Equilibrium Regents

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

Ammonia is produced commercially by the Haber reaction:   N_{2 (g)} + 3 H_{2 (g)} -->  2 NH_{3 (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) + Heat
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

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

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.

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

Consider the following equilibrium system:
CaCO_3(s) ⇄ CaO_(s) + CO_2(g) 
Which one of the following changes would cause the above system to shift left?

• Add more CaO
• Remove CO₂
• Add CaCO₃
• Add a catalyst

Tags

NGSS.HS-PS1-5

Identify the INCORRECT statement about achieving equilibrium.

• achieved when product and reactant concentration is equal
• achieved when forward + reverse rxn rates are same
• achieved when concentration of reactants is constant
• achieved when rxn quotient Q = equilibrium constant

At what time (in seconds) is equilibrium established?

• 0 seconds
• 1 second
• 5 seconds
• 10 seconds