Question 1

Consider the equation 2SO₂ (g)+ O₂ (g)⇔ 2SO₃ (g). Removing product will ________.

Accepted Answer

Removing product will shift the reaction to the right according to Le Chatelier's principle.

Question 2

Consider the reaction: 2HS1U1B12S1U1B0S (g)+ 3OS1U1B12S1U1B0 (g)⇔ 2SOS1U1B12S1U1B0 (g)+ 2HS1U1B12S1U1B0O (g)to answer the following questions.
-Refer to the reaction shown above. Adding helium to the reaction vessel will ________.

Accepted Answer

Adding an inert gas like helium will not have any effect on the position of the equilibrium because the concentration of the gases involved in the reaction remains unchanged. Only changes in the concentrations of the reactants or products or changes in temperature and pressure can affect the equilibrium position.

Question 3

Consider the reaction: FeClS1U1B13 S1U1B0 + KSCN ⇔ KS1U1B13S1U1B0[Fe(SCN)S1U1B16S1U1B0] + 3KCl
yellow colorless red colorless
-Refer to the equilibrium shown above. Adding iron(III)chloride will ________.

Accepted Answer

The addition of iron(III) chloride will increase the concentration of Fe3+, shifting the equilibrium to the right according to Le Chatelier's principle. This will increase the concentration of the complex ion [Fe(SCN)16]3-, which is responsible for the red color of the solution. Therefore, the solution will turn more red.

Question 4

In an endothermic reaction, adding heat will ________.

Accepted Answer

In an endothermic reaction, adding heat shifts the equilibrium to the right, favoring the formation of products. This means both the amount of products will increase and the amount of reactants will decrease.

Question 5

Consider the equation 2NH₃ (g)⇔ N₂ (g)+ 3H₂ (g). Increasing the volume will ________.

Accepted Answer

Increasing the volume of the system decreases the pressure, and the reaction will shift towards the side with more moles of gas to counteract this change. In this case, the right side has more moles of gas (4 moles) compared to the left side (2 moles), so the reaction will shift to the right.

Question 6

Consider the reaction: 2HS1U1B12S1U1B0S (g)+ 3OS1U1B12S1U1B0 (g)⇔ 2SOS1U1B12S1U1B0 (g)+ 2HS1U1B12S1U1B0O (g)to answer the following questions.
-Refer to the reaction shown above. Removing sulfur dioxide as it is formed will ________.

Accepted Answer

According to Le Chatelier's principle, removing a product of a reaction will shift the equilibrium towards the side that produces more of that product. Therefore, removing sulfur dioxide will shift the reaction to the right, forming more of the product, SO2.

Question 7

In an exothermic reaction, adding heat will ________.

Accepted Answer

In an exothermic reaction, adding heat shifts the equilibrium to favor the reactants, thus decreasing the amount of products according to Le Chatelier's principle.

Question 8

Consider the equation O₂ (g)+ 2H₂ (g)⇔ 2H₂O (g). Increasing the concentration of hydrogen gas will ________.

Accepted Answer

Increasing the concentration of a reactant (in this case, hydrogen gas) will shift the equilibrium of the reaction to the right, favoring the formation of more product (in this case, H2₂O).

Question 9

Consider the reaction: A + 3B ⇔ 2C. Equal numbers of moles for A and B are added to the reaction vessel and equilibrium established. At that point ________.

Accepted Answer

The answer of Consider the reaction: A + 3B ⇔...

Question 10

Consider the equation 2NH₃ (g)⇔ N₂ (g)+ 3H₂ (g). Increasing the pressure will ________.

Accepted Answer

Increasing pressure will shift the equilibrium towards the side with fewer moles of gas, according to Le Chatelier's principle. The left-hand side of the equation has one mole of gas, while the right-hand side has four moles of gas. Therefore, increasing the pressure will shift the equilibrium to the left, towards the side with fewer moles of gas.

Question 11

Consider the equation 2NH₃ (g)⇔ N₂ (g)+ 3H₂ (g). Decreasing the concentration of ammonia gas will ________.

Accepted Answer

Decreasing the concentration of ammonia gas will shift the equilibrium to the left in order to compensate for the decrease in reactants. This is based on the principle of Le Chatelier's principle, which states that a system at equilibrium will respond to a stress by shifting the equilibrium in the direction that counteracts the stress. Since the equilibrium constant is unknown, the effect of temperature change cannot be determined.

Question 12

For an endothermic reaction, lowering the temperature of the reaction will ________.

Accepted Answer

For an endothermic reaction, lowering the temperature of the reaction will decrease the amount of products as the reaction requires heat to form products. Lowering the temperature reduces the amount of heat available for the reaction to occur, thus decreasing the amount of products formed. It will not increase the amount of products or decrease the amount of reactants.

Question 13

Consider the equation: CHS1U1B14S1U1B0 (g)+ 2OS1U1B12S1U1B0 (g)⇔ COS1U1B12S1U1B0 (g)+ 2HS1U1B12S1U1B0O (g)to answer the questions below.
-Refer to the equilibrium shown above. If oxygen is removed this will ________.

Accepted Answer

According to Le Chatelier's principle, if a reactant is removed, the equilibrium will shift in the direction that produces more of that reactant. Therefore, the equilibrium will shift to the left to produce more oxygen.

Question 14

Consider the reaction: 2HS1U1B12S1U1B0S (g)+ 3OS1U1B12S1U1B0 (g)⇔ 2SOS1U1B12S1U1B0 (g)+ 2HS1U1B12S1U1B0O (g)to answer the following questions.
-Refer to the reaction shown above. Increasing the volume of the system will ________.

Accepted Answer

Increasing the volume of the system decreases the pressure, favoring the side with more moles of gas. The left side has 5 moles of gas, while the right side has 4 moles, so the reaction shifts to the left.

Question 15

Consider the equation: CHS1U1B14S1U1B0 (g)+ 2OS1U1B12S1U1B0 (g)⇔ COS1U1B12S1U1B0 (g)+ 2HS1U1B12S1U1B0O (g)to answer the questions below.
-Refer to the equilibrium shown above. If the reaction vessel is expanded, this will ________.

Accepted Answer

Expanding the reaction vessel will not affect the equilibrium, since the number of moles on both sides of the equation will remain the same. This means that the concentration of the reactants and products will stay the same, and there will be no need for the reaction to shift in either direction in order to maintain equilibrium.

Question 16

Consider the equation: CHS1U1B14S1U1B0 (g)+ 2OS1U1B12S1U1B0 (g)⇔ COS1U1B12S1U1B0 (g)+ 2HS1U1B12S1U1B0O (g)to answer the questions below.
-Refer to the equilibrium shown above. Adding excess oxygen will ________.

Accepted Answer

Adding excess oxygen will increase the concentration of a reactant, causing the equilibrium to shift to the right to favor the formation of products according to Le Chatelier's principle.

Question 17

Consider the equation N₂ (g)+ 3H₂ (g)⇔ 2NH₃ (g). Removing ammonia as soon as it is formed will ________.

Accepted Answer

According to Le Chatelier's principle, removing the product (ammonia) from the reaction will shift the equilibrium towards the side that produces more NH3 to replace what was removed. Therefore, the reaction will shift to the right to produce more ammonia.

Question 18

For an exothermic reaction, lowering the temperature of the reaction will ________.

Accepted Answer

For an exothermic reaction, lowering the temperature shifts the equilibrium towards the products (according to Le Chatelier's principle), which effectively increases the amount of products and decreases the amount of reactants.

Question 19

Consider the reaction: 2HS1U1B12S1U1B0S (g)+ 3OS1U1B12S1U1B0 (g)⇔ 2SOS1U1B12S1U1B0 (g)+ 2HS1U1B12S1U1B0O (g)to answer the following questions.
-Refer to the reaction shown above. Which of the following will shift the equilibrium to the left?

Accepted Answer

Decreasing the pressure will shift the equilibrium to the side with fewer moles of gas, which is the left side in this case. Adding sulfur dioxide will also shift the equilibrium to the left because it is a reactant in the forward reaction.

Question 20

Consider the reaction: 2HS1U1B12S1U1B0S (g)+ 3OS1U1B12S1U1B0 (g)⇔ 2SOS1U1B12S1U1B0 (g)+ 2HS1U1B12S1U1B0O (g)to answer the following questions. -Refer to the reaction shown above. Adding H₂O to the reaction vessel will ________.

Accepted Answer

The answer of Consider the reaction: 2HS1U1B12S1U1B0S (g)+ 3OS1U1B12S1U1B0 (g)⇔...

Quiz 14: Chemical Equilibrium

Consider the equation 2SO₂ (g) + O₂ (g) ⇔ 2SO₃ (g) . Removing product will ________.

Consider the reaction: 2H₂S (g) + 3O₂ (g) ⇔ 2SO₂ (g) + 2H₂O (g) to answer the following questions. -Refer to the reaction shown above. Adding helium to the reaction vessel will ________.

Consider the reaction: FeCl₃ + KSCN ⇔ K₃[Fe(SCN) ₆] + 3KCl yellow colorless red colorless -Refer to the equilibrium shown above. Adding iron(III) chloride will ________.

In an endothermic reaction, adding heat will ________.

Consider the equation 2NH₃ (g) ⇔ N₂ (g) + 3H₂ (g) . Increasing the volume will ________.

Consider the reaction: 2H₂S (g) + 3O₂ (g) ⇔ 2SO₂ (g) + 2H₂O (g) to answer the following questions. -Refer to the reaction shown above. Removing sulfur dioxide as it is formed will ________.

In an exothermic reaction, adding heat will ________.

Consider the equation O₂ (g) + 2H₂ (g) ⇔ 2H₂O (g) . Increasing the concentration of hydrogen gas will ________.

Consider the reaction: A + 3B ⇔ 2C. Equal numbers of moles for A and B are added to the reaction vessel and equilibrium established. At that point ________.

Consider the equation 2NH₃ (g) ⇔ N₂ (g) + 3H₂ (g) . Increasing the pressure will ________.

Consider the equation 2NH₃ (g) ⇔ N₂ (g) + 3H₂ (g) . Decreasing the concentration of ammonia gas will ________.

For an endothermic reaction, lowering the temperature of the reaction will ________.

Consider the equation: CH₄ (g) + 2O₂ (g) ⇔ CO₂ (g) + 2H₂O (g) to answer the questions below. -Refer to the equilibrium shown above. If oxygen is removed this will ________.

Consider the reaction: 2H₂S (g) + 3O₂ (g) ⇔ 2SO₂ (g) + 2H₂O (g) to answer the following questions. -Refer to the reaction shown above. Increasing the volume of the system will ________.

Consider the equation: CH₄ (g) + 2O₂ (g) ⇔ CO₂ (g) + 2H₂O (g) to answer the questions below. -Refer to the equilibrium shown above. If the reaction vessel is expanded, this will ________.

Consider the equation: CH₄ (g) + 2O₂ (g) ⇔ CO₂ (g) + 2H₂O (g) to answer the questions below. -Refer to the equilibrium shown above. Adding excess oxygen will ________.

Consider the equation N₂ (g) + 3H₂ (g) ⇔ 2NH₃ (g) . Removing ammonia as soon as it is formed will ________.

For an exothermic reaction, lowering the temperature of the reaction will ________.

Consider the reaction: 2H₂S (g) + 3O₂ (g) ⇔ 2SO₂ (g) + 2H₂O (g) to answer the following questions. -Refer to the reaction shown above. Which of the following will shift the equilibrium to the left?

Consider the reaction: 2H₂S (g) + 3O₂ (g) ⇔ 2SO₂ (g) + 2H₂O (g) to answer the following questions. -Refer to the reaction shown above. Adding H₂O to the reaction vessel will ________.

Quiz 14: Chemical Equilibrium

Consider the equation 2SO2 (g) + O2 (g) ⇔ 2SO3 (g) . Removing product will ________.

Consider the reaction: 2H2S (g) + 3O2 (g) ⇔ 2SO2 (g) + 2H2O (g) to answer the following questions. -Refer to the reaction shown above. Adding helium to the reaction vessel will ________.

Consider the reaction: FeCl3 + KSCN ⇔ K3[Fe(SCN) 6] + 3KCl yellow colorless red colorless -Refer to the equilibrium shown above. Adding iron(III) chloride will ________.

In an endothermic reaction, adding heat will ________.

Consider the equation 2NH3 (g) ⇔ N2 (g) + 3H2 (g) . Increasing the volume will ________.

Consider the reaction: 2H2S (g) + 3O2 (g) ⇔ 2SO2 (g) + 2H2O (g) to answer the following questions. -Refer to the reaction shown above. Removing sulfur dioxide as it is formed will ________.

In an exothermic reaction, adding heat will ________.

Consider the equation O2 (g) + 2H2 (g) ⇔ 2H2O (g) . Increasing the concentration of hydrogen gas will ________.

Consider the reaction: A + 3B ⇔ 2C. Equal numbers of moles for A and B are added to the reaction vessel and equilibrium established. At that point ________.

Consider the equation 2NH3 (g) ⇔ N2 (g) + 3H2 (g) . Increasing the pressure will ________.

Consider the equation 2NH3 (g) ⇔ N2 (g) + 3H2 (g) . Decreasing the concentration of ammonia gas will ________.

For an endothermic reaction, lowering the temperature of the reaction will ________.

Consider the equation: CH4 (g) + 2O2 (g) ⇔ CO2 (g) + 2H2O (g) to answer the questions below. -Refer to the equilibrium shown above. If oxygen is removed this will ________.

Consider the reaction: 2H2S (g) + 3O2 (g) ⇔ 2SO2 (g) + 2H2O (g) to answer the following questions. -Refer to the reaction shown above. Increasing the volume of the system will ________.

Consider the equation: CH4 (g) + 2O2 (g) ⇔ CO2 (g) + 2H2O (g) to answer the questions below. -Refer to the equilibrium shown above. If the reaction vessel is expanded, this will ________.

Consider the equation: CH4 (g) + 2O2 (g) ⇔ CO2 (g) + 2H2O (g) to answer the questions below. -Refer to the equilibrium shown above. Adding excess oxygen will ________.

Consider the equation N2 (g) + 3H2 (g) ⇔ 2NH3 (g) . Removing ammonia as soon as it is formed will ________.

For an exothermic reaction, lowering the temperature of the reaction will ________.

Consider the reaction: 2H2S (g) + 3O2 (g) ⇔ 2SO2 (g) + 2H2O (g) to answer the following questions. -Refer to the reaction shown above. Which of the following will shift the equilibrium to the left?

Consider the reaction: 2H2S (g) + 3O2 (g) ⇔ 2SO2 (g) + 2H2O (g) to answer the following questions. -Refer to the reaction shown above. Adding H2O to the reaction vessel will ________.

Consider the equation 2SO₂ (g) + O₂ (g) ⇔ 2SO₃ (g) . Removing product will ________.

Consider the reaction: 2H₂S (g) + 3O₂ (g) ⇔ 2SO₂ (g) + 2H₂O (g) to answer the following questions. -Refer to the reaction shown above. Adding helium to the reaction vessel will ________.

Consider the reaction: FeCl₃ + KSCN ⇔ K₃[Fe(SCN) ₆] + 3KCl yellow colorless red colorless -Refer to the equilibrium shown above. Adding iron(III) chloride will ________.

Consider the equation 2NH₃ (g) ⇔ N₂ (g) + 3H₂ (g) . Increasing the volume will ________.

Consider the reaction: 2H₂S (g) + 3O₂ (g) ⇔ 2SO₂ (g) + 2H₂O (g) to answer the following questions. -Refer to the reaction shown above. Removing sulfur dioxide as it is formed will ________.

Consider the equation O₂ (g) + 2H₂ (g) ⇔ 2H₂O (g) . Increasing the concentration of hydrogen gas will ________.

Consider the equation 2NH₃ (g) ⇔ N₂ (g) + 3H₂ (g) . Increasing the pressure will ________.

Consider the equation 2NH₃ (g) ⇔ N₂ (g) + 3H₂ (g) . Decreasing the concentration of ammonia gas will ________.

Consider the equation: CH₄ (g) + 2O₂ (g) ⇔ CO₂ (g) + 2H₂O (g) to answer the questions below. -Refer to the equilibrium shown above. If oxygen is removed this will ________.

Consider the reaction: 2H₂S (g) + 3O₂ (g) ⇔ 2SO₂ (g) + 2H₂O (g) to answer the following questions. -Refer to the reaction shown above. Increasing the volume of the system will ________.

Consider the equation: CH₄ (g) + 2O₂ (g) ⇔ CO₂ (g) + 2H₂O (g) to answer the questions below. -Refer to the equilibrium shown above. If the reaction vessel is expanded, this will ________.

Consider the equation: CH₄ (g) + 2O₂ (g) ⇔ CO₂ (g) + 2H₂O (g) to answer the questions below. -Refer to the equilibrium shown above. Adding excess oxygen will ________.

Consider the equation N₂ (g) + 3H₂ (g) ⇔ 2NH₃ (g) . Removing ammonia as soon as it is formed will ________.

Consider the reaction: 2H₂S (g) + 3O₂ (g) ⇔ 2SO₂ (g) + 2H₂O (g) to answer the following questions. -Refer to the reaction shown above. Which of the following will shift the equilibrium to the left?

Consider the reaction: 2H₂S (g) + 3O₂ (g) ⇔ 2SO₂ (g) + 2H₂O (g) to answer the following questions. -Refer to the reaction shown above. Adding H₂O to the reaction vessel will ________.