Solutions and Equilibrium

Given the equation representing a reaction at equilibrium: 
N₂(g) + 3H₂(g) --> 2NH₃(g) + energy
Which change causes the equilibrium to shift to the right?

• decreasing the concentration of H₂(g)
• decreasing the pressure
• increasing the concentration of N₂(g)
• increasing the temperature

Tags

NGSS.HS-PS1-5

NGSS.HS-PS1-6

Given the reaction at equilibrium:
A(g) + B(g) <=> A₂B₃(g)
Which change will not affect the equilibrium concentrations of A(g), B(g), and A₂B₃(g)?

• adding more A(g)
• adding a catalyst
• increasing the temperature
• increasing the pressure

Tags

NGSS.HS-PS1-6

Ammonia is produced commercially by the Haber reaction:   N₂ (g) + 3 H₂ (g) -->  2 NH₃ (g)
The formation of ammonia is favored by

• an increase in pressure
• a decrease in pressure
• removal of N₂(g)
• removal of H₂(g)

Given the reaction at equilibrium:
2H₂(g) + O₂(g) ↔ 2H₂O(g) + energy
Which concentration changes occur when the temperature of the system is increased?

• The [H₂] decreases and the [O₂] decreases.
• The [H₂] decreases and the [O₂] increases.
• The [H₂] increases and the [O₂] decreases.
• The [H₂] increases and the [O₂] increases.

Tags

NGSS.HS-PS1-5

NGSS.HS-PS1-6

Given the reaction at equilibrium:
AgCl(s) ↔ Ag⁺(aq) + Cl^-(aq)
The addition of Cl^- ions will cause the concentration of Ag⁺(aq) to

• decrease as the amount of AgCl(s) decreases
• decrease as the amount of AgCl(s) increases
• increase as the amount of AgCl(s) decreases
• increase as the amount of AgCl(s) increases

Tags

NGSS.HS-PS1-5

NGSS.HS-PS1-6

Which statement is true for a saturated solution?

• It must be a concentrated solution.
• It must be a diluted solution.
• Neither dissolving nor crystallizing is occurring.
• The rate of dissolving equals the rate of crystallizing.

In which reaction at equilibrium will the point of equilibrium shift to the right when the pressure decreases at constant temperature?

• N₂(g) + 3H₂(g) ↔ 2NH₃(g)
• H₂(g) + Br₂(g) ↔ 2HBr(g)
• CaCO₃(s) ↔ CaO(s) + CO₂(g)
• N₂(g) + O₂(g) ↔ 2NO(g)

Tags

NGSS.HS-PS1-6

Given the reaction at equilibrium:
N₂(g) + 3H₂(g) ↔ 2NH₃(g)
Increasing the concentration of N₂(g) will increase the forward reaction rate due to

• a decrease in the number of effective collisions
• an increase in the number of effective collisions
• a decrease in the activation energy
• an increase in the activation energy

Tags

NGSS.HS-PS1-5

Given the reaction at equilibrium:
N₂(g) + O₂(g) ↔ 2NO(g)
As the concentration of N₂(g) is increased, the concentration of O₂(g) will

• decrease
• increase
• remain the same

Tags

NGSS.HS-PS1-5

Given the reaction system in a closed container at equilibrium and at a temperature of 298 K:
N₂O₄ (g)  <-->  2NO₂ (g)
The measurable quantities of the gases at equilibrium must be

• decreasing
• increasing
• equal
• constant

Tags

NGSS.HS-PS1-6