SO2Cl2 decomposes in the gas phase by the reaction SO2Cl2 (g) →SO2 (g) + Cl2 (g) The reaction is first order in SO2Cl2 and the rate constant is 3.0 × 10- 6 s- 1at 600 K. A vessel is charged with 2.4 atm of SO2Cl2 at 600 K. The partial pressure of SO2Cl2 at 3.0 × 105 s is Atm)

A) 1.4 × 105 B) 0.76 C) 0.29 D) 2.2 E) 0.98 A) 1.4 × 105 B) 0.76 C) 0.29 D) 2.2 E) 0.98

The combustion of ethylene proceeds by the reaction C2H4 (g) + 3O2 (g) →2CO2 (g) + 2H2O (g) When the rate of disappearance of O2 is 0.28 M s- 1, the rate of appearance of CO2 is _ _ M s- 1.

A) 0.84 B) 0.42 C) 0.56 D) 0.093 E) 0.19 A) 0.84 B) 0.42 C) 0.56 D) 0.093 E) 0.19

The isomerization of methylisonitrile to acetonitrile CH3NC (g) → CH3CN (g) Is first order in CH3NC. The half life of the reaction is 1.60 × 105 s at 444 K. The rate constant when the initial [CH3NC] is 0.030 M is _ s- 1.

A) 2.08 × 10- 4 B) 4.80 × 103 C) 7.10 × 107 D) 2.31 × 105 E) 4.33 × 10- 6 A) 2.08 × 10- 4 B) 4.80 × 103 C) 7.10 × 107 D) 2.31 × 105 E) 4.33 × 10- 6

The elementary reaction 2NO2 (g) → 2NO (g) + O2 (g) Is second order in NO2 and the rate constant at 501 K is 7.93 × 10- 3 M- 1s- 1. The reaction half- life at this temperature when [NO2]0 = 0.450 M is s.

A) 126 B) 0.011 C) 3.6 × 10- 3 D) 280 E) 87 A) 126 B) 0.011 C) 3.6 × 10- 3 D) 280 E) 87

The data in the table below were obtained for the reaction: 2 ClOS1U1B12 S1U1B0(aq) + 2 OHS1U1P1- S1S1P0(aq) → ClOS1U1B13S1U1B0S1U1P1- S1S1P0(aq) + ClOS1U1B12S1U1B0S1U1P1- S1S1P0(aq) + HS1U1B12S1U1B0O (1) -What is the order of the reaction with respect to OH- ?

A) 0 B) 1 C) 2 D) 3 E) 4 A) 0 B) 1 C) 2 D) 3 E) 4

At elevated temperatures, methylisonitrile (CH3NC) isomerizes to acetonitrile (CH3CN): CH3NC (g) → CH3CN (g) At the start of the experiment, there are 0.200 mol of reactant (CH3NC) and 0 mol of product (CH3CN) in the reaction vessel. After 25 min of reaction, 0.108 mol of reactant (CH3NC) remain. The average rate of decomposition of methyl isonitrile, CH3NC, in this 25 min period is mol/min.

A) 0.54 B) 3.7 × 10- 3 C) 4.3 × 10- 3 D) 0.092 E) 2.3 A) 0.54 B) 3.7 × 10- 3 C) 4.3 × 10- 3 D) 0.092 E) 2.3

Nitrogen dioxide decomposes to nitric oxide and oxygen via the reaction: 2NO2 → 2NO + O2 In a particular experiment at 300°C, [NO2] drops from 0.0100 to 0.00650 M in 100 s. The rate of disappearance of NO2 for this period is _ M/s.

A) 0.35 B) 1.8 × 10- 3 C) 3.5 × 10- 3 D) 7.0 × 10- 3 E) 3.5 × 10- 5 A) 0.35 B) 1.8 × 10- 3 C) 3.5 × 10- 3 D) 7.0 × 10- 3 E) 3.5 × 10- 5

Exam 14: Chemical Kinetics

A flask is charged with 0.124 mol of A and allowed to react to form B according to the reaction A(g) -B(g). The following data are obtained for [A] as the reaction proceeds: -How many moles of B are present at 10 s?

(Multiple Choice)

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Question 21

The data in the table below were obtained for the reaction: A + B - P -The order of the reaction in B is _ .

(Multiple Choice)

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Question 22

The reaction A - B is first order in [A]. Consider the following data. -The rate constant for this reaction is s^-¹.

(Multiple Choice)

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Question 23

SO₂Cl₂decomposes in the gas phase by the reaction SO₂Cl₂(g) →SO₂(g) + Cl₂(g) The reaction is first order in SO₂Cl₂and the rate constant is 3.0 × 10^-⁶s^-¹at 600 K. A vessel is charged with 2.4 atm of SO₂Cl₂at 600 K. The partial pressure of SO₂Cl₂at 3.0 × 10⁵s is Atm)

(Multiple Choice)

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Question 24

The combustion of ethylene proceeds by the reaction C₂H₄(g) + 3O₂(g) →2CO₂(g) + 2H₂O (g) When the rate of disappearance of O₂is 0.28 M s^-¹, the rate of appearance of CO₂is _ _ M s^-¹.

(Multiple Choice)

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Question 25

The primary source of the specificity of enzymes is .

(Multiple Choice)

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Question 26

Reaction rates are affected by reactant concentrations and temperature. This is accounted for by the .

(Short Answer)

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Question 27

The isomerization of methylisonitrile to acetonitrile CH₃NC (g) → CH₃CN (g) Is first order in CH₃NC. The half life of the reaction is 1.60 × 10⁵s at 444 K. The rate constant when the initial [CH₃NC] is 0.030 M is _ s^-¹.

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Question 28

The relationship of absorbed light to the concentration of the substance absorbing the light is governed by .

(Short Answer)

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Question 29

The elementary reaction 2NO₂(g) → 2NO (g) + O₂(g) Is second order in NO₂and the rate constant at 501 K is 7.93 × 10^-³M^-¹s^-¹. The reaction half- life at this temperature when [NO₂]₀= 0.450 M is s.

(Multiple Choice)

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Question 30

The data in the table below were obtained for the reaction: 2 ClO₂(aq) + 2 OH^-(aq) → ClO₃^-(aq) + ClO₂^-(aq) + H₂O (1) -What is the order of the reaction with respect to OH^-?

(Multiple Choice)

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Question 31

If the rate law for the reaction is first order in A and second order in B, then the rate law is rate = .

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Question 32

At elevated temperatures, methylisonitrile (CH₃NC) isomerizes to acetonitrile (CH₃CN): CH₃NC (g) → CH₃CN (g) At the start of the experiment, there are 0.200 mol of reactant (CH₃NC) and 0 mol of product (CH₃CN) in the reaction vessel. After 25 min of reaction, 0.108 mol of reactant (CH₃NC) remain. The average rate of decomposition of methyl isonitrile, CH₃NC, in this 25 min period is mol/min.

(Multiple Choice)

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Question 33

Consider the following reaction: 3A - 2B The average rate of appearance of B is given by O[B]/Ot. Comparing the rate of appearance of B and the rate of disappearance of A, we get O[B]/Ot = × (- O[A]/Ot).

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Question 34

The rate of a reaction depends on _.

(Multiple Choice)

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Question 35

A flask is charged with 0.124 mol of A and allowed to react to form B according to the reaction A(g) -B(g). The following data are obtained for [A] as the reaction proceeds: -The average rate of appearance of B between 20 s and 30 s is mol/s.

(Multiple Choice)

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Question 36

The minimum energy to initiate a chemical reaction is the .

(Short Answer)

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Question 37

The average rate disappearance of A between 20 s and 30 s is mol/s.

(Multiple Choice)

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Question 38

Nitrogen dioxide decomposes to nitric oxide and oxygen via the reaction: 2NO₂→ 2NO + O₂ In a particular experiment at 300°C, [NO₂] drops from 0.0100 to 0.00650 M in 100 s. The rate of disappearance of NO₂for this period is _ M/s.

(Multiple Choice)

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Question 39

The number of molecules that participate as reactants defines the of the reaction.

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Question 40

Showing 21 - 40 of 110

Exam 14: Chemical Kinetics

A flask is charged with 0.124 mol of A and allowed to react to form B according to the reaction A(g) -B(g). The following data are obtained for [A] as the reaction proceeds: -How many moles of B are present at 10 s?

The data in the table below were obtained for the reaction: A + B - P -The order of the reaction in B is _ .

The reaction A - B is first order in [A]. Consider the following data. -The rate constant for this reaction is s- 1.

SO2Cl2 decomposes in the gas phase by the reaction SO2Cl2 (g) →SO2 (g) + Cl2 (g) The reaction is first order in SO2Cl2 and the rate constant is 3.0 × 10- 6 s- 1at 600 K. A vessel is charged with 2.4 atm of SO2Cl2 at 600 K. The partial pressure of SO2Cl2 at 3.0 × 105 s is Atm)

The combustion of ethylene proceeds by the reaction C2H4 (g) + 3O2 (g) →2CO2 (g) + 2H2O (g) When the rate of disappearance of O2 is 0.28 M s- 1, the rate of appearance of CO2 is _ _ M s- 1.

The primary source of the specificity of enzymes is .

Reaction rates are affected by reactant concentrations and temperature. This is accounted for by the .

The isomerization of methylisonitrile to acetonitrile CH3NC (g) → CH3CN (g) Is first order in CH3NC. The half life of the reaction is 1.60 × 105 s at 444 K. The rate constant when the initial [CH3NC] is 0.030 M is _ s- 1.

The relationship of absorbed light to the concentration of the substance absorbing the light is governed by .

The elementary reaction 2NO2 (g) → 2NO (g) + O2 (g) Is second order in NO2 and the rate constant at 501 K is 7.93 × 10- 3 M- 1s- 1. The reaction half- life at this temperature when [NO2]0 = 0.450 M is s.

The data in the table below were obtained for the reaction: 2 ClO2 (aq) + 2 OH- (aq) → ClO3- (aq) + ClO2- (aq) + H2O (1) -What is the order of the reaction with respect to OH- ?

If the rate law for the reaction is first order in A and second order in B, then the rate law is rate = .

Consider the following reaction: 3A - 2B The average rate of appearance of B is given by O[B]/Ot. Comparing the rate of appearance of B and the rate of disappearance of A, we get O[B]/Ot = × (- O[A]/Ot).

The rate of a reaction depends on _.

A flask is charged with 0.124 mol of A and allowed to react to form B according to the reaction A(g) -B(g). The following data are obtained for [A] as the reaction proceeds: -The average rate of appearance of B between 20 s and 30 s is mol/s.

The minimum energy to initiate a chemical reaction is the .

The average rate disappearance of A between 20 s and 30 s is mol/s.

Nitrogen dioxide decomposes to nitric oxide and oxygen via the reaction: 2NO2 → 2NO + O2 In a particular experiment at 300°C, [NO2] drops from 0.0100 to 0.00650 M in 100 s. The rate of disappearance of NO2 for this period is _ M/s.

The number of molecules that participate as reactants defines the of the reaction.

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The reaction A - B is first order in [A]. Consider the following data. -The rate constant for this reaction is s^-¹.

The combustion of ethylene proceeds by the reaction C₂H₄(g) + 3O₂(g) →2CO₂(g) + 2H₂O (g) When the rate of disappearance of O₂is 0.28 M s^-¹, the rate of appearance of CO₂is _ _ M s^-¹.

The isomerization of methylisonitrile to acetonitrile CH₃NC (g) → CH₃CN (g) Is first order in CH₃NC. The half life of the reaction is 1.60 × 10⁵s at 444 K. The rate constant when the initial [CH₃NC] is 0.030 M is _ s^-¹.

The elementary reaction 2NO₂(g) → 2NO (g) + O₂(g) Is second order in NO₂and the rate constant at 501 K is 7.93 × 10^-³M^-¹s^-¹. The reaction half- life at this temperature when [NO₂]₀= 0.450 M is s.

The data in the table below were obtained for the reaction: 2 ClO₂(aq) + 2 OH^-(aq) → ClO₃^-(aq) + ClO₂^-(aq) + H₂O (1) -What is the order of the reaction with respect to OH^-?

Nitrogen dioxide decomposes to nitric oxide and oxygen via the reaction: 2NO₂→ 2NO + O₂ In a particular experiment at 300°C, [NO₂] drops from 0.0100 to 0.00650 M in 100 s. The rate of disappearance of NO₂for this period is _ M/s.