Deck 14: Chemical Kinetics

Question 1

Which of the following is a homogeneous reaction?

A)dissolving salt in water
B)neutralizing aqueous acid with solid sodium hydroxide
C)iron rusting
D)phosphorus igniting in air
E)titration of an unknown base with aqueous hydrochloric acid

Answer 1

titration of an unknown base with aqueous hydrochloric acid

Question 2

The fact that granulated sugar dissolves faster than a sugar cube of the same mass can best be explained by which of the following statements?

A)The ability of reacting or interacting molecules to come in contact with each other is greater for granulated sugar.
B)Dissolving the sugar increases the temperature of the solution.
C)Sugar cubes are coated to slow the dissolving process.
D)The concentration of granulated sugar is higher than that of a sugar cube.
E)None of the above

Answer 2

The ability of reacting or interacting molecules to come in contact with each other is greater for granulated sugar.

Question 3

Most heterogeneous reactions are slower than similar homogeneous reactions. Which of the following best explains why?

A)The temperature of the two phases is different.
B)Heterogeneous mixtures are not allowed to react, and therefore are heterogeneous.
C)Heterogeneous mixtures require the use of a catalyst.
D)The ability of reactants to come in contact with each other in heterogeneous mixtures is limited by the different phases.
E)The activation energy of heterogeneous reactions is always much higher.

Answer 3

The ability of reactants to come in contact with each other in heterogeneous mixtures is limited by the different phases.

Question 4

Nitrogen monoxide reacts with bromine at elevated temperatures, according to the equation:2NO(g)+ Br₂(g) $\rarr$ 2NOBr(g)In a certain reaction mixture, the rate of formation of NOBr(g)was 4.50 × 10^-4 mol L^-1 s^-1. What was the rate of consumption of Br₂(g)?

A)4.50 × 10^-4 mol L^-1 s^-1
B)2.25 × 10^-4 mol L^-1 s^-1
C)9.00 × 10^-4 mol L^-1 s^-1
D)2.12 × 10^-4 mol L^-1 s^-1
E)2.03 × 10^-3 mol L^-1 s^-1

Question 5

Nitrogen monoxide reacts with chlorine at high temperature, according to the equation: 2NO(g)+ Cl₂(g) $\rarr$ 2NOCl(g)In a certain reaction mixture, the rate of formation of NOCl(g)was 4.50 × 10^-4 mol L^-1 s^-1. What was the rate of consumption of NO(g)?

A)4.50 × 10^-4 mol L^-1 s^-1
B)2.25 × 10^-4 mol L^-1 s^-1
C)9.00 × 10^-4 mol L^-1 s^-1
D)2.12 × 10^-4 mol L^-1 s^-1
E)2.03 × 10^-3 mol L^-1 s^-1

Question 6

In a reaction described by the equation: 2CH₄O(g)+ 3O₂(g) $\rarr$ 2CO₂(g)+ 4H₂O(g),the rate of consumption of O₂(g)is 0.400 mol L^-1 s^-1. What is the rate of formation of H₂O(g)?

A)0.300 mol L^-1 s^-1
B)0.400 mol L^-1 s^-1
C)0.533 mol L^-1 s^-1
D)0.800 mol L^-1 s^-1
E)1.33 mol L^-1 s^-1

Question 7

In a reaction described by the equation:2 CH₄O(g)+ 3 O₂(g) $\rarr$ 2 CO₂(g)+ 4 H₂O(g),the rate of consumption of O₂(g)is 0.400 mol L^-1 s^-1. What is the rate of consumption of CH₄O(g)?

A)0.200 mol L^-1 s^-1
B)0.267 mol L^-1 s^-1
C)0.333 mol L^-1 s^-1
D)0.400 mol L^-1 s^-1
E)0.600 mol L^-1 s^-1

Question 8

Cyclobutane, C₄H₈, decomposes as shown: C₄H₈(g) $\rarr$ 2 C₂H₄(g). In a study of this reaction, the rate of consumption of C₄H₈ at a certain point was 4.50 × 10^-4 mol L^-1 s^-1. What is the rate at which C₂H₄(g)is being generated at this point?

A)4.50 × 10^-4 mol L^-1 s^-1
B)2.25 × 10^-4 mol L^-1 s^-1
C)9.00 × 10^-4 mol L^-1 s^-1
D)2.12 × 10^-4 mol L^-1 s^-1
E)2.03 × 10^-3 mol L^-1 s^-1

Question 9

A 10-mm cube of copper metal is placed in 250 mL of 12 M nitric acid at 25°C and the reaction below occurs: Cu(s)+ 4H⁺(aq)+ 2NO₃^-(aq) $\rarr$ Cu²⁺(aq)+ 2NO₂(g)+ 2H₂O(l)At a particular instant in time, nitrogen dioxide is being produced at the rate of . At this same instant, what is the rate at which hydrogen ions are being consumed?

A)1.3 × 10^-4 M/min
B)5.2 × 10^-4 M/min
C)2.6 × 10^-4 M/min
D)1.0 × 10^-3 M/min
E)6.5 × 10^-5 M/min

Question 10

The average reaction rate over a time period in graph b can be found by

A)taking the average of the rate every 100 s.
B)drawing a line tangent to the curve at the initial and final times, and then averaging.
C)drawing a line tangent to the curve at that point.
D)subtracting the final concentration from the initial concentration and dividing by the time interval.
E)subtracting the final time from the initial time and dividing by the concentration interval.

Question 11

The instantaneous rate at any point in graph b can be found by

A)taking the average of all rates found every 100 s.
B)drawing a line tangent to the curve at the initial and final times, and then averaging.
C)drawing a line tangent to the curve at that point.
D)subtracting the final concentration from the initial concentration and dividing by the time interval.
E)subtracting the final time from the initial time and dividing by the concentration.

Question 12

The rate of a chemical reaction in solution can be measured in the units

A)L² mol^-1 s^-1.
B)mol L^-1 s^-1.
C)s^-2.
D)mol s L^-1.
E)sec L^-1 mol^-1.

Question 13

A reaction has the rate law, rate = k[A][B]². Which change will cause the greatest increase in the reaction rate?

A)decreasing both concentrations by half
B)doubling the concentration of B
C)quadrupling the concentration of A
D)tripling the concentration of B
E)doubling the concentration of A

Question 14

A reaction has the rate law, rate = k[A]³[B]. Which change will cause the greatest increase in the reaction rate?

A)doubling the concentration of A and halving the concentration of B
B)quadrupling the concentration of B
C)tripling the concentration of A
D)doubling the concentration of A and tripling the concentration of B
E)tripling the concentration of B

Question 15

The reaction, 2NO(g)+ O₂(g) $\rarr$ 2NO₂(g), was found to be first order in each of the two reactants and second order overall. The rate law is, therefore:

A)rate = k[NO]²
B)rate = k[NO][O₂]
C)rate = k[NO₂]²[NO]²[O₂]^½
D)rate = k[NO]²[O₂]²
E)rate = k([NO][O₂])²

Question 16

The reaction, NO₂Cl(g)+ Cl(g) $\rarr$ NO₂(g)+ Cl₂(g), was found to be first order in each of the two reactants and second order overall. The rate law is, therefore:

A)rate = k[NO₂]²
B)rate = k[Cl]
C)rate = k[NO₂Cl][Cl][NO₂][Cl₂]
D)rate = k[NO₂Cl][Cl]
E)rate = k[NO₂][ Cl₂]

Question 17

A reaction has the rate law: rate = k[A][B]². What is the overall order of the reaction?

A)2nd
B)4th
C)1st
D)3rd
E)0

Question 18

A reaction has the rate law, rate = k[A][B]³. What is the overall order of the reaction?

A)0
B)4th
C)1st
D)3rd
E)2nd

Question 19

The reaction 2NO (g)+ 2H₂ (g) $\rarr$ N₂ (g)+ 2H₂O (g)was found to follow the rate law:rate = k[NO]²[H₂]. By what factor will the rate of reaction increase if the pressure of NO gas is increased from 2.0 atm to 3.0 atm? Assume all other conditions are held constant.

A)1.5
B)1
C)2.25
D)2
E)3

Question 20

A reaction has the rate law: rate = k[A][B]². What is the order of the reaction, with respect to B?

A)2nd
B)4th
C)1st
D)3rd
E)0

Question 21

A reaction has the rate law: rate = k[A]³[B]. What is the order of the reaction, with respect to A?

A)2nd
B)4th
C)1st
D)3rd
E)0

Question 22

For the reaction, 2 XO + O₂ $\rarr$ 2 XO₂, data obtained from measurement of the initial rate of reaction at varying concentrations are given below. The rate law is therefore:

A)rate = k[XO]² [O₂]
B)rate = k[XO][O₂]²
C)rate = k[XO][O₂]
D)rate = k[XO]² [O₂]²
E)rate = k[XO]²/[O₂]²

Question 23

The units of the rate constant for a particular reaction are min^-1. What is the overall order of the reaction?

A)Zero
B)First
C)Second
D)Third
E)Fourth

Question 24

The units of the rate constant for a particular reaction are L mol^-1 min^-1. What is the overall order of the reaction?

A)Zero
B)First
C)Second
D)Third
E)Fourth

Question 25

Nitric oxide reacts with bromine at elevated temperatures according to the equation 2NO(g)+ Br₂(g) $\rarr$ 2 NOBr(g)The experimental rate law is rate = k[NO][Br₂]. In a certain reaction mixture, the rate of formation of NOBr(g)was found to be 4.50 × 10^-4 mol L^-1 s^-1. Which unit below is the correct unit for the rate constant?

A)mol L^-1 s^-1
B)s^-1
C)mol² L^-2 s^-1
D)L mol^-1 s^-1
E)L² mol^-2 s^-1

Question 26

For the reaction, 3B + C $\rarr$ E + 2F, initial rate measurements were carried out and data from three trials are shown below: The rate law, therefore, is

A)rate = k[B]³[C]
B)rate = k[B][C]
C)rate = k[B]²[C]²
D)rate = k[B]²[C]
E)rate = k[B][C]²

Question 27

Given the reaction, aA + bB $\rarr$ dD + eE If we try rate = k[A]^q[B]^r for a generic rate law statement, which one of the statements below is false?

A)The exponents q and r are often integers.
B)The exponent q and r must be determined experimentally.
C)The exponents q and r are equal to the coefficients a and b, respectively.
D)The overall order of the reaction is q + r.
E)The symbol k represents the rate constant.

Question 28

The reaction, A + 2B products, was studied. A timer was started when reagents A and B were mixed, and stopped when a specific quantity of product C accumulated. The data contains initial amounts of reactants used and the time needed to reach the specific quantity of C. Based on the data below, we can conclude that Hint: Remember reaction rate is proportional to 1/time.

A)the reaction is first order with respect to substance A.
B)the reaction is zero order with respect to substance A.
C)the reaction is one-half order with respect to substance A.
D)the reaction is second order with respect to substance A.
E)the reaction is third order with respect to substance B

Question 29

For the reaction, 2M + 2N $\rarr$ 2P + Q, studies on how the initial rate of the reaction varied with concentration were carried out. Some data is given below.

A)the rate law is therefore: rate = k[N]²
B)the rate law is therefore: rate = k[M][N]²
C)the rate law is therefore: rate = k[M][N]
D)the rate law is therefore: rate = k[M]²
E)the rate law is therefore: rate = k[M]²[N]²

Question 30

For the reaction, A + 2B $\rarr$ C + 2D, the following data were obtained .

A)the rate law is therefore: rate = k[A][B]²
B)the rate law is therefore: rate = k[B]
C)the rate law is therefore: rate = k[A]
D)the rate law is therefore: rate = k[A][B]
E)the rate law is therefore: rate = k[A]²[B]

Question 31

For the reaction, A + 2B $\rarr$ C + 2D, some measurements of the initial rate of reaction at varying concentration gave the following data.

A)the rate law is therefore: rate = k[A]²[B]
B)the rate law is therefore: rate = k[A][B]²
C)the rate law is therefore: rate = k[A]²[B]²
D)the rate law is therefore: rate = k[A][B]
E)the rate law is therefore: rate = k[A][B]³

Question 32

The reaction, 2A₂X₄(g) $\rarr$ 2A₂X₃(g)+ X₂(g), was found to be first order. The rate law, therefore, should be:

A)rate = k([A₂X₃]²[X₂])/[A₂X₄]²
B)rate = k[A₂X₄]²
C)rate = k([A₂X₃][X₂])/[A₂X₄]
D)rate = k[A₂X₄]
E)rate = k[A₂X₄]²/([A₂X₃]²[X₂])

Question 33

The data below were obtained in a study on how the rate of a reaction was affected by the concentration of its reactants. The data indicate:

A)the order of the reaction with respect to C cannot be determined.
B)the reaction is second order with respect to C.
C)the reaction is zero order with respect to C.
D)the reaction is first order with respect to C.
E)the order of the reaction with respect to C is minus one.

Question 34

Given these data in a study on how the rate of a reaction was affected by the concentration of the reactants: Hint: When you have three reactants, determine if any of them are 0 order.

A)the reaction is zero order with respect to B.
B)the reaction is first order with respect to B.
C)the reaction order for B cannot be determined.
D)the reaction is second order with respect to B.
E)the reaction order for B is minus one.

Question 35

Given these data in a study on how the rate of a reaction was affected by the concentration of the reactants: Hint: When you have three reactants, determine if any of them are 0 order.

A)the reaction is first order with respect to A.
B)the reaction is second order with respect to A.
C)the reaction is zero order with respect to A.
D)the reaction order for A is minus one (Rate proportional to 1/[A]).
E)the reaction order for A cannot be determined from just this data alone.

Question 36

Given these data in a study on how the rate of a reaction was affected by the concentration of the reactants, what is the numerical value of the rate constant, (k), for this reaction (where units match the data)? Hint: When you have three reactants, determine if any of them are 0 order.

A)2083
B)694
C)417
D)2500
E)83.3

Question 37

What is the order of the reaction with respect to reactant A?Determining A Rate Law From Experimental Data The following data was found for the reaction:A + B $\rarr$ Products

A)Zero
B)First
C)Second
D)Third
E)Fourth

Question 38

What is the order of the reaction with respect to reactant B? Determining A Rate Law From Experimental Data The following data was found for the reactionA + B $\rarr$ Products

A)Zero
B)First
C)Second
D)Third
E)Fourth

Question 39

The data shown below was determined for the reaction A + B $\rarr$ Products.Which of the following is the correct rate law for this reaction?

A)rate = k[A][B]
B)rate = k[A]
C)rate = k[B]²
D)rate = k[B]
E)rate = k[A][B]²

Question 40

The data shown below was determined for the reaction A + B $\rarr$ Products. What is the numerical value of the rate constant, (k), for this reaction?

A)258.2
B)378.8
C)1.72 × 10⁴
D)8.33
E)1.125

Question 41

The data shown below was determined for the reaction A + B $\rarr$ Products.What is the missing value in the table, for the initial rate of the reaction in Experiment 5?

A)1.125
B)0.500
C)2.83
D)1.53
E)2.00

Question 42

The half-life of a chemical reaction was found to be independent of the quantity of reactant which was employed. The reaction is, therefore,

A)possibly first order.
B)definitely first order.
C)zero order.
D)possibly second order.
E)definitely second order.

Question 43

If a reaction involving a single reactant is first order, with a rate constant of 4.50 × 10^-2 s^-1, how much time is required for 75.0% of the initial quantity of reactant to be used up?

A)16.7 seconds
B)30.9 seconds
C)23.1 seconds
D)25.3 seconds
E)11.6 seconds

Question 44

Graph b can best be described as

A)Zero-order rate process.
B)First-order rate process.
C)Second-order rate process.
D)B or C
E)A or C

Question 45

We should determine the reaction order from graph b by

A)plotting [A] vs. time.
B)plotting 1/[A] vs. time.
C)plotting ln[A] vs. time.
D)plotting the square root of concentration vs. time.
E)B and C

Question 46

Concentration vs. time data for a first-order reaction is shown in the graph below. What should be done to determine the half-life of the reaction?

A)Multiply [A] by k
B)Plot 1/[A] vs. time
C)Plot ln[A] vs. time
D)Plot the square root of concentration vs. time
E)B and C

Question 47

The initial concentration of a reactant in a first-order reaction is 0.620 M. What will be its concentration after 3 half-lives have passed?

A)0.0865 M
B)0.0775 M
C)0.310 M
D)0.207 M
E)0.103 M

Question 48

The initial concentration of a reactant in a first-order reaction is 0.860 M. What will be its concentration after 4 half-lives have passed?

A)0.215 M
B)0.0538 M
C)0.250 M
D)0.125 M
E)0.108 M

Question 49

The reaction A ? Products is a zero-order reaction with a rate constant of 4.81 × 10^-3 M s^-1. If the reaction starts with a 33.1 M concentration of A, at what time will the concentration of A be 24.1 M?

A)43.7 min
B)72.8 min
C)661 min
D)1870 min
E)31.2 min

Question 50

In a first-order reaction with only one reagent, the reaction was started with a concentration of reactant equal to 0.0800 M. After exactly two hours, the concentration had fallen to 0.0400 M. What is the molarity after exactly four hours?

A)0.0000 M
B)0.0100 M
C)0.0150 M
D)0.0200 M
E)0.0300 M

Question 51

The decomposition of an aldehyde solution in carbon tetrachloride is a first-order reaction with a rate constant of 1.20 × 10^-3 min^-1. If we start with [aldehyde] = 0.0500 M, what will the concentration of aldehyde be 150 minutes later?

A)0.00900 M
B)0.0418 M
C)0.00926 M
D)0.00499 M
E)0.000333 M

Question 52

The initial concentration of a reactant in a first order reaction is 0.620 M. What will be its concentration after 3 half-lives?

A)0.0865 M
B)0.310 M
C)0.0775 M
D)0.103 M
E)0.207 M

Question 53

For the reaction, A $\rarr$ B + C, the rate law is rate = k[A]. If it takes 80.0 seconds for 70.0% of a 10.0 gram sample of A to be transformed into products, what is the value of the rate constant?

A)0.00450 s^-1
B)0.0290 s^-1
C)0.00530 s^-1
D)0.0150 s^-1
E)5.40 s^-1

Question 54

For the reaction, A $\rarr$ B + C, the rate law is rate = k[A] where k = 0.0175 s^-1. How long will it take to reach 35.0 g from a 100.0 g sample?

A)1.00 min
B)7.77 min
C)0.0184 s
D)39.6 s
E)1.06 s

Question 55

The reaction of substance A with substance C was carefully studied under conditions where the [C] remained essentially constant. The graph of [A] vs. time gave a straight line while the graph of ln[A] vs. time and that of 1/[A] vs. time both gave curves.

A)The reaction is therefore zero order with respect to A.
B)The reaction is therefore one-half order with respect to A.
C)The reaction is therefore first order with respect to A.
D)The reaction is therefore second order with respect to A.
E)The reaction is therefore third order with respect to A.

Question 56

A reaction is first-order overall. For a given sample, its initial rate is 0.0200 mol L^-1 s^-1, and 25.0 days later its rate dropped to 6.25 × 10^-4 mol L^-1 s^-1. What is its half-life?

A)25.0 days
B)50.0 days
C)12.5 days
D)5.0 days
E)37.5 days

Question 57

In a first-order reaction with only one reagent, the reaction was started with a concentration of reactant equal to 0.0800 M. After exactly two hours, the concentration had fallen to 0.0400 M. What is the molarity after exactly six hours?

A)0.0000 M
B)0.0100 M
C)0.0150 M
D)0.0200 M
E)0.0300 M

Question 58

The rate constant for a first-order decomposition reaction is 0.0111 min^-1. What is the half-life of the reaction?

A)111 min
B)62.4 min
C)5000 sec
D)31.25 min
E)27.1 min

Question 59

Given a reaction, 2A + B $\rarr$ P, for which the rate law is rate = k[A]. Which equation or statement is true?

A)[A] = 1/kt
B)ln[A] = k/t
C)1/[A] = kt
D)The half-life is 0.693/k.
E)e^[A] = kt

Question 60

In a first-order reaction, what fraction of the reactant will remain after 4 half-lives?

A)1/16
B)1/8
C)1/9
D)1/4
E)1/3

Question 61

In a first-order reaction, what fraction of the reactant will remain after 3 half-lives?

A)1/16
B)1/8
C)1/9
D)1/4
E)1/3

Question 62

A first-order reaction has a rate constant of 0.00318 min¹. The half-life of this reaction is, therefore,

A)94.7 minutes.
B)218 minutes.
C)31.4 minutes.
D)5.24 seconds.
E)68.6 minutes.

Question 63

For the reaction 2A + B $\rarr$ Products The rate equation was found to be rate = k[A]². If the rate constant was found to be 0.045 M^-1 min^-1 and the reaction started with an initial concentration of A equal to 0.50 M, what is the concentration of A after 30.0 minutes?

A)0.011 M
B)0.13 M
C)0.30 M
D)1.54 M
E)3.35 M

Question 64

For the reaction 2A + B $\rarr$ Products The rate equation was found to be rate = k[A]². If the rate constant was found to be 0.035 M^-1 min^-1 and the reaction started with an initial concentration of A equal to 0.50 M, how long will it take for the concentration of A to reach 0.25 M?

A)4.2 sec
B)57.1 min
C)49.8 min
D)1.05 sec
E)53.5 min

Question 65

The reaction A $\rarr$ Products is a zero-order reaction with a rate constant of 2.56 × 10^-3 M s^-1. If the concentration of A is 75.6 M after 12.7 minutes, what was the initial concentration of A?

A)838 M
B)100 M
C)75.6 M
D)77.6 M
E)73.6 M

Question 66

At a certain temperature the second-order reaction NOCl(g) $\rarr$ NO(g)+ 1/2Cl₂(g)is 50% complete after 6.23 hours when the initial concentration of NOCl is 4.78 mol/L. How long will it take for the reaction to be 75% complete?

A)18.7 hr
B)17.5 hr
C)8.2 hr
D)31.5 hr
E)12.5 hr.

Question 67

Charcoal taken from the site of an ancient village was found to have a ¹⁴C to ¹²C ratio of one-third that is found in living plant life. Using this data, what is the age of the charcoal sample? The half-life of ¹⁴C is 5730 years.

A)12,300 yrs.
B)9,080 yrs.
C)6,950 yrs.
D)1,800 yrs.
E)2510 yrs.

Question 68

For a first-order reaction with a single reactant, after 230.0 seconds, 10.0% of the reactant remains. The rate constant for the reaction is, therefore,

A)0.000640 s^-1
B)0.0100 s^-1
C)100 s^-1
D)0.0510 s^-1
E)0.0915 s^-1

Question 69

Graph a can best be described as a

A)Zero-order rate process.
B)First-order rate process.
C)Second-order rate process.
D)B or C
E)A or C

Question 70

The reaction of substance A with substance C was carefully studied under conditions where the [C] remained essentially constant. The graphs of [A] vs. time and that of ln[A] vs. time both gave curves, but the graph of 1/[A] vs. time gave a straight line.

A)The reaction is therefore zero order with respect to A.
B)The reaction is therefore one-half order with respect to A.
C)The reaction is therefore first order with respect to A.
D)The reaction is therefore second order with respect to A.
E)The reaction is therefore third order with respect to A.

Question 71

A sample of Peruvian corn was found to have a ¹⁴C to ¹²C ratio of 8.0 × 10^-13. Similar corn samples taken present day have a ¹⁴C to ¹²C ratio of 1.2 × 10^-12. Using this data, what is the age of the Peruvian corn sample?Hint: The half-life of 14C is 5730 years.

A)2.5 yrs.
B)15,700 yrs.
C)5,240 yrs.
D)1,470 yrs.
E)3,350 yrs.

Question 72

What two factors influence the effectiveness of molecular collisions in producing chemical change?
1. The molar masses of the reactants
2. The activation energy
3. The pressure
4. The orientation of the reactants

A)3 and 4
B)1 and 3
C)1 and 2
D)2 and 4
E)2 and 3

Question 73

When there is an increase in temperature of a system the rate of reaction often increases. Which of the following best explains why this happens?
1. The concentrations increase with temperature.
2. The number of collisions with the sufficient kinetic energy increase with temperature.
3. The number of collisions per unit time increases with temperature.
4. The orientation of the molecules change with temperature.

A)3 and 4
B)1 and 3
C)1 and 2
D)2 and 4
E)2 and 3

Question 74

For a one step reaction, the activation energy for the forward reaction is 40.0 kJ mol^-1, and the heat of reaction is 20.0 kJ mol^-1. Which statement below is true?

A)The activation energy of the forward reaction would be affected to a greater extent than the activation energy of the reverse reaction by addition of a catalyst.
B)The value for the heat of reaction would be decreased by addition of a catalyst.
C)The reaction is endothermic.
D)The reverse reaction has a higher activation energy than the forward reaction.
E)The reaction rate would be decreased by an increase in temperature.

Question 75

For a one-step reaction, the activation energy for the forward reaction is 40.0 kJ mol^-1, and the heat of reaction is 20.0 kJ mol^-1. Calculate the activation energy for the reverse reaction.

A)+60.0 kJ mol^-1
B)-20.0 kJ mol^-1
C)-1200 kJ mol^-1
D)+20.0 kJ mol^-1
E)+1200 kJ mol^-1

Question 76

The reaction progress for a given reaction is shown below. Which corresponds to the activation energy of the forward reaction, E_a?

A)A
B)B
C)C
D)D
E)none of these

Question 77

The reaction progress for a given reaction is shown below. Which corresponds to the overall energy change of the reaction, ? (The heat of reaction)

A)A
B)B
C)C
D)D
E)none of these

Question 78

The reaction progress for a given reaction is shown below. The point on the diagram where the energy of the system is at a maximum is called the

A)transition state.
B)critical point.
C)formation energy of the reactants.
D)formation energy of the products.
E)rate determining state.

Question 79

The reaction progress for a given reaction is shown below. Which corresponds to the activation energy of the reverse reaction, E_a?

A)A
B)B
C)C
D)D
E)none of these

Question 80

The reaction A + 3B $\rarr$ D + F was studied, and the following mechanism was determined The step with largest activation energy is

A)the first step.
B)the second step.
C)the third step.
D)None of the steps has an activation energy.
E)All of the steps have the same activation energy.