ch 10 chem

What is the correct form for the equilibrium constant expression for this reaction? H2(g) + F2(g) ⇌ 2HF(g)

(HF)^2 --------- (H2)(F2)

The equation for the formation of ammonia from nitrogen and hydrogen is shown below. What is the form of the equilibrium constant? 3H2(g) + N2(g) ⇌ 2NH3(g) A) B) C) D) E)

(Nh3)^2 ----------- (N2)(H2)3

If the equilibrium concentrations are [PCl5] = 1.0 M, [PCl3] = 0.10 M, [Cl2] = 0.10 M, what is the value of the equilibrium constant? A) 1.0 × 10-2 B) 1.0 × 10-4 C) 10 × 10-2 D) 1.0 × 102 E) 2.0 × 10-2

A) 1.0 × 10-2

For the following reaction, the equilibrium constant Kc is 0.60 at a certain temperature. If the concentration of NO(g) and NOBr(g) are both 0.50 M,at equilibrium, what is the concentration of Br2(g)? 2NO(g) + Br2(g) ⇌ 2NOBr(g) A) 1.7 M B) 0.60 M C) 0.36 M D) 2.8 M E) 1.0 M

A) 1.7 M

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? A) Hypoxia results. B) Anemia results. C) Nitrogen narcosis results. D) Oxygen poisoning results. E) Acclimatization results.

A) Hypoxia results.

Which of the following equilibrium constants indicates the reaction that gives the smallest amount of product? A) Kc = 5 × 10-10 B) Kc = 5 × 10-1 C) Kc = 5 × 100 D) Kc = 5 × 101 E) Kc = 5 × 1010

A) Kc = 5 × 10-10

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) A) The concentration of reactant is much greater than the concentration of products. B) The concentration of products is much greater than the concentration of reactants. C) The concentrations of products and reactants are approximately equal. D) A catalyst will increase the concentration of products formed. E) At equilibrium, the concentrations of reactants and products are equal.

A) The concentration of reactant is much greater than the concentration of products.

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? A) The equilibrium constant for the binding of CO is greater. B) The equilibrium constant for the binding of oxygen is greater. C) The concentration of carbon monoxide at equilibrium is twice that of oxygen. D) Oxygen and carbon monoxide have the same formula mass. E) Oxygen and carbon monoxide react with hemoglobin in different fashions.

A) The equilibrium constant for the binding of CO is greater.

In a catalytic converter in an automobile, the reaction of carbon monoxide with oxygen produces A) carbon dioxide. B) carbon and more oxygen. C) water. D) methane. E) nitrogen oxide.

A) carbon dioxide.

In the reaction of nitrogen and hydrogen to give ammonia, all the reactants and products are A) gases. B) liquids. C) solids. D) boiling. E) frozen.

A) gases.

In a catalyzed chemical reaction, one function of a catalyst is to A) increase the number of successful reactant collisions. B) decrease the concentration of reactants. C) change the equilibrium concentrations of the products and reactants. D) increase the energy given off during the reaction. E) increase the temperature at which the reaction is carried out.

A) increase the number of successful reactant collisions.

A reaction that can proceed in either the forward or the reverse direction as written is called a ________ reaction. A) reversible B) miniscule C) microscopic D) solid phase E) favored

A) reversible

The rate of any chemical reaction can be determined by observing A) the amount of product formed in a unit of time. B) the ratio of product concentration to reactant concentration. C) the percent composition of the final product. D) the theoretical yield of the reaction. E) the number of chemical bonds broken and remade.

A) the amount of product formed in a unit of time.

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? A) Less reaction will take place. B) More iron oxide will be produced. C) The reaction mixture will catch fire. D) There is no effect; a catalyst is needed. E) The rate of production of iron oxide will slow down

B) More iron oxide will be produced.

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) A) The equilibrium shifts to produce more N2. B) The equilibrium shifts to produce more NO. C) The equilibrium is not affected. D) Extra catalyst is required to reach equilibrium. E) The temperature of the reaction mixture is raised

B) The equilibrium shifts to produce more NO.

For the following reaction, the equilibrium concentration of NO2 is 0.38 M and equilibrium concentration of N2O4 is 1.0M. What is the value of the equilibrium constant? 2NO2(g) ⇌ N2O4(g) A) 0.14 B) 2.6 C) 6.9 D) 0.38 E) 1.0

C) 6.9

A catalyst is A) a reactant in a chemical reaction. B) a product in a chemical reaction. C) a substance that speeds up a reaction without being consumed in the reaction. D) a substance that increases the energy of the products. E) a substance that decreases the energy of the products.

C) a substance that speeds up a reaction without being consumed in the reaction.

Refrigerating perishable foods affects biochemical reactions by A) increasing concentrations of antioxidants. B) removing bacteria. C) decreasing the rate of reactions affecting spoilage. D) catalyzing the removal of harmful chemicals from the foods. E) improving the appearance of the foods.

C) decreasing the rate of reactions affecting spoilage.

The activation energy of a chemical reaction is the energy that A) must be removed from the mixture. B) must be released from the mixture. C) initiates the reaction. D) activates the catalyst. E) is the difference in the energies of the starting materials and products.

C) initiates the reaction.

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]? A) 0.010 M B) 0.0020 M C) 0.042 M D) 0.024 M E) 0.0010 M

D) 0.024 M

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) A) 5 × 10-4 M B) 2.2 × 10-4 M C) 5 × 10-2 M D) 2.2 × 10-2 M E) 2.2 M

D) 2.2 × 10-2 M

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? A) The concentration of products exceeds the concentration of reactants. B) The concentrations of reactants and products are equal. C) The reactants are solids. D) The concentration of reactants exceeds the concentration of products. E) The products are solids.

D) The concentration of reactants exceeds the concentration of products.

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) A) The equilibrium shifts to produce more products. B) The position of the equilibrium remains unchanged. C) The rate of formation of products is increased. D) The equilibrium shifts to produce more reactants. E) The catalyst for the reaction is used up.

D) The equilibrium shifts to produce more reactants.

The physiological equilibrium system that keeps the temperature of the body constant is called A) stimulation. B) regulation. C) metabolism. D) homeostasis. E) catalysis.

D) homeostasis.

An equilibrium in which all the components are gases is a ________ equilibrium. A) heterogeneous B) liquid C) catalytic D) homogeneous E) reversible

D) homogeneous

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 A) more carbonic acid. B) more water. C) more oxygen. D) more carbon dioxide. E) more hydrogen ions

D) more carbon dioxide.

One metal that is used as a catalyst in a catalytic converter in an automobile is A) carbon. B) iron. C) copper. D) platinum. E) plutonium.

D) platinum.

N2(g) + O2(g) ⇌ 2NO(g) For the reaction at equilibrium, if the volume of the container is decreased, the amount of NO present will A) decrease. B) increase. C) double. D) stay the same. E) triple.

D) stay the same.

When a reaction is at equilibrium, A) all reaction stops. B) no more reactants are converted to products. C) the reaction is no longer reversible. D) the forward and reverse reactions occur at the same rate. E) the products and reactants have the same energy content.

D) the forward and reverse reactions occur at the same rate.

In the following gas phase reaction, what is the effect of adding more NO2 to the starting reaction mixture? 2NO2(g) ⇌ N2O4(g) A) It would make the reaction more endothermic. B) It would make the reaction more exothermic. C) It would slow the reaction down. D) It would decrease the final quantity of products. E) It would increase the final quantity of products.

E) It would increase the final quantity of products.

In any chemical reaction, the rate of the reaction can be increased by A) decreasing the temperature. B) changing the size of the container. C) adding water to the reaction. D) adding product molecules to the reaction mixture. E) increasing the concentrations of the reactants.

E) increasing the concentrations of the reactants.

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 A) mostly starting materials. B) an equal mixture of products and reactants. C) twice as much starting material as product. D) twice as much product as starting material. E) mostly products.

E) mostly products.

For the following equilibrium reaction, which cause and effect are correctly matched? CO(g) + 2H2(g) ⇌ CH3OH(g) + heat A) add heat, shift right B) add CO, shift left C) remove CH3OH, shift left D) remove heat, no change E) remove H2, shift left

E) remove H2, shift left

A chemical reaction has reached equilibrium when A) the concentrations of reactants and products are equal. B) all reactants have been converted to products. C) all products have been removed from the reaction mixture. D) the catalyst has been used up. E) the rate of the forward reaction equals the rate of the reverse reaction.

E) the rate of the forward reaction equals the rate of the reverse reaction.

What is the correct form of the equilibrium constant for the reaction of hydrogen and oxygen to form water? The equation is: 2H2(g) + O2(g) ⇌ H2O(g)

Kc=H2O ------ (O2)(H2)^2