Equilibrium Mixed Practice

What are the two factors to look for when determining if the reaction is at equilibrium?

• Forward reaction rate is faster than the reverse and concentrations of reactants and products are equal

• Forward and reverse reaction rates are equal and concentrations of reactant and products are constant

• Forward and reverse reaction rates are equal and concentrations of reactants and products are equal

• Forward reaction rate is faster than the reverse and concentrations of reactants and products are equal

Tags

NGSS.HS-PS1-6

Select all of the statements that are always correct about dynamic equilibrium

• established when the product and reactant concentrations are equal

• achieved when the forward and reverse reaction rates are same

• established when the concentration of reactants is unchanging

• achieved when the concentration ratio of reactants to products becomes stable

• achieved when the forward and reverse reactions stop occurring

At what time did the reaction establish equilibrium?

• t₁

• t₂

• t₃

• t₄

Given the equation representing a reaction:

N₂O_4(g) ⇌ 2NO_2(g)

Which statement describes this reaction at equilibrium?

• The concentration of N₂O₄(g) must equal the concentration of NO₂(g).

• The concentration of N₂O₄(g) and the concentration of NO₂(g) must be constant.

• The rate of the forward reaction is greater than the rate of the reverse reaction.

• The rate of the reverse reaction is greater than the rate of the forward reaction.

The statement that if a system at equilibrium is disturbed, the reaction will proceed in one direction or another in order to reestablish equilibrium, is known as:

• the principle of equilibrium

• Priestley’s principle

• Le Chatelier’s principle

• Faraday’s principle

• the law of mass action

Tags

NGSS.HS-PS1-6

Consider the reversible reaction

N₂ (g) + O₂ (g) + 181 kJ ⇌ 2NO (g). Adding O₂ will...

• shift the equilibrium left and increase [NO]

• shift the equilibrium right and increase [NO]

• shift the equilibrium left and decrease [NO]

• shift the equilibrium right and decrease [NO]

Tags

NGSS.HS-PS1-5

Consider the reversible reaction

N₂ (g) + O₂ (g) + 181 kJ ⇌ 2NO (g).

If N₂ is removed...

• the equilibrium will shift right, creating more products.

• the equilibrium will shift right, creating more reactants.

• the equilibrium will shift left, creating more products.

• The equilibrium will shift left, creating more reactants.

Tags

NGSS.HS-PS1-6

Consider the reversible reaction

N₂ (g) + O₂ (g) + 181 kJ ⇌ 2NO (g). Which change will increase the amount of N₂ at equilibrium?

• decreasing the pressure

• adding a catalyst.

• decreasing the temperature.

• adding O₂

• increasing the temperature

Consider the reversible reaction:

CO (g) + 2H₂ (g) ⇌ CH₃OH (g) + energy. Cooling the reaction mixture will ___.

• shift the equilibrium to the right and increase [CH₃OH]

• shift the equilibrium to the left and increase [CH₃OH]

• shift the equilibrium to the left and decrease [CH₃OH]

• shift the equilibrium to the right and decrease [CH₃OH]

Tags

NGSS.HS-PS1-5

Consider the reversible reaction:

CO (g) + 2H₂ (g) ⇌ CH₃OH (g) + energy. Adding a catalyst will____.

• have no effect on the equilibrium position

• shift the equilibrium to the left

• shift the equilibrium to the right

• increase the activation energy of the forward reaction

Tags

NGSS.HS-PS1-6