Question 1

If you could somehow remove I₂ from the following reaction (already at equilibrium): H₂ + I₂ ⇔ 2HI what would you expect to happen to the rate of the reverse reaction (right to left)?

Accepted Answer

The answer of If you could somehow remove I₂ from...

Question 2

In the reaction N₂ (g)+ O₂ (g)⇔ 2NO (g), reducing the pressure will shift the equilibrium to the right.

Accepted Answer

In general, decreasing the pressure of a system will shift the equilibrium towards the side with more moles of gas. However, in this reaction, both sides have the same number of moles of gas (2). Therefore, changing the pressure will not have any significant effect on the equilibrium position.

Question 3

In the reaction Ni (s)+ 4CO (g)⇔ Ni(CO)₄ (g), adding extra nickel will shift the equilibrium to the right.

Accepted Answer

Adding extra nickel does not shift the equilibrium because nickel is a solid, and changes in the concentration of solids do not affect the equilibrium position.

Question 4

Among the two reactions whose equilibrium constants are 0.003 and 30, the one that will produce greater quantities of products is the one whose equilibrium constant is 30.

Accepted Answer

The equilibrium constant (Kc) measures the ratio of products to reactants at equilibrium. A higher Kc value indicates that more products are formed at equilibrium, while a lower Kc value indicates that more reactants are present at equilibrium. Therefore, the reaction with a Kc value of 30 will produce greater quantities of products than the reaction with a Kc value of 0.003.

Question 5

Predict the shift in the direction of the reaction for the following chemical reaction: CH₄ + O₂ ⇔ CO₂ + H₂O a)if methane (CH₄)is added. b)if carbon dioxide (CO₂)is added. c)if water (H₂O)is removed.

Accepted Answer

The answer of Predict the shift in the direction of...

Question 6

In the reaction N₂H₄ (g)⇔ 2 H₂ (g)+ N₂(g)at 1500 K, the equilibrium concentrations of each species are, [N₂] = 0.10 M, and [N₂H₄] = 0.10 M. The equilibrium constant value is 0.04.

Accepted Answer

The equilibrium constant expression is Kc = ([H₂]^2 [N₂]) / [N₂H₄]. Plugging in the given concentrations and the equilibrium constant value, we get: 0.04 = (0.1^2 x 0.1) / 0.1 0.04 = 0.1 Since this statement is false, the opposite must be true, which is that the statement "The equilibrium constant value is 0.04" is false. The correct equilibrium constant value is actually 4. Therefore, the answer is A.

Question 7

In the reaction N₂ (g)+ 2O₂ (g)⇔ 2NO₂ (g), reducing the pressure will shift the equilibrium to the left

Accepted Answer

Reducing the pressure favors the side with more moles of gas. The left side has 3 moles of gas (1 N2 + 2 O2), while the right side has 2 moles of NO2.

Question 8

The term "molar solubility of a salt" refers to the molar concentration of one anion (or cation)formed in an aqueous , saturated solution of that salt.

Accepted Answer

The molar solubility of a salt refers to the concentration of one of its ions in a saturated solution. It is typically expressed in units of moles per liter (M).

Question 9

If the value of the equilibrium constant for the forward reaction is 2.5 × 10³⁰, the value of the equilibrium constant for the reverse reaction is 4.0 × 10^-³⁰.

Accepted Answer

The equilibrium constant for the reverse reaction is the reciprocal of the equilibrium constant for the forward reaction. Therefore, the correct value for the equilibrium constant of the reverse reaction would be 4.0 × 10^-12.

Question 10

In the reaction Cl₂ (g)+ 3F₂ (g)⇔ 2ClF₃ (g), reducing the pressure will shift the equilibrium to the right.

Accepted Answer

According to Le Chatelier's principle, a decrease in pressure will shift the equilibrium in the direction that produces fewer gas molecules. In this case, the reactants and products all have the same number of gas molecules (4), so a change in pressure will not affect the equilibrium position.

Question 11

Predict the shift in the direction of the reaction for the following chemical reaction: 3O₂ + ultraviolet light ⇔ 2O₃ a)if oxygen (O₂)is added. b)if ozone (O₃)is removed. c)if oxygen (O₂)is removed. d)if more ultraviolet light is added.

Accepted Answer

The answer of Predict the shift in the direction of...

Question 12

In the reaction 3O₂ (g)⇔ 2O₃ (g), expanding the reaction vessel will shift the equilibrium to the right.

Accepted Answer

According to Le Chatelier's principle, expanding the volume of the reaction vessel will shift the equilibrium towards the side with more moles of gas. In this case, both the reactant and product sides have the same number of gas molecules, so expanding the vessel will not have any effect on the equilibrium position. Therefore, the correct answer is B, false.

Question 13

The double arrow in a chemical reaction indicates that the equilibrium is established because the rate of the forward reaction is equal to the rate of the reverse reaction.

Accepted Answer

The double arrow in a chemical reaction signifies that the reaction can occur in both forward and reverse directions, indicating that the system has reached equilibrium. At equilibrium, the rate of the forward reaction is equal to the rate of the reverse reaction.

Question 14

Predict the shift in the direction of the reaction for the following chemical reaction: 4HCl + O₂ ⇔ 2Cl₂ + 2H₂O a)if you add water (H₂O). b)if you remove chlorine (Cl₂). c)if you remove oxygen (O₂).

Accepted Answer

The answer of Predict the shift in the direction of...

Question 15

If you could somehow add more N₂O₄ to the following reaction (already at equilibrium): N₂O₄ ⇔ NO₂ what would expect to happen to the rate of the forward (left to right)reaction?

Accepted Answer

The answer of If you could somehow add more N₂O₄...

Question 16

A product favored reaction has K_eq < 1.

Accepted Answer

A product favored reaction has K_eq > 1, indicating that at equilibrium, the concentration of products is greater than the concentration of reactants.

Question 17

In the reaction PCl₅ ⇔ PCl₃ + Cl₂ at 500 K, the equilibrium concentrations of each species are [PCl₅] = 0.008 M, [PCl₃] = 0.02 M, and [Cl₂] = 0.02 M. The equilibrium constant value is 0.5.

Accepted Answer

The equilibrium constant value (Kc) is calculated by dividing the product of the concentrations of the products by the product of the concentrations of the reactants, each raised to their stoichiometric coefficients. Kc = ([PCl₃][Cl₂])/[PCl₅] = (0.02 x 0.02)/(0.008) = 0.05 Since the given equilibrium constant value is 0.5 and the calculated value of Kc is 0.05, the answer is false.

Question 18

Adding a catalyst to any reaction will always change the value of the equilibrium constant.

Accepted Answer

Adding a catalyst does not change the value of the equilibrium constant. It only reduces the activation energy and speeds up the rate of the forward and backward reactions equally, thereby reaching equilibrium faster.

Question 19

In the reaction 3O₂ (g)⇔ 2O₃ (g), removing ozone as soon as it is formed will shift the equilibrium to the right.

Accepted Answer

According to Le Chatelier's principle, removing one of the products (ozone) will cause the reaction to shift in the direction that produces more of that product, which in this case is to the right. Therefore, removing ozone as it is formed will shift the equilibrium to the right.

Question 20

Changing the temperature of a reaction will not change the equilibrium value.

Accepted Answer

Changing the temperature of a reaction can shift the equilibrium position of the reaction either forward or backward, resulting in a change in the equilibrium value.

Quiz 14: Chemical Equilibrium

If you could somehow remove I2 from the following reaction (already at equilibrium): H2 + I2 ⇔ 2HI what would you expect to happen to the rate of the reverse reaction (right to left)?

In the reaction N2 (g)+ O2 (g)⇔ 2NO (g), reducing the pressure will shift the equilibrium to the right.

In the reaction Ni (s)+ 4CO (g)⇔ Ni(CO)4 (g), adding extra nickel will shift the equilibrium to the right.

Among the two reactions whose equilibrium constants are 0.003 and 30, the one that will produce greater quantities of products is the one whose equilibrium constant is 30.

Predict the shift in the direction of the reaction for the following chemical reaction: CH4 + O2 ⇔ CO2 + H2O a)if methane (CH4)is added. b)if carbon dioxide (CO2)is added. c)if water (H2O)is removed.

In the reaction N2H4 (g)⇔ 2 H2 (g)+ N2 (g)at 1500 K, the equilibrium concentrations of each species are, [N2] = 0.10 M, and [N2H4] = 0.10 M. The equilibrium constant value is 0.04.

In the reaction N2 (g)+ 2O2 (g)⇔ 2NO2 (g), reducing the pressure will shift the equilibrium to the left

The term "molar solubility of a salt" refers to the molar concentration of one anion (or cation)formed in an aqueous , saturated solution of that salt.

If the value of the equilibrium constant for the forward reaction is 2.5 × 1030, the value of the equilibrium constant for the reverse reaction is 4.0 × 10-30.

In the reaction Cl2 (g)+ 3F2 (g)⇔ 2ClF3 (g), reducing the pressure will shift the equilibrium to the right.

Predict the shift in the direction of the reaction for the following chemical reaction: 3O2 + ultraviolet light ⇔ 2O3 a)if oxygen (O2)is added. b)if ozone (O3)is removed. c)if oxygen (O2)is removed. d)if more ultraviolet light is added.

In the reaction 3O2 (g)⇔ 2O3 (g), expanding the reaction vessel will shift the equilibrium to the right.

The double arrow in a chemical reaction indicates that the equilibrium is established because the rate of the forward reaction is equal to the rate of the reverse reaction.

Predict the shift in the direction of the reaction for the following chemical reaction: 4HCl + O2 ⇔ 2Cl2 + 2H2O a)if you add water (H2O). b)if you remove chlorine (Cl2). c)if you remove oxygen (O2).

If you could somehow add more N2O4 to the following reaction (already at equilibrium): N2O4 ⇔ NO2 what would expect to happen to the rate of the forward (left to right)reaction?

A product favored reaction has Keq < 1.

In the reaction PCl5 ⇔ PCl3 + Cl2 at 500 K, the equilibrium concentrations of each species are [PCl5] = 0.008 M, [PCl3] = 0.02 M, and [Cl2] = 0.02 M. The equilibrium constant value is 0.5.

Adding a catalyst to any reaction will always change the value of the equilibrium constant.

In the reaction 3O2 (g)⇔ 2O3 (g), removing ozone as soon as it is formed will shift the equilibrium to the right.

Changing the temperature of a reaction will not change the equilibrium value.

If you could somehow remove I₂ from the following reaction (already at equilibrium): H₂ + I₂ ⇔ 2HI what would you expect to happen to the rate of the reverse reaction (right to left)?

In the reaction N₂ (g)+ O₂ (g)⇔ 2NO (g), reducing the pressure will shift the equilibrium to the right.

In the reaction Ni (s)+ 4CO (g)⇔ Ni(CO)₄ (g), adding extra nickel will shift the equilibrium to the right.

Predict the shift in the direction of the reaction for the following chemical reaction: CH₄ + O₂ ⇔ CO₂ + H₂O a)if methane (CH₄)is added. b)if carbon dioxide (CO₂)is added. c)if water (H₂O)is removed.

In the reaction N₂H₄ (g)⇔ 2 H₂ (g)+ N₂(g)at 1500 K, the equilibrium concentrations of each species are, [N₂] = 0.10 M, and [N₂H₄] = 0.10 M. The equilibrium constant value is 0.04.

In the reaction N₂ (g)+ 2O₂ (g)⇔ 2NO₂ (g), reducing the pressure will shift the equilibrium to the left

If the value of the equilibrium constant for the forward reaction is 2.5 × 10³⁰, the value of the equilibrium constant for the reverse reaction is 4.0 × 10^-³⁰.

In the reaction Cl₂ (g)+ 3F₂ (g)⇔ 2ClF₃ (g), reducing the pressure will shift the equilibrium to the right.

Predict the shift in the direction of the reaction for the following chemical reaction: 3O₂ + ultraviolet light ⇔ 2O₃ a)if oxygen (O₂)is added. b)if ozone (O₃)is removed. c)if oxygen (O₂)is removed. d)if more ultraviolet light is added.

In the reaction 3O₂ (g)⇔ 2O₃ (g), expanding the reaction vessel will shift the equilibrium to the right.

Predict the shift in the direction of the reaction for the following chemical reaction: 4HCl + O₂ ⇔ 2Cl₂ + 2H₂O a)if you add water (H₂O). b)if you remove chlorine (Cl₂). c)if you remove oxygen (O₂).

If you could somehow add more N₂O₄ to the following reaction (already at equilibrium): N₂O₄ ⇔ NO₂ what would expect to happen to the rate of the forward (left to right)reaction?

A product favored reaction has K_eq < 1.

In the reaction PCl₅ ⇔ PCl₃ + Cl₂ at 500 K, the equilibrium concentrations of each species are [PCl₅] = 0.008 M, [PCl₃] = 0.02 M, and [Cl₂] = 0.02 M. The equilibrium constant value is 0.5.

In the reaction 3O₂ (g)⇔ 2O₃ (g), removing ozone as soon as it is formed will shift the equilibrium to the right.