared times concentration of N2

What is the stoichiometric coefficient of hydrogen in the equilibrium expression?

• 4

• 3

• 2

• 1

What is the calculated equilibrium concentration of NH3?

• 0.53 M

• 2.53 M

• 1.53 M

• 3.53 M