Chapter 10

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12/11/23, 11:53 PM Chapter 10 Assignment https://session.masteringchemistry.com/myct/assignmentPrintView?assignmentID=11885468 1/35 Chapter 10 Assignment Due: 12:00am on Tuesday, December 12, 2023 You will receive no credit for items you complete after the assignment is due. Grading Policy Chapter 10 Reading Question 2 Part A Which of the following conditions will decrease the rate of a reaction? Hint 1. Conditions that alter the rate of a reaction. Several factors can increase or decrease the rate of a reaction. These include temperature, concentration of the reactants, and the presence of a catalyst. See Section 10.1. ANSWER: Correct Chapter 10 Reading Question 1 Part A For a chemical reaction to occur, three factors must be met. Which of the following factors is required for a reaction to occur? Hint 1. Three factors are required for a chemical reaction to occur. Without all three, the reaction may not occur. See Section 10.1. ANSWER: Correct Introduction to Factors That Affect Rate Learning Goal: To learn how temperature, concentration, and catalysts affect the rate of a reaction. The rate of a reaction is defined as the ratio of the change in concentration of a product to the change in time: Three major factors will affect the rate of the reaction: temperature, concentration, and catalysts. In general, an increase in temperature, an increase in reactant concentration, or the presence of a catalyst will all increase the rate of the reaction. an increase in the concentration of the reactants a decrease in temperature an increase in temperature addition of a catalyst The molecules that are reacting must come close to each other. There must be fewer product molecules than reactant molecules. The reactants must align properly to break and form bonds. The reactants must be in the correct physical state.

12/11/23, 11:53 PM Chapter 10 Assignment https://session.masteringchemistry.com/myct/assignmentPrintView?assignmentID=11885468 2/35 Ammonia, , is used in numerous industrial processes, including the production of pharmaceuticals such as sulfonamide and antimalarials and vitamins such as the B vitamins. The equilibrium equation for the synthesis of ammonia (sometimes known as the Haber process) is Part A The Haber process is typically carried out at a temperature of approximately 500 . What would happen to the rate of the forward reaction if the temperature were lowered to 100 ? Hint 1. Conditions for collisions The reactants are gases. Imagine the gas molecules bouncing around inside a container. Three conditions must be met for two molecules to react with one another: 1. The molecules must collide. 2. The molecules must align properly during the collision. 3. The collision must occur with enough energy. The minimum energy is called activation energy . Hint 2. How does temperature affect collisions? Chemical reactions occur when molecules collide. Determine how changes in temperature affect collisions. Drag each question into the bin with its correct answer. Hint 1. Relating kinetic energy and temperature A change in temperature changes the kinetic energy and speed of the molecules. ANSWER: ANSWER: Correct Most reactions double in rate for each 10 increase in temperature. Part B What would happen to the rate of the forward reaction if the concentration of nitrogen were decreased? Hint 1. Conditions for collisions The reactants are gases. Imagine the gas molecules bouncing around inside a container. Three conditions must be met for two molecules to react with one another: Reset Help The reaction rate would . increase decrease not change Does a change in temperature affect the orientation of molecules during a collision? Does a change in temperature affect how often the molecules collide? Does a change in temperature affect the energy with which molecules collide? No Yes

12/11/23, 11:53 PM Chapter 10 Assignment https://session.masteringchemistry.com/myct/assignmentPrintView?assignmentID=11885468 3/35 1. The molecules must collide. 2. The molecules must align properly during the collision. 3. The collision must occur with enough energy. The minimum energy is called activation energy . Hint 2. How does concentration affect collisions? For ammonia to be produced, nitrogen must collide with hydrogen. Determine how changes in concentration affect collisions. Drag each question into the bin with its correct answer. Hint 1. Probability of collision The more molecules there are in a given space, the greater the chance that two of them will collide. If there are fewer molecules in a given space, there is less of a chance that two of them will collide. ANSWER: ANSWER: Correct As the concentration of nitrogen decreases, collisions between nitrogen and hydrogen are less likely to occur. Part C Which of the following would increase the rate of the reverse reaction? Hint 1. The reverse reaction Since the Haber process is an equilibrium reaction, we can consider both the forward and reverse directions of the reaction and how they are affected by various factors. In the reverse reaction, ammonia breaks apart into nitrogen and hydrogen. You can see this by reading the chemical equation backward. Hint 2. Determine whether reactant or product concentration affects the reaction rate ANSWER: Reset Help The reaction rate would . increase decrease not change The rate of a reaction is affected by the concentration of reactants only. products only. both reactants and products. Does a change in concentration affect the orientation of molecules during a collision? Does a change in concentration affect the energy with which molecules collide? Does a change in concentration affect how often the molecules collide? No Yes

12/11/23, 11:53 PM Chapter 10 Assignment https://session.masteringchemistry.com/myct/assignmentPrintView?assignmentID=11885468 4/35 Hint 3. Identify the reactant in the reverse reaction What is the reactant in the reverse reaction of the Haber process? ANSWER: ANSWER: Correct The concentration of affects how quickly and can be made. Part D What will happen to the rates of the forward and reverse reactions when a catalyst is added? Hint 1. What is the purpose of a catalyst? What does a catalyst do? ANSWER: Hint 2. A picture of the energy barrier Notice that the uncatalyzed reaction (green line) has a much higher activation energy than the catalyzed reaction (purple line). Also, notice that this is true whether you read the graph from left to right or from right to left. ANSWER: increasing the concentration of ammonia decreasing the temperature increasing the concentration of nitrogen A catalyst affects the number of collisions between reactant molecules. A catalyst affects the energy with which the reactants collide. A catalyst affects the energy barrier (activation energy) of the reaction. Forward rate increases; reverse rate decreases. Both forward and reverse rates increase. Both forward and reverse rates decrease. Forward rate decreases; reverse rate increases.

12/11/23, 11:53 PM Chapter 10 Assignment https://session.masteringchemistry.com/myct/assignmentPrintView?assignmentID=11885468 5/35 Correct The Haber process can be cheaply catalyzed using porous iron. A much more effective catalyst for the Haber process is osmium; however, it is very expensive and toxic. Chapter 10 Reading Question 3 Part A Which of the following statements is true about a reversible reaction that has reached chemical equilibrium? Hint 1. Definition of a reversible reaction. Reversible reactions have both a forward and a reverse reaction, which occur at the same time. See Section 10.2. ANSWER: Correct Chemical Equilibrium Learning Goal: To use the concept of reversible reactions to explain chemical equilibrium. At equilibrium the rate of the forward reaction is equal to the rate of the reverse reaction. This results in no further change in the concentrations of the reactants and products, even though the two reactions continue at equal but opposite rates. Part A Photosynthesis can be represented by Which of the following will be false when the photosynthesis reaction reaches equilibrium? 1. The rate of formation of is equal to the rate of formation of . 2. The concentration of will begin decreasing. 3. The concentrations of and will not change. 4. The concentrations of and will be equal. Hint 1. Relating coefficients and rate conceptually Look at the coefficients in the chemical equation representing photosynthesis. Oxygen is being produced six times faster than glucose. Carbon dioxide is being consumed six times faster than glucose is being produced. However, carbon dioxide and water are being consumed at the same rate. Hint 2. How is the rate of a reaction defined mathematically? Which of these represents the definition of the rate of a reaction? ANSWER: The rate of the forward reaction is increasing, while the reverse reaction has completely stopped. The reverse reaction occurs at a slower rate than the forward reaction. The forward reaction occurs at a faster rate than the reverse reaction. The forward and reverse reactions occur at the same rate.

12/11/23, 11:53 PM Chapter 10 Assignment https://session.masteringchemistry.com/myct/assignmentPrintView?assignmentID=11885468 6/35 Hint 3. Relating coefficients and rate mathematically Typically, the rate of a reaction is defined in terms of the change in concentration of a product. Thus, for a simple reaction such as the rate of the reaction is defined as To define the rate of this reaction in terms of the reactant, we must consider the effect of the coefficient. Since there are two molecules lost for every one molecule created, the change in is twice as fast as the change in . Further, since is decreasing, we must include a negative sign to produce a positive value for the rate. Thus the rate of this reaction in terms of is ANSWER: Correct At equilibrium, the forward and reverse rates are equal. So the rate of formation of will be equal to the rate of formation of . Concentrations do not change at equilibrium because all species are being produced at the same rate as they are being consumed. Part B An intermediate step in the process that ultimately produces sulfuric acid, is the catalytic oxidation of to . Vanadium(V) oxide is the catalyst. The three chemical species in the reaction are in equilibrium as follows: Which of the following are true statements about this reaction? 1. When is mixed with in a container, the initial rate of the forward reaction (production of ) is faster than the initial rate of the reverse reaction (production of ). 2. As is used up and accumulates, the rate of the forward reaction increases and the rate of the reverse reaction decreases. 3. At equilibrium the rate of production of reaches zero. 4. At equilibrium the concentration of will no longer be changing. Hint 1. How do the concentrations of SO 2 and SO 3 compare initially? Which of the following best characterizes the relationship between the and concentrations as the reaction just starts to happen when is mixed with in a container? ANSWER: Hint 2. What factors affect the rate of the forward reaction? Which of the following factors will not affect the rate of the forward reaction? 1. temperature 2. concentration of 3. concentration of 4. concentration of ANSWER: 1 and 2 are false 2 and 3 are false 2 and 4 are false 3 and 4 are false [ ] [ ] < = >

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