Given the following proposed mechanism,predict the rate law for the overall reaction. $\quad$A2 + 2B → 2AB (overall reaction) $\quad$$\underline{\text{Mechanism}}$ $\quad$A2 ⇌ 2A $\quad$$\quad$ fast $\quad$A + B → AB $\quad$slow

A) Rate = k[A][B] B) Rate = k[A2][B] C) Rate = k[A2][B]1/2 D) Rate = k[A2] E) Rate = k[A2]1/2[B] A) Rate = k[A][B] B) Rate = k[A2][B] C) Rate = k[A2][B]1/2 D) Rate = k[A2] E) Rate = k[A2]1/2[B]

Without performing complex calculations,determine the order of a reaction that has the following initial rates for the specified starting concentration: \[\begin{array} { l | l } { [ \mathrm { A } ] \left( \mathrm { mol } \mathrm { L } ^ { - 1 } \right) } & \text { Initial Rate } \left( \mathrm { mol } \mathrm { L } ^{- 1} \mathrm {~s} ^ { - 1 } \right) \\ \hline 0.35 & 0.038 \\ 0.70 & 0.038 \\ 1.05 & 0.038 \end{array}\]

A) zero order B) first order C) second order D) third order E) impossible to determine A) zero order B) first order C) second order D) third order E) impossible to determine

Determine the missing initial rate for the following $\frac{3}{2}$ order reaction given the following information: \[\begin{array} { l | l } { [ \mathrm { A } ] \left( \mathrm { mol } \mathrm { L } ^ { - 1 } \right) } & \text { Initial Rate } \left( \mathrm { mol } \mathrm { L } ^{- 1} \mathrm {~s} ^ { - 1 } \right) \\ \hline 0.0174 & 0.16 \\ 0.0361 & ? \\ 0.0996 & 2.2 \end{array}\]

A) 0.48 mol L-1 s-1 B) 0.38 mol L-1 s-1 C) 0.91 mol L-1 s-1 D) 1.3 mol L-1 s-1 E) 0.84 mol L-1 s-1 A) 0.48 mol L-1 s-1 B) 0.38 mol L-1 s-1 C) 0.91 mol L-1 s-1 D) 1.3 mol L-1 s-1 E) 0.84 mol L-1 s-1

For a reaction that follows the general rate law,Rate = k[A][B]2,what will happen to the rate of reaction if the concentration of B is increased by a factor of 3.00?

A) The rate will decrease by a factor of 1/9.00. B) The rate will decrease by a factor of 1/3.00. C) The rate will increase by a factor of 3.00. D) The rate will increase by a factor of 9.00. A) The rate will decrease by a factor of 1/9.00. B) The rate will decrease by a factor of 1/3.00. C) The rate will increase by a factor of 3.00. D) The rate will increase by a factor of 9.00.

Calculate the activation energy,Ea,for a reaction with a frequency factor,A,of 9.3 × 1010 s-1 and a rate constant of 1.06 × 103 s-1 at 273 K.

A) 42 kJ mol-1 B) 45 kJ mol-1 C) 36 kJ mol-1 D) 49 kJ mol-1 E) 58 kJ mol-1 A) 42 kJ mol-1 B) 45 kJ mol-1 C) 36 kJ mol-1 D) 49 kJ mol-1 E) 58 kJ mol-1

Nitrogen dioxide decomposes at 300 °C via a second-order process to produce nitrogen monoxide and oxygen according to the following chemical equation: 2NO2(g)→ 2NO(g)+ O2(g). A sample of NO2(g)is initially placed in a 2.50 L reaction vessel at 300 °C.If the half-life and the rate constant at 300 °C are 11 seconds and 0.54 L mol-1 s-1,respectively,how many moles of NO2 were in the original sample?

A) 0.17 mol B) 0.42 mol C) 5.9 mol D) 15 mol A) 0.17 mol B) 0.42 mol C) 5.9 mol D) 15 mol

Exam 13: Chemical Kinetics

Given the following proposed mechanism,predict the rate law for the overall reaction. $\quad$ A₂ + 2B → 2AB (overall reaction) $\quad$ $\underline{\text{Mechanism}}$ $\quad$ A₂ ⇌ 2A $\quad$ $\quad$ fast $\quad$ A + B → AB $\quad$ slow

(Multiple Choice)

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Question 61

If the concentration of a reactant is 6.25%,how many half-lives has it gone through?

(Multiple Choice)

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Question 62

Without performing complex calculations,determine the order of a reaction that has the following initial rates for the specified starting concentration: [] Initial Rate 0.35 0.038 0.70 0.038 1.05 0.038

(Multiple Choice)

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Question 63

The first-order reaction,SO₂Cl₂ → SO₂ + Cl₂,has a half-life of 8.75 hours at 593 K.How long will it take for the concentration of SO₂Cl₂ to fall to 16.5% of its initial value?

(Multiple Choice)

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Question 64

Derive an expression for a "1/3-life" for a first-order reaction.

(Multiple Choice)

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Question 65

A reaction with an activation energy of 84.6 kJ mol^-1 has a rate constant of 0.00681 L mol^-1 s^-1 at 325 K.What is the rate constant at 375 K?

(Multiple Choice)

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Question 66

The first-order decay of radon has a half-life of 3.823 days.How many grams of radon remain after 7.22 days if the sample initially weighs 250.0 grams?

(Multiple Choice)

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Question 67

A particular first-order reaction has a rate constant of 1.35 × $10 ^ { 2 }$ $s ^ { - 1 }$ at 25.0 °C.What is the magnitude of k at 75.0 °C if $E_{\mathrm{a}}=82.5 \mathrm{~kJ} \mathrm{~mol}^{-1} ?$

(Multiple Choice)

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Question 68

Determine the missing initial rate for the following $\frac{3}{2}$ order reaction given the following information: [] Initial Rate 0.0174 0.16 0.0361 ? 0.0996 2.2

(Multiple Choice)

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Question 69

The isomerization reaction,CH₃NC → CH₃CN,is first order and the rate constant is equal to 0.46 s^-1 at 600 K.What is the concentration of CH₃NC after 0.20 minutes if the initial concentration is 0.30 mol L^-1?

(Multiple Choice)

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Question 70

The first-order rearrangement of CH₃NC is measured to have a rate constant of 3.61 × 10^-15 s^-1 at 298 K and a rate constant of 8.66 × 10^-7 s^-1 at 425 K.Determine the activation energy for this reaction.

(Multiple Choice)

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Question 71

A particular first-order reaction has a rate constant of 1.35 × $10 ^ { 2 }$ $s ^ { - 1 }$ at 25.0 °C.What is the magnitude of k at $95^{\circ} \mathrm{C}$ if $E_{\mathrm{a}}=55.5 \mathrm{~kJ} \mathrm{~mol}-1 ?$

(Multiple Choice)

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Question 72

For a reaction that follows the general rate law,Rate = k[A][B]²,what will happen to the rate of reaction if the concentration of B is increased by a factor of 3.00?

(Multiple Choice)

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Question 73

The isomerization of methylisonitrile to acetonitrile $\mathrm { CH } _ { 3 }$ NC(g)? $\mathrm { CH } _ { 3 }$ CN(g) is first order in $\mathrm { CH } _ { 3 }$ NC.The half-life of the reaction is 8.42 × 10^-2 at 575 K.The rate constant when the initial [ $\mathrm { CH } _ { 3 }$ NC] is 0.030 mol L^-1 is ________ $s ^ { - 1 }$ .

(Multiple Choice)

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Question 74

Calculate the activation energy,E_a,for a reaction with a frequency factor,A,of 9.3 × 10¹⁰ s^-1 and a rate constant of 1.06 × 10³ s^-1 at 273 K.

(Multiple Choice)

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Question 75

A catalyst is needed in the hydrogenation of double bonds.In the first step,the reactants must come into contact with a metal surface.This step is known as

(Multiple Choice)

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Question 76

Determine the rate law and the value of k for the following reaction using the data provided: CO(g)+ Cl₂(g)→ COCl₂(g)[CO]_i(M) $\quad$ [Cl₂]_i $\quad$ (M)Initial Rate (M¹s^-1) $\quad$ $\quad$ $\quad$ $\quad$ $\quad$ $\quad$ $\quad$ $\quad$ $\quad$ 0.25 $\quad$ $\quad$ $\quad$ 0.40 $\quad$ $\quad$ 0.696 $\quad$ $\quad$ $\quad$ $\quad$ $\quad$ $\quad$ $\quad$ $\quad$ $\quad$ 0.25 $\quad$ $\quad$ $\quad$ 0.80 $\quad$ $\quad$ 1.97 $\quad$ $\quad$ $\quad$ $\quad$ $\quad$ $\quad$ $\quad$ $\quad$ $\quad$ 0.50 $\quad$ $\quad$ $\quad$ 0.80 $\quad$ $\quad$ 3.94

(Multiple Choice)

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Question 77

What is the difference between average reaction rate and instantaneous reaction rate?

(Essay)

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Question 78

Nitrogen dioxide decomposes at 300 °C via a second-order process to produce nitrogen monoxide and oxygen according to the following chemical equation: 2NO₂(g)→ 2NO(g)+ O₂(g). A sample of NO₂(g)is initially placed in a 2.50 L reaction vessel at 300 °C.If the half-life and the rate constant at 300 °C are 11 seconds and 0.54 L mol^-1 s^-1,respectively,how many moles of NO₂ were in the original sample?

(Multiple Choice)

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Question 79

Given the following balanced equation,determine the rate of reaction with respect to [SO₂]. 2SO₂(g)+ O₂(g)? 2SO₃(g)

(Multiple Choice)

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Question 80

Showing 61 - 80 of 156

Exam 13: Chemical Kinetics

Given the following proposed mechanism,predict the rate law for the overall reaction. \quad A2 + 2B → 2AB (overall reaction) \quadMechanism‾\underline{\text{Mechanism}}Mechanism​ \quad A2 ⇌ 2A \quad\quad fast \quad A + B → AB \quad slow

If the concentration of a reactant is 6.25%,how many half-lives has it gone through?

Without performing complex calculations,determine the order of a reaction that has the following initial rates for the specified starting concentration: [] Initial Rate 0.35 0.038 0.70 0.038 1.05 0.038

The first-order reaction,SO2Cl2 → SO2 + Cl2,has a half-life of 8.75 hours at 593 K.How long will it take for the concentration of SO2Cl2 to fall to 16.5% of its initial value?

Derive an expression for a "1/3-life" for a first-order reaction.

A reaction with an activation energy of 84.6 kJ mol-1 has a rate constant of 0.00681 L mol-1 s-1 at 325 K.What is the rate constant at 375 K?

The first-order decay of radon has a half-life of 3.823 days.How many grams of radon remain after 7.22 days if the sample initially weighs 250.0 grams?

A particular first-order reaction has a rate constant of 1.35 × 10210 ^ { 2 }102 s−1s ^ { - 1 }s−1 at 25.0 °C.What is the magnitude of k at 75.0 °C if Ea=82.5 kJ mol−1? E_{\mathrm{a}}=82.5 \mathrm{~kJ} \mathrm{~mol}^{-1} ? Ea​=82.5 kJ mol−1?

Determine the missing initial rate for the following 32\frac{3}{2}23​ order reaction given the following information: [] Initial Rate 0.0174 0.16 0.0361 ? 0.0996 2.2

The isomerization reaction,CH3NC → CH3CN,is first order and the rate constant is equal to 0.46 s-1 at 600 K.What is the concentration of CH3NC after 0.20 minutes if the initial concentration is 0.30 mol L-1?

The first-order rearrangement of CH3NC is measured to have a rate constant of 3.61 × 10-15 s-1 at 298 K and a rate constant of 8.66 × 10-7 s-1 at 425 K.Determine the activation energy for this reaction.

A particular first-order reaction has a rate constant of 1.35 × 10210 ^ { 2 }102 s−1s ^ { - 1 }s−1 at 25.0 °C.What is the magnitude of k at 95∘C 95^{\circ} \mathrm{C} 95∘C if Ea=55.5 kJ mol−1? E_{\mathrm{a}}=55.5 \mathrm{~kJ} \mathrm{~mol}-1 ? Ea​=55.5 kJ mol−1?

For a reaction that follows the general rate law,Rate = k[A][B]2,what will happen to the rate of reaction if the concentration of B is increased by a factor of 3.00?

Calculate the activation energy,Ea,for a reaction with a frequency factor,A,of 9.3 × 1010 s-1 and a rate constant of 1.06 × 103 s-1 at 273 K.

A catalyst is needed in the hydrogenation of double bonds.In the first step,the reactants must come into contact with a metal surface.This step is known as

What is the difference between average reaction rate and instantaneous reaction rate?

Given the following balanced equation,determine the rate of reaction with respect to [SO2]. 2SO2(g)+ O2(g)? 2SO3(g)

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Given the following proposed mechanism,predict the rate law for the overall reaction. $\quad$ A₂ + 2B → 2AB (overall reaction) $\quad$ $\underline{\text{Mechanism}}$ $\quad$ A₂ ⇌ 2A $\quad$ $\quad$ fast $\quad$ A + B → AB $\quad$ slow

The first-order reaction,SO₂Cl₂ → SO₂ + Cl₂,has a half-life of 8.75 hours at 593 K.How long will it take for the concentration of SO₂Cl₂ to fall to 16.5% of its initial value?

A reaction with an activation energy of 84.6 kJ mol^-1 has a rate constant of 0.00681 L mol^-1 s^-1 at 325 K.What is the rate constant at 375 K?

A particular first-order reaction has a rate constant of 1.35 × $10 ^ { 2 }$ $s ^ { - 1 }$ at 25.0 °C.What is the magnitude of k at 75.0 °C if $E_{\mathrm{a}}=82.5 \mathrm{~kJ} \mathrm{~mol}^{-1} ?$

Determine the missing initial rate for the following $\frac{3}{2}$ order reaction given the following information: [] Initial Rate 0.0174 0.16 0.0361 ? 0.0996 2.2

The isomerization reaction,CH₃NC → CH₃CN,is first order and the rate constant is equal to 0.46 s^-1 at 600 K.What is the concentration of CH₃NC after 0.20 minutes if the initial concentration is 0.30 mol L^-1?

The first-order rearrangement of CH₃NC is measured to have a rate constant of 3.61 × 10^-15 s^-1 at 298 K and a rate constant of 8.66 × 10^-7 s^-1 at 425 K.Determine the activation energy for this reaction.

A particular first-order reaction has a rate constant of 1.35 × $10 ^ { 2 }$ $s ^ { - 1 }$ at 25.0 °C.What is the magnitude of k at $95^{\circ} \mathrm{C}$ if $E_{\mathrm{a}}=55.5 \mathrm{~kJ} \mathrm{~mol}-1 ?$

For a reaction that follows the general rate law,Rate = k[A][B]²,what will happen to the rate of reaction if the concentration of B is increased by a factor of 3.00?

Calculate the activation energy,E_a,for a reaction with a frequency factor,A,of 9.3 × 10¹⁰ s^-1 and a rate constant of 1.06 × 10³ s^-1 at 273 K.

Given the following balanced equation,determine the rate of reaction with respect to [SO₂]. 2SO₂(g)+ O₂(g)? 2SO₃(g)