Equilibrium Shifts and Stressors Quiz

• Shifts to produce more product

• Shifts to produce more reactant

• No change

• Cannot be determined

Answer explanation

According to Le Chatelier's principle, increasing the concentration of a reactant (N2) shifts the equilibrium to the right, favoring the production of more product (NH3). Thus, the equilibrium shifts to produce more product.

Tags

NGSS.HS-PS1-5

• Shifts to produce more product

• Shifts to produce more reactant

• No change

• Cannot be determined

Answer explanation

Increasing the temperature of an exothermic reaction shifts the equilibrium to favor the reactants, as the system tries to absorb the added heat. Therefore, the position of equilibrium shifts to produce more reactant.

• Shifts to produce more product

• Shifts to produce more reactant

• No change

• Cannot be determined

Answer explanation

In this reaction, there are 2 moles of gas on the left (H2 and I2) and 2 moles on the right (2HI). Increasing pressure by decreasing volume affects the equilibrium only if there is a difference in moles of gas, which there isn't here. Thus, no change occurs.

Tags

NGSS.HS-PS1-6

• Shifts to produce more product

• Shifts to produce more reactant

• No change

• Cannot be determined

Answer explanation

Decreasing the concentration of NO2 shifts the equilibrium to the left, according to Le Chatelier's principle, to produce more reactants (NO2) in order to counteract the change.

Tags

NGSS.HS-PS1-5

• Shifts to produce more product

• Shifts to produce more reactant

• No change

• Cannot be determined

Answer explanation

Increasing the temperature of an endothermic reaction shifts the equilibrium to the right, favoring the production of more products (CaO and CO2) to absorb the added heat, thus producing more product.

Tags

NGSS.HS-PS1-6

• Shifts to produce more product

• Shifts to produce more reactant

• No change

• Cannot be determined

Answer explanation

Decreasing pressure by increasing volume shifts the equilibrium towards the side with more moles of gas. In this reaction, there are 3 moles of reactants (2H2 + O2) and 2 moles of products (2H2O). Thus, it shifts to produce more reactants.

Tags

NGSS.HS-PS1-6

• Shifts to produce more product

• Shifts to produce more reactant

• No change

• Cannot be determined

Answer explanation

Adding more H2O increases its concentration, shifting the equilibrium to the right to produce more products (CO and H2) according to Le Chatelier's principle.

Tags

NGSS.HS-PS1-5

• Shifts to produce more product

• Shifts to produce more reactant

• No change

• Cannot be determined

Answer explanation

For an endothermic reaction, heat is absorbed. Decreasing temperature shifts the equilibrium to the left, favoring the reactants (N2 and O2) to produce more reactants and less product (NO). Thus, it shifts to produce more reactant.

• Shifts to produce more product

• Shifts to produce more reactant

• No change

• Cannot be determined

Answer explanation

Increasing pressure shifts the equilibrium towards the side with fewer moles of gas. In this case, the left side (PCl5) has 1 mole, while the right side (PCl3 + Cl2) has 2 moles. Thus, the equilibrium shifts to produce more reactant.

• Shifts to produce more product

• Shifts to produce more reactant

• No change

• Cannot be determined

Answer explanation

Increasing the concentration of N2O4 shifts the equilibrium to the left, according to Le Chatelier's principle, to counteract the change. This results in the production of more reactants (NO2).

Tags

NGSS.HS-PS1-5