Question 1

The physiological equilibrium system that keeps the temperature of the body constant is called __________.

Accepted Answer

The process by which the body maintains a stable internal environment despite changes in the external environment is called homeostasis. One way that the body achieves this is through regulation of body temperature, which is controlled by a physiological equilibrium system. This system works to keep the body temperature within a narrow range, even when the external temperature changes.

Question 2

Which of the following equilibrium constants indicates the reaction that gives the smallest amount of product?

Accepted Answer

A smaller equilibrium constant (Kc) indicates that the reaction favors the reactants, resulting in a smaller amount of product at equilibrium.

Question 3

The equilibrium for the reaction for the decomposition of PCl₅ to chlorine and PCl₃ is 0.042. PCl₅(g) ⇌ PCl₃(g)+ Cl₂(g) If the equilibrium concentrations are [PCl₃] = 0.010 M, [Cl₂] = 0.10 M, what is the value of [PCl₅]?

Accepted Answer

We can use the equilibrium constant expression: K = [PCl₃][Cl₂]/[PCl₅] Plugging in the given values: 0.042 = (0.010)(0.10)/x Solving for x: x = (0.010)(0.10)/0.042 = 0.024 M Therefore, the answer is D) 0.024 M.

Question 4

The value of the equilibrium constant for the combination of nitrogen and oxygen to make NO is 2 × 10^-9. What does this tell you about the concentrations of materials in the equilibrium mixture?

Accepted Answer

The equilibrium constant (K) is equal to the ratio of product concentrations to reactant concentrations, each raised to their stoichiometric coefficients. In this case, K = [NO]/([N2][O2]). Since the value of K is less than 1, it indicates that the concentration of reactants (N2 and O2) will be higher than the concentration of products (NO) at equilibrium. Choice D correctly reflects this relationship.

Question 5

Treatment of carbon monoxide poisoning can be accomplished by the use of pure oxygen for breathing. This is an example of the use of __________ in a clinical setting.

Accepted Answer

Le Chatelier's principle is applied here as increasing the concentration of oxygen shifts the equilibrium towards the formation of oxyhemoglobin, reducing the concentration of carboxyhemoglobin in the blood.

Question 6

When you open a bottle of a soft drink and leave it open, the drink eventually goes flat. This happens because the equilibrium between carbonic acid and carbon dioxide shifts to produce

Accepted Answer

When a bottle of soft drink is opened and left open, the pressure inside the bottle decreases. This decrease in pressure causes the equilibrium between carbonic acid and carbon dioxide to shift towards the production of more carbon dioxide in order to increase the pressure inside the bottle. As a result, the drink becomes flat. Therefore, the correct choice is D) more carbon dioxide.

Question 7

Iron metal reacts with oxygen gas to produce iron(III) oxide. What will be the effect of increasing the pressure of oxygen gas in a closed reaction vessel?

Accepted Answer

Increasing the pressure of oxygen gas will shift the equilibrium towards the product side, resulting in more iron(III) oxide being produced.

Question 8

For the reaction of carbon with carbon dioxide to make carbon monoxide, one set of conditions produced a K_c = 1.2 × 10^-1. At equilibrium at a certain temperature, the concentration of product was 0.60 M. What was the concentration of carbon dioxide at that temperature? C(s) + CO₂(g) ⇌ 2CO(g)

Accepted Answer

The answer of For the reaction of carbon with carbon...

Question 9

For the following equilibrium reaction, which cause and effect are correctly matched? CO(g) + 2H₂(g) ⇌ CH₃OH(g) + heat

Accepted Answer

Removing H₂ will shift the equilibrium to the left to produce more H₂, according to Le Chatelier's principle.

Question 10

In the following gas phase reaction, Kc is much less than 1. At equilibrium, which of the following statements is true? 
COCl₂(g) ⇌ CO(g) + Cl₂(g)

Accepted Answer

The answer of In the following gas phase reaction, Kc...

Question 11

The equilibrium constant for the production of carbon dioxide from carbon monoxide and oxygen is K_c = 2 × 10¹¹. This means that the reaction mixture at equilibrium is likely to consist of

Accepted Answer

A very large equilibrium constant (Kc = 2 × 10^11) indicates that the reaction strongly favors the formation of products at equilibrium.

Question 12

For the following reaction, the equilibrium constant Kc is 2.0 at a certain temperature. If the concentration of both products is 0.10 M at equilibrium, what is the concentration of the starting material, NOBr?
 2NOBr(g) ⇌ 2NO(g) + Br₂(g)

Accepted Answer

The answer of For the following reaction, the equilibrium constant...

Question 13

In the following gas phase reaction, what is the effect of adding more NO₂ to the starting reaction mixture? 
2NO₂(g) ⇌ N₂O₄(g)

Accepted Answer

Adding more NO₂ shifts the equilibrium to the right, according to Le Chatelier's principle, increasing the quantity of N₂O₄ produced.

Question 14

In the reaction of nitrogen gas with oxygen gas to produce nitrogen oxide, what is the effect of adding more oxygen gas to the initial reaction mixture? The reaction is shown below. 
N₂(g) + O₂(g) ⇌ 2NO(g)

Accepted Answer

According to Le Chatelier's principle, if more of one reactant is added to an equilibrium mixture, the equilibrium will shift towards the direction that produces less of that reactant. In this case, adding more oxygen gas would cause the equilibrium to shift towards the production of more nitrogen oxide, resulting in the formation of more NO. Therefore, the correct answer is B.

Question 15

The reaction of hemoglobin with oxygen can be written as follows. 
Hb + O₂ ⇌ HbO₂
If the amount of oxygen available to the blood decreases significantly, what happens to the individual involved?

Accepted Answer

When the amount of oxygen available to the blood decreases significantly, hypoxia results, which is a condition where the body tissues do not receive enough oxygen to function properly. This can lead to a range of symptoms, including shortness of breath, headache, confusion, and even coma or death if left untreated.

Question 16

Carbon monoxide binds to hemoglobin 140 times more strongly than oxygen does. What does this tell you about the equilibrium constants for the two reactions of hemoglobin with carbon monoxide and oxygen?

Accepted Answer

The strength of binding is related to the equilibrium constant, with a stronger binding indicating a larger equilibrium constant. Therefore, the equilibrium constant for the binding of CO is greater than that of oxygen.

Question 17

In the reaction of carbon dioxide with water to give carbonic acid, the only gaseous component is the carbon dioxide. What will happen to the equilibrium concentration of carbonic acid if the pressure of carbon dioxide is increased in the container?

Accepted Answer

According to Le Chatelier's principle, if the pressure of the system is increased, the equilibrium will shift in the direction that produces fewer moles of gas. In this case, increasing the pressure of carbon dioxide will shift the equilibrium to the right, producing more carbonic acid, which is a liquid. Therefore, the concentration of carbonic acid will increase.

Question 18

In an exothermic reaction, heat can be considered a __________.

Accepted Answer

In an exothermic reaction, heat is released as a product of the reaction. It is not a reactant, a rate, a catalyst, or a determinant.

Question 19

PCl₅ (g) ⇌ PCl₃ (g)+ Cl₂ (g) For the reaction at equilibrium, if the volume of the container is increased, the amount of PCl₅ present will

Accepted Answer

According to Le Chatelier's principle, if the volume of the container is increased, the equilibrium will shift to the side with fewer moles of gas. In this case, the left side has 2 moles of gas (PCl₅ and Cl₂) while the right side has only 1 mole of gas (Cl₂). Therefore, the equilibrium will shift towards the right side, decreasing the amount of PCl₅ present.

Question 20

In the following gas phase reaction, what is the effect on the direction of the reaction if more SO₃ is added to the reaction mixture? 
2SO₂(g) + O₂(g) ⇌ 2SO₃(g)

Accepted Answer

According to Le Chatelier's principle, adding more SO₃ will shift the equilibrium to the left to produce more reactants (SO₂ and O₂) to counteract the change.

Quiz 9: Reaction Rates and Chemical Equilibrium

The physiological equilibrium system that keeps the temperature of the body constant is called __________.

Which of the following equilibrium constants indicates the reaction that gives the smallest amount of product?

The equilibrium for the reaction for the decomposition of PCl₅ to chlorine and PCl₃ is 0.042. PCl₅(g) ⇌ PCl₃(g) + Cl₂(g) If the equilibrium concentrations are [PCl₃] = 0.010 M, [Cl₂] = 0.10 M, what is the value of [PCl₅]?

The value of the equilibrium constant for the combination of nitrogen and oxygen to make NO is 2 × 10^-9. What does this tell you about the concentrations of materials in the equilibrium mixture?

Treatment of carbon monoxide poisoning can be accomplished by the use of pure oxygen for breathing. This is an example of the use of __________ in a clinical setting.

When you open a bottle of a soft drink and leave it open, the drink eventually goes flat. This happens because the equilibrium between carbonic acid and carbon dioxide shifts to produce

Iron metal reacts with oxygen gas to produce iron(III) oxide. What will be the effect of increasing the pressure of oxygen gas in a closed reaction vessel?

For the reaction of carbon with carbon dioxide to make carbon monoxide, one set of conditions produced a K_c = 1.2 × 10^-1. At equilibrium at a certain temperature, the concentration of product was 0.60 M. What was the concentration of carbon dioxide at that temperature? C(s) + CO₂(g) ⇌ 2CO(g)

For the following equilibrium reaction, which cause and effect are correctly matched? CO(g) + 2H₂(g) ⇌ CH₃OH(g) + heat

In the following gas phase reaction, Kc is much less than 1. At equilibrium, which of the following statements is true? COCl₂(g) ⇌ CO(g) + Cl₂(g)

The equilibrium constant for the production of carbon dioxide from carbon monoxide and oxygen is K_c = 2 × 10¹¹. This means that the reaction mixture at equilibrium is likely to consist of

For the following reaction, the equilibrium constant Kc is 2.0 at a certain temperature. If the concentration of both products is 0.10 M at equilibrium, what is the concentration of the starting material, NOBr? 2NOBr(g) ⇌ 2NO(g) + Br₂(g)

In the following gas phase reaction, what is the effect of adding more NO₂ to the starting reaction mixture? 2NO₂(g) ⇌ N₂O₄(g)

In the reaction of nitrogen gas with oxygen gas to produce nitrogen oxide, what is the effect of adding more oxygen gas to the initial reaction mixture? The reaction is shown below. N₂(g) + O₂(g) ⇌ 2NO(g)

The reaction of hemoglobin with oxygen can be written as follows. Hb + O₂ ⇌ HbO₂ If the amount of oxygen available to the blood decreases significantly, what happens to the individual involved?

Carbon monoxide binds to hemoglobin 140 times more strongly than oxygen does. What does this tell you about the equilibrium constants for the two reactions of hemoglobin with carbon monoxide and oxygen?

In the reaction of carbon dioxide with water to give carbonic acid, the only gaseous component is the carbon dioxide. What will happen to the equilibrium concentration of carbonic acid if the pressure of carbon dioxide is increased in the container?

In an exothermic reaction, heat can be considered a __________.

PCl₅ (g) ⇌ PCl₃ (g) + Cl₂ (g) For the reaction at equilibrium, if the volume of the container is increased, the amount of PCl₅ present will

In the following gas phase reaction, what is the effect on the direction of the reaction if more SO₃ is added to the reaction mixture? 2SO₂(g) + O₂(g) ⇌ 2SO₃(g)

Quiz 9: Reaction Rates and Chemical Equilibrium

The physiological equilibrium system that keeps the temperature of the body constant is called __________.

Which of the following equilibrium constants indicates the reaction that gives the smallest amount of product?

The equilibrium for the reaction for the decomposition of PCl5 to chlorine and PCl3 is 0.042. PCl5(g) ⇌ PCl3(g) + Cl₂(g) If the equilibrium concentrations are [PCl3] = 0.010 M, [Cl₂] = 0.10 M, what is the value of [PCl5]?

The value of the equilibrium constant for the combination of nitrogen and oxygen to make NO is 2 × 10-9. What does this tell you about the concentrations of materials in the equilibrium mixture?

Treatment of carbon monoxide poisoning can be accomplished by the use of pure oxygen for breathing. This is an example of the use of __________ in a clinical setting.

When you open a bottle of a soft drink and leave it open, the drink eventually goes flat. This happens because the equilibrium between carbonic acid and carbon dioxide shifts to produce

Iron metal reacts with oxygen gas to produce iron(III) oxide. What will be the effect of increasing the pressure of oxygen gas in a closed reaction vessel?

For the reaction of carbon with carbon dioxide to make carbon monoxide, one set of conditions produced a Kc = 1.2 × 10-1. At equilibrium at a certain temperature, the concentration of product was 0.60 M. What was the concentration of carbon dioxide at that temperature? C(s) + CO₂(g) ⇌ 2CO(g)

For the following equilibrium reaction, which cause and effect are correctly matched? CO(g) + 2H₂(g) ⇌ CH3OH(g) + heat

In the following gas phase reaction, Kc is much less than 1. At equilibrium, which of the following statements is true? COCl₂(g) ⇌ CO(g) + Cl₂(g)

The equilibrium constant for the production of carbon dioxide from carbon monoxide and oxygen is Kc = 2 × 1011. This means that the reaction mixture at equilibrium is likely to consist of

For the following reaction, the equilibrium constant Kc is 2.0 at a certain temperature. If the concentration of both products is 0.10 M at equilibrium, what is the concentration of the starting material, NOBr? 2NOBr(g) ⇌ 2NO(g) + Br₂(g)

In the following gas phase reaction, what is the effect of adding more NO₂ to the starting reaction mixture? 2NO₂(g) ⇌ N₂O₄(g)

In the reaction of nitrogen gas with oxygen gas to produce nitrogen oxide, what is the effect of adding more oxygen gas to the initial reaction mixture? The reaction is shown below. N₂(g) + O₂(g) ⇌ 2NO(g)

The reaction of hemoglobin with oxygen can be written as follows. Hb + O₂ ⇌ HbO₂ If the amount of oxygen available to the blood decreases significantly, what happens to the individual involved?

Carbon monoxide binds to hemoglobin 140 times more strongly than oxygen does. What does this tell you about the equilibrium constants for the two reactions of hemoglobin with carbon monoxide and oxygen?

In the reaction of carbon dioxide with water to give carbonic acid, the only gaseous component is the carbon dioxide. What will happen to the equilibrium concentration of carbonic acid if the pressure of carbon dioxide is increased in the container?

In an exothermic reaction, heat can be considered a __________.

PCl5 (g) ⇌ PCl3 (g) + Cl₂ (g) For the reaction at equilibrium, if the volume of the container is increased, the amount of PCl5 present will

In the following gas phase reaction, what is the effect on the direction of the reaction if more SO₃ is added to the reaction mixture? 2SO₂(g) + O₂(g) ⇌ 2SO₃(g)

The equilibrium for the reaction for the decomposition of PCl₅ to chlorine and PCl₃ is 0.042. PCl₅(g) ⇌ PCl₃(g) + Cl₂(g) If the equilibrium concentrations are [PCl₃] = 0.010 M, [Cl₂] = 0.10 M, what is the value of [PCl₅]?

The value of the equilibrium constant for the combination of nitrogen and oxygen to make NO is 2 × 10^-9. What does this tell you about the concentrations of materials in the equilibrium mixture?

For the reaction of carbon with carbon dioxide to make carbon monoxide, one set of conditions produced a K_c = 1.2 × 10^-1. At equilibrium at a certain temperature, the concentration of product was 0.60 M. What was the concentration of carbon dioxide at that temperature? C(s) + CO₂(g) ⇌ 2CO(g)

For the following equilibrium reaction, which cause and effect are correctly matched? CO(g) + 2H₂(g) ⇌ CH₃OH(g) + heat

The equilibrium constant for the production of carbon dioxide from carbon monoxide and oxygen is K_c = 2 × 10¹¹. This means that the reaction mixture at equilibrium is likely to consist of

PCl₅ (g) ⇌ PCl₃ (g) + Cl₂ (g) For the reaction at equilibrium, if the volume of the container is increased, the amount of PCl₅ present will