Equilibrium Expressions and Concentrations

The video tutorial addresses a problem involving equilibrium constants. It begins by introducing a chemical reaction and setting up the problem with given conditions. The instructor explains how to write the equilibrium expression and interpret the equilibrium constant (KC). The tutorial then demonstrates solving the problem using algebraic methods, calculating the equilibrium concentrations of the reactants and products. The video emphasizes understanding the direction of the equilibrium shift and the algebraic manipulation required to find the solution.

What is the initial concentration of each gas in the container?

• 3 moles per liter

• 0.5 moles per liter

• 2 moles per liter

• 1 mole per liter

What does an equilibrium constant greater than 1 indicate about the reaction?

• More reactants than products

• More products than reactants

• Equal amounts of reactants and products

• No reaction occurs

In the equilibrium expression, which components are placed in the numerator?

• Products

• Inert gases

• Catalysts

• Reactants

Which direction does the equilibrium shift when the constant is 16?

• Both directions

• To the right

• To the left

• No shift

What is the algebraic expression used to represent the change in concentration of SO3 and NO?

• 1 - x

• x + 1

• 1 + x

• x - 1

How is the equilibrium constant expression simplified using perfect squares?

• By adding the squares

• By subtracting the squares

• By taking the square root

• By multiplying the squares

What is the value of x after solving the algebraic equation?

• 0.3

• 1.2

• 0.6

• 0.9

How many moles of NO2 are present at equilibrium?

• 1.6 moles

• 1.0 moles

• 0.6 moles

• 0.4 moles

What is the concentration of NO at equilibrium?

• 1.6 M

• 0.4 M

• 1.0 M

• 0.6 M

What happens to the concentration of reactants as the equilibrium shifts to the right?

• It increases

• It decreases

• It remains the same

• It doubles