Question

A chemical equilibrium between gaseous reactants and products is shown.

N2(g) + 3H2(g) ⇌ 2NH3(g)


How will the reaction be affected if the pressure on the system is decreased?


It will shift toward the reactant side as there is lower pressure on the reactant side.


It will shift toward the product side as there is higher pressure on the product side.


It will shift toward the reactant side as there are a greater number of moles of gas on the reactant side.


It will shift toward the product side as there are a fewer number of moles of gas on the product side.




Question 2 (Worth 2 points)


(07. 07 LC)


According to Le Châtelier's principle, an increase in temperature will shift the equilibrium position toward the products in an endothermic reaction.


True


False




Question 3 (Worth 3 points)


(07. 07 MC)


Match the action to the effect on the equilibrium position for the reaction N2(g) + 3H2(g) ⇌ 2NH3(g).


Match Term Definition

Decreasing the pressure A) Shift to the left

Adding hydrogen gas B) Shift to the right

Adding a catalyst C) No effect



Question 4 (Worth 3 points)


(07. 07 MC)


What change would shift the equilibrium system to the left?


A(g) + B(s) + Energy ⇌ 3C(g)


Adding more of gas C to the system


Heating the system


Increasing the volume


Removing some of gas C from the system


Points earned on this question: 3


Question 5 (Worth 3 points)


(07. 07 MC)


What stress would shift the equilibrium position of the following system to the left?


N2O3(g) ⇌ NO(g) + NO2(g); ΔH is negative



Decreasing the concentration of N2O3


Heating the system


Adding a catalyst


Increasing the concentration of NO




Question 6 (Worth 3 points)


(07. 07 MC)


Nitrogen dioxide gas is dark brown in color and remains in equilibrium with dinitrogen tetroxide gas, which is colorless.


2NO2(g) ⇌ N2O4(g)


When a light brown colored mixture of the two gases at equilibrium was moved from room temperature to a higher temperature, the mixture turned dark brown in color. Which of the following conclusions about this equilibrium mixture is true?


This reaction is exothermic because the system shifted to the left on heating.


This reaction is exothermic because the system shifted to the right on heating.


This reaction is endothermic because the system shifted to the left on heating.


This reaction is endothermic because the system shifted to the right on heating.




Question 7 (Worth 3 points)


(07. 07 LC)


According to Le Châtelier's principle, how will a decrease in concentration of a reactant affect the equilibrium system?


Shift it toward the products


Shift it toward the reactants


Shift it toward the side with higher total mole concentration


Shift it toward the side with lower total mole concentration

Answer 1

Question 1: How will the reaction be affected if the pressure on the system is decreased?

It will shift toward the reactant side as there is a lower pressure on the reactant side.

Question 2: According to Le Châtelier's principle, an increase in temperature will shift the equilibrium position toward the products in an endothermic reaction.

True

Question 3: Match the action to the effect on the equilibrium position for the reaction N2(g) + 3H2(g) ⇌ 2NH3(g).

Decreasing the pressure: A) Shift to the left

Adding hydrogen gas: B) Shift to the right

Adding a catalyst: C) No effect

Question 4: What change would shift the equilibrium system to the left?

A(g) + B(s) + Energy ⇌ 3C(g)

Removing some of gas C from the system

Question 5: What stress would shift the equilibrium position of the following system to the left?

N2O3(g) ⇌ NO(g) + NO2(g); ΔH is negative

Increasing the concentration of N2O3

Question 6: Nitrogen dioxide gas is dark brown in color and remains in equilibrium with dinitrogen tetroxide gas, which is colorless.

2NO2(g) ⇌ N2O4(g)

When a light brown colored mixture of the two gases at equilibrium was moved from room temperature to a higher temperature, the mixture turned dark brown in color. Which of the following conclusions about this equilibrium mixture is true?

This reaction is endothermic because the system shifted to the right on heating.

Question 7: According to Le Châtelier's principle, how will a decrease in concentration of a reactant affect the equilibrium system?

Shift it toward the products

Answer 2

The answer is: It will shift the equilibrium toward the reactants.

Step-by-step explanation:

For the given questions related to chemical equilibrium and Le Châtelier's principle, here are the answers:

Question 1: How will the reaction be affected if the pressure on the system is decreased?

The answer is: It will shift toward the side with fewer moles of gas, which is the reactant side. Therefore, the correct option is: "It will shift toward the reactant side as there are a greater number of moles of gas on the reactant side."

Question 2: According to Le Châtelier's principle, an increase in temperature will shift the equilibrium position toward the products in an endothermic reaction.

The answer is: True. An increase in temperature favors the endothermic reaction, so the equilibrium will shift toward the products.

Question 3: Match the action to the effect on the equilibrium position for the reaction N2(g) + 3H2(g) ⇌ 2NH3(g).

The correct matching is:

Decreasing the pressure: Shift to the left (A)

Adding hydrogen gas: Shift to the right (B)

Adding a catalyst: No effect (C)

Question 4: What change would shift the equilibrium system to the left?

The correct option is: Removing some of gas C from the system.

Question 5: What stress would shift the equilibrium position of the following system to the left? N2O3(g) ⇌ NO(g) + NO2(g); ΔH is negative.

The correct option is: Decreasing the concentration of N2O3.

Question 6: Nitrogen dioxide gas is dark brown in color and remains in equilibrium with dinitrogen tetroxide gas, which is colorless. 2NO2(g) ⇌ N2O4(g). When a light brown colored mixture of the two gases at equilibrium was moved from room temperature to a higher temperature, the mixture turned dark brown in color. Which of the following conclusions about this equilibrium mixture is true?

The correct conclusion is: This reaction is endothermic because the system shifted to the right on heating.

Question 7: According to Le Châtelier's principle, how will a decrease in concentration of a reactant affect the equilibrium system?