Question 1

The reaction
3C + D $\rightarrow$ products
Has rate = k[D] and has a half-life of 1.29 s.If initially [D] = 0.820,What is the concentration of D after 2.55 s?

Accepted Answer

A)  0.21 
B)  0.12 
C)  0.56 
D)  0.28 
E)  0.41 
A)  0.21 
B)  0.12 
C)  0.56 
D)  0.28 
E)  0.41

Question 2

Given:
5Br-(aq)+ BrO3-(aq)+ 6H+(aq)$\rightarrow$3Br2(aq)+ 3H2O(l)
Rate = k[Br-][ BrO3-][H+]2 
The overall order of the reaction and the order with respect to H+ are

Accepted Answer

A)  4 and 2. 
B)  5 and 6. 
C)  3 and 2. 
D)  5 and 2. 
E)  6 and 2. 
A)  4 and 2. 
B)  5 and 6. 
C)  3 and 2. 
D)  5 and 2. 
E)  6 and 2.

Question 3

The reaction [(CN)5CoOH2]2-(aq)+ SCN-(aq)$\rightarrow$[(CN)5CoSCN]3-+ H2O(l)
has the rate law,rate=k[(CN)5CoOH22-].Postulate a mechanism for this reaction.

Accepted Answer

[(CN)₅CoOH₂]²

Question 4

For the reaction
HO(g)+ H2(g)$\rightarrow$H2O(g)+ H(g)
A plot of
$\ln k$
Versus 1/T gives a straight line with a slope equal to -5.1 * 103 K.What is the activation energy for the reaction?

Accepted Answer

A)  42 kJ.mol-1  
B)  98 kJ.mol-1  
C)  0.61 kJ.mol-1  
D)  5.1 kJ.mol-1  
E)  12 kJ.mol-1  
A)  42 kJ.mol-1  
B)  98 kJ.mol-1  
C)  0.61 kJ.mol-1  
D)  5.1 kJ.mol-1  
E)  12 kJ.mol-1

Question 5

The fraction of molecules that collide with a kinetic energy equal to the activation energy for a reaction decreases rapidly with an increase in temperature.

Accepted Answer

A) True 
 B)False

Question 6

The concentration.time curves for two sets of reactions, A/B and C/D,
Are:  
Which set of reactions has the largest rate constant?

Accepted Answer

The answer of The concentration.time curves for two sets of...

Question 7

The rates of first-order and second-order reactions do not change with elapsed time

Accepted Answer

A) True 
 B)False

Question 8

The rate law for the following mechanism is
NO2(g)+ F2(g)$\rightarrow$NO2F(g)+ F(g)
K1,
Slow
F(g)+ NO2(g)$\rightarrow$NO2F(g)
K2,
Fast

Accepted Answer

A)  rate = k2[NO2]2.  
B)  rate = k2[NO2][F]. 
C)  rate = k1[NO2][F2]. 
D)  rate = k1k2[NO2]2.  
E)  rate = k1[NO2F][F]. 
A)  rate = k2[NO2]2.  
B)  rate = k2[NO2][F]. 
C)  rate = k1[NO2][F2]. 
D)  rate = k1k2[NO2]2.  
E)  rate = k1[NO2F][F].

Question 9

What is the half-life of a second order reaction?

Accepted Answer

The answer of What is the half-life of a second...

Question 10

The reaction between nitrogen dioxide and carbon monoxide is thought to occur by the mechanism
2NO2(g$\rightarrow$NO3(g)+ NO(g) 
K1,Slow
NO3(g)+ CO(g)$\rightarrow$NO2(g)+ CO2(g)
K2,Fast
The rate law for this mechanism is

Accepted Answer

A)  rate = k1k2[NO2]2[CO]. 
B)  rate = (k1/k2)[NO2]2[CO]. 
C)  rate = k1[NO3][NO]. 
D)  rate = k2[NO3][CO]. 
E)  rate = k1[NO2]2.  
A)  rate = k1k2[NO2]2[CO]. 
B)  rate = (k1/k2)[NO2]2[CO]. 
C)  rate = k1[NO3][NO]. 
D)  rate = k2[NO3][CO]. 
E)  rate = k1[NO2]2.

Question 11

All of the following statements with respect to the effect of a catalyst on a reaction are true except:

Accepted Answer

A)  A catalyst has no effect on the equilibrium composition of the reaction. 
B)  A catalyst provides a lower activation energy for the reaction. 
C)  When a reaction is catalyzed, both forward and reverse reactions are accelerated. 
D)  A catalyst speeds up a reaction by providing an alternate pathway for the reaction. 
E)  When a catalyst speeds up a reaction, the rate law stays the same. 
A)  A catalyst has no effect on the equilibrium composition of the reaction. 
B)  A catalyst provides a lower activation energy for the reaction. 
C)  When a reaction is catalyzed, both forward and reverse reactions are accelerated. 
D)  A catalyst speeds up a reaction by providing an alternate pathway for the reaction. 
E)  When a catalyst speeds up a reaction, the rate law stays the same.

Question 12

The rate of formation of oxygen in the reaction
2N2O5(g)$\rightarrow$ 4NO2(g)+ O2(g)Is 2.28 (mol O2).L-1.s-1.What is the rate of formation of NO2?

Accepted Answer

A)  0.57 (mol NO2).L-1.s-1  
B)  9.12 (mol NO2).L-1.s-1  
C)  2.28 (mol NO2).L-1.s-1  
D)  1.14 (mol NO2).L-1.s-1  
E)  4.56 (mol NO2).L-1.s-1  
A)  0.57 (mol NO2).L-1.s-1  
B)  9.12 (mol NO2).L-1.s-1  
C)  2.28 (mol NO2).L-1.s-1  
D)  1.14 (mol NO2).L-1.s-1  
E)  4.56 (mol NO2).L-1.s-1

Question 13

Consider the reaction for the dimerization of butadiene(g)at a certain temperature.
2C4H6(g)$\rightarrow$ C8H12(g)
 rate = k[C4H6]2.When the initial concentration of butadiene is 0.500 M,
the time required for 80% dimerization is measured at 11.4 s.What is the rate constant for the dimerization?

Accepted Answer

0.704 M<sup>-</sup><

Question 14

Consider the reaction
2A $\rightarrow$ B,Rate = k[A]2
If the rate of appearance of B is followed,derive the experimental rate constant.

Accepted Answer

k is deter

Question 15

A possible mechanism for the reaction A + B + D $\rightarrow$ E + F is
A + B
k1,k-1,fast
$f$ 
C
C + D $\rightarrow$ E + F
k2
where C is a reactive intermediate present in very low concentrations.
Calculate the steady state concentration of C in terms of the rate constants for the individual steps and the concentrations of the reactants.

Accepted Answer

[C] = k₁[A]

Question 16

It is important to distinguish between the reaction rate and the rate constant.The units of reaction rate are M.s-1.

Accepted Answer

A) True 
 B)False

Question 17

The concentration-time dependence for two first order reactions is:    
Which reaction has the greater t½?

Accepted Answer

the reacti

Question 18

For a given first-order reaction, after 2.00 min,20% of the reactants remain.Calculate the rate constant for the reaction.

Accepted Answer

A)  0.0134 s-1  
B)  0.000808 s-1  
C)  74.6 s-1  
D)  0.00582 s-1  
E)  0.00186 s-1  
A)  0.0134 s-1  
B)  0.000808 s-1  
C)  74.6 s-1  
D)  0.00582 s-1  
E)  0.00186 s-1

Question 19

The reaction
2ClO2(g)+ F2(g)$\rightarrow$2FClO2(g)
Is first order in both ClO2 and F2.When the initial concentrations of ClO2 and F2 are equal,The rate after 25% of the F2 has reacted is what percent of the initial rate?

Accepted Answer

A)  75.0% 
B)  18.8% 
C)  37.5% 
D)  28.1% 
E)  12.5% 
A)  75.0% 
B)  18.8% 
C)  37.5% 
D)  28.1% 
E)  12.5%

Question 20

In the reaction: A + B $\rightarrow$ C, where: rate = k[A][B], Which of the following is true?

Accepted Answer

A)  The rate is first order with respect to A 
B)  The rate is first order with respect to B 
C)  The rate is second order overall 
D)  All of the above are true. 
A)  The rate is first order with respect to A 
B)  The rate is first order with respect to B 
C)  The rate is second order overall 
D)  All of the above are true.

The reaction 3C + D $\rightarrow$ products Has rate = k[D] and has a half-life of 1.29 s.If initially [D] = 0.820,What is the concentration of D after 2.55 s?

Given: 5Br^-(aq)+ BrO₃^-(aq)+ 6H⁺(aq) $\rightarrow$ 3Br₂(aq)+ 3H₂O(l) Rate = k[Br^-][ BrO₃^-][H⁺]² The overall order of the reaction and the order with respect to H⁺ are

The reaction [(CN)₅CoOH₂]²^-(aq)+ SCN^-(aq) $\rightarrow$ [(CN)₅CoSCN]³^-+ H₂O(l) has the rate law,rate=k[(CN)₅CoOH₂2^-].Postulate a mechanism for this reaction.

For the reaction HO(g)+ H₂(g) $\rightarrow$ H₂O(g)+ H(g) A plot of $\ln k$ Versus 1/T gives a straight line with a slope equal to -5.1 * 10³ K.What is the activation energy for the reaction?

The fraction of molecules that collide with a kinetic energy equal to the activation energy for a reaction decreases rapidly with an increase in temperature.

The concentration.time curves for two sets of reactions, A/B and C/D, Are: Which set of reactions has the largest rate constant?

The rates of first-order and second-order reactions do not change with elapsed time

The rate law for the following mechanism is NO₂(g)+ F₂(g) $\rightarrow$ NO₂F(g)+ F(g) K₁, Slow F(g)+ NO₂(g) $\rightarrow$ NO₂F(g) K₂, Fast

What is the half-life of a second order reaction?

The reaction between nitrogen dioxide and carbon monoxide is thought to occur by the mechanism 2NO₂(g $\rightarrow$ NO₃(g)+ NO(g) K₁,Slow NO₃(g)+ CO(g) $\rightarrow$ NO₂(g)+ CO₂(g) K₂,Fast The rate law for this mechanism is

All of the following statements with respect to the effect of a catalyst on a reaction are true except:

The rate of formation of oxygen in the reaction 2N₂O₅(g) $\rightarrow$ 4NO₂(g)+ O₂(g)Is 2.28 (mol O₂).L^-¹.s^-¹.What is the rate of formation of NO₂?

Consider the reaction 2A $\rightarrow$ B,Rate = k[A]² If the rate of appearance of B is followed,derive the experimental rate constant.

It is important to distinguish between the reaction rate and the rate constant.The units of reaction rate are M.s^-¹.

The concentration-time dependence for two first order reactions is: Which reaction has the greater t_½?

For a given first-order reaction, after 2.00 min,20% of the reactants remain.Calculate the rate constant for the reaction.

The reaction 2ClO₂(g)+ F₂(g) $\rightarrow$ 2FClO₂(g) Is first order in both ClO₂ and F₂.When the initial concentrations of ClO₂ and F₂ are equal,The rate after 25% of the F₂ has reacted is what percent of the initial rate?

In the reaction: A + B $\rightarrow$ C, where: rate = k[A][B], Which of the following is true?

Atoms

Molecules

States of Matter

Thermodynamics

Equilibrium

Reactions

The Main-Group Elements

The D-Block Elements

Nuclear Chemistry

Organic Chemistry

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Exam 7: Kinetics

The reaction 3C + D →\rightarrow→ products Has rate = k[D] and has a half-life of 1.29 s.If initially [D] = 0.820,What is the concentration of D after 2.55 s?

Given: 5Br-(aq)+ BrO3-(aq)+ 6H+(aq) →\rightarrow→ 3Br2(aq)+ 3H2O(l) Rate = k[Br-][ BrO3-][H+]2 The overall order of the reaction and the order with respect to H+ are

The reaction [(CN)5CoOH2]2-(aq)+ SCN-(aq) →\rightarrow→ [(CN)5CoSCN]3-+ H2O(l) has the rate law,rate=k[(CN)5CoOH22-].Postulate a mechanism for this reaction.

For the reaction HO(g)+ H2(g) →\rightarrow→ H2O(g)+ H(g) A plot of ln⁡k\ln klnk Versus 1/T gives a straight line with a slope equal to -5.1 * 103 K.What is the activation energy for the reaction?

The fraction of molecules that collide with a kinetic energy equal to the activation energy for a reaction decreases rapidly with an increase in temperature.

The concentration.time curves for two sets of reactions, A/B and C/D, Are: Which set of reactions has the largest rate constant?

The rates of first-order and second-order reactions do not change with elapsed time

The rate law for the following mechanism is NO2(g)+ F2(g) →\rightarrow→ NO2F(g)+ F(g) K1, Slow F(g)+ NO2(g) →\rightarrow→ NO2F(g) K2, Fast

What is the half-life of a second order reaction?

The reaction between nitrogen dioxide and carbon monoxide is thought to occur by the mechanism 2NO2(g →\rightarrow→ NO3(g)+ NO(g) K1,Slow NO3(g)+ CO(g) →\rightarrow→ NO2(g)+ CO2(g) K2,Fast The rate law for this mechanism is

All of the following statements with respect to the effect of a catalyst on a reaction are true except:

The rate of formation of oxygen in the reaction 2N2O5(g) →\rightarrow→ 4NO2(g)+ O2(g)Is 2.28 (mol O2).L-1.s-1.What is the rate of formation of NO2?

Consider the reaction 2A →\rightarrow→ B,Rate = k[A]2 If the rate of appearance of B is followed,derive the experimental rate constant.

It is important to distinguish between the reaction rate and the rate constant.The units of reaction rate are M.s-1.

The concentration-time dependence for two first order reactions is: Which reaction has the greater t½?

For a given first-order reaction, after 2.00 min,20% of the reactants remain.Calculate the rate constant for the reaction.

The reaction 2ClO2(g)+ F2(g) →\rightarrow→ 2FClO2(g) Is first order in both ClO2 and F2.When the initial concentrations of ClO2 and F2 are equal,The rate after 25% of the F2 has reacted is what percent of the initial rate?

In the reaction: A + B →\rightarrow→ C, where: rate = k[A][B], Which of the following is true?

Atoms

Molecules

States of Matter

Thermodynamics

Equilibrium

Reactions

The Main-Group Elements

The D-Block Elements

Nuclear Chemistry

Organic Chemistry

Filters

The reaction 3C + D $\rightarrow$ products Has rate = k[D] and has a half-life of 1.29 s.If initially [D] = 0.820,What is the concentration of D after 2.55 s?

Given: 5Br^-(aq)+ BrO₃^-(aq)+ 6H⁺(aq) $\rightarrow$ 3Br₂(aq)+ 3H₂O(l) Rate = k[Br^-][ BrO₃^-][H⁺]² The overall order of the reaction and the order with respect to H⁺ are

The reaction [(CN)₅CoOH₂]²^-(aq)+ SCN^-(aq) $\rightarrow$ [(CN)₅CoSCN]³^-+ H₂O(l) has the rate law,rate=k[(CN)₅CoOH₂2^-].Postulate a mechanism for this reaction.

For the reaction HO(g)+ H₂(g) $\rightarrow$ H₂O(g)+ H(g) A plot of $\ln k$ Versus 1/T gives a straight line with a slope equal to -5.1 * 10³ K.What is the activation energy for the reaction?

The rate law for the following mechanism is NO₂(g)+ F₂(g) $\rightarrow$ NO₂F(g)+ F(g) K₁, Slow F(g)+ NO₂(g) $\rightarrow$ NO₂F(g) K₂, Fast

The reaction between nitrogen dioxide and carbon monoxide is thought to occur by the mechanism 2NO₂(g $\rightarrow$ NO₃(g)+ NO(g) K₁,Slow NO₃(g)+ CO(g) $\rightarrow$ NO₂(g)+ CO₂(g) K₂,Fast The rate law for this mechanism is

The rate of formation of oxygen in the reaction 2N₂O₅(g) $\rightarrow$ 4NO₂(g)+ O₂(g)Is 2.28 (mol O₂).L^-¹.s^-¹.What is the rate of formation of NO₂?

Consider the reaction 2A $\rightarrow$ B,Rate = k[A]² If the rate of appearance of B is followed,derive the experimental rate constant.

It is important to distinguish between the reaction rate and the rate constant.The units of reaction rate are M.s^-¹.

The concentration-time dependence for two first order reactions is: Which reaction has the greater t_½?

The reaction 2ClO₂(g)+ F₂(g) $\rightarrow$ 2FClO₂(g) Is first order in both ClO₂ and F₂.When the initial concentrations of ClO₂ and F₂ are equal,The rate after 25% of the F₂ has reacted is what percent of the initial rate?

In the reaction: A + B $\rightarrow$ C, where: rate = k[A][B], Which of the following is true?