Nitric oxide gas (NO) reacts with chlorine gas according to the chemical equation given below.NO + 1/2Cl2 $\rarr$ NOCl The following initial rates of reaction have been measured for the given reagent concentrations. $\begin{array}{lccc} Expt.\# & Rate (M/hr) & NO (M) & \mathrm{Cl}_{2}(\mathrm{M}) \\\hline 1 & 1.19 & 0.50 & 0.50 \\ 2 & 4.79 & 1.00 & 0.50 \\ 3 & 9.59 & 1.00 & 1.00 \\ \end{array}$ Which of the following is the rate law (rate equation) for this reaction

A) rate = k[NO] B) rate = k[NO][Cl2]1/2 C) rate = k[NO][Cl2] D) rate = k[NO]2[Cl2] E) rate = k[NO]2[Cl2]2 A) rate = k[NO] B) rate = k[NO][Cl2]1/2 C) rate = k[NO][Cl2] D) rate = k[NO]2[Cl2] E) rate = k[NO]2[Cl2]2

The data below were determined for the reaction shown below.S2O82- + 3I - (aq) $\rarr$2SO42- + I3- $\begin{array}{lccc} \text { Expt. \# } & \left[\mathrm{S}_{2-} \mathrm{O}_{8}{ }^{2}\right] & {[I-]} & \text { Initial Rate } \\ \hline 1 & 0.038 & 0.060 & 1.4 \times 10^{-5} \mathrm{M} / \mathrm{s} \\ 2 & 0.076 & 0.060 & 2.8 \times 10^{-5} \mathrm{M} / \mathrm{s} \\ 3 & 0.076 & 0.030 & 1.4 \times 10^{-5} \mathrm{M} / \mathrm{s} \end{array}$ The rate law for this reaction must be:

A) rate = k[S2O82- ][I -]3 B) rate = k[S2O82-] C) rate = k[S2O82-]2[I -]2 D) rate = k[I -] E) rate = k[S2O82-][I -] A) rate = k[S2O82- ][I -]3 B) rate = k[S2O82-] C) rate = k[S2O82-]2[I -]2 D) rate = k[I -] E) rate = k[S2O82-][I -]

A reaction was experimentally determined to follow the rate law, Rate = k[A]2 where k = 0.456 s-1M-1. Starting with [A]o = 0.500 M, how many seconds will it take for [A]t = 0.250 M

A) 2.85 x 10-2 s B) 1.14 x 10-1 s C) 1.52 s D) 4.39 s E) 5.48x10-1 s A) 2.85 x 10-2 s B) 1.14 x 10-1 s C) 1.52 s D) 4.39 s E) 5.48x10-1 s

At a certain temperature, the data below were collected for the reaction below.2ICl + H2 $\rarr$I2 + 2HCl.Determine the rate constant for the reaction.

A) 1.5 * 10-2 L/mol·s B) 2.0 * 10-1 L/mol·s C) 1.5 * 10-1 L/mol·s D) 2.5 * 10-2 L/mol·s E) None of the above A) 1.5 * 10-2 L/mol·s B) 2.0 * 10-1 L/mol·s C) 1.5 * 10-1 L/mol·s D) 2.5 * 10-2 L/mol·s E) None of the above

The following mechanism has been suggested for the reaction: $\begin{array}{ll} \mathrm{H}_{2} \mathrm{O}_{2}+2 \mathrm{H}^{+}+2 \mathrm{I}^{-} \rightarrow \mathrm{I}_{2}+2 \mathrm{H}_{2} \mathrm{O} \\ \mathrm{H}_{2} \mathrm{O}_{2}+\mathrm{I}^{-} \rightarrow \mathrm{HOI}+\mathrm{OH}^{-} & \mathrm{Slow}\\ \mathrm{OH}^{-}+\mathrm{H}^{+} \rightarrow \mathrm{H}_{2} \mathrm{O} & \mathrm{Fast}\\ \mathrm{HOI}+\mathrm{H}^{+}+\mathrm{I}^{-} \rightarrow \mathrm{I}_{2}+\mathrm{H}_{2} \mathrm{O}& \mathrm{Fast} \end{array}$ Identify the molecularity of the rate determining step.

A) unimolecular B) bimolecular C) termolecular D) unimolecular and bimolecular E) bimolecular and termolecular A) unimolecular B) bimolecular C) termolecular D) unimolecular and bimolecular E) bimolecular and termolecular

Aspirin, C9H8O4, slowly decomposes at room temperature by reacting with water in the atmosphere to produce acetic acid, HC2H3O2, and 2-hydroxybenzoic acid, C7H6O3 (this is why old bottles of aspirin often smell like vinegar): C9H8O4 + H2O $\rarr$ HC2H3O2 + C7H6O3 Concentration and rate data for this reaction are given below. $\begin{array}{ccc} \mathbf{\left[\mathrm{C}_{9} \mathrm{H}_{5} \mathrm{O}_{4}\right](\mathrm{M})} & \mathbf{\left[\mathrm{H}_{2} \mathrm{O}\right] (M)} & \mathbf{Rate (M/s)} \\\hline 0.0100 & 0.0200 & 2.4 \times 10^{-13} \\ 0.0100 & 0.0800 & 9.6 \times 10^{-13} \\ 0.0200 & 0.0200 & 4.8 \times 10^{-13} \\ \end{array}$ Write the rate law for this reaction and calculate k (be sure to include the correct units).

A) rate = k[C9H8O4][H2O]2, and the rate constant is 1.2 *10-9 M-2s-1 or 1.2 * 10-9 1/(M2 s) B) rate = k[C9H8O4], and the rate constant is 1.2 * 10-9 -1 or 1.2 * 10-9 1/ s C) rate = k[C9H8O4]2[H2O], and the rate constant is 1.2 * 10-9 M-2s-1 or 1.2 * 10-9 1/(M2 s) D) rate = k[C9H8O4][H2O], and the rate constant is 1.2 *10-9 M-1s-1 or 1.2 * 10-9 1/(M s) E) None of the above A) rate = k[C9H8O4][H2O]2, and the rate constant is 1.2 *10-9 M-2s-1 or 1.2 * 10-9 1/(M2 s) B) rate = k[C9H8O4], and the rate constant is 1.2 * 10-9 -1 or 1.2 * 10-9 1/ s C) rate = k[C9H8O4]2[H2O], and the rate constant is 1.2 * 10-9 M-2s-1 or 1.2 * 10-9 1/(M2 s) D) rate = k[C9H8O4][H2O], and the rate constant is 1.2 *10-9 M-1s-1 or 1.2 * 10-9 1/(M s) E) None of the above

Exam 13: Chemical Kinetics

The first-order decomposition of phosphene to phosphorus and hydrogen, shown below, 4PH₃(g) $\rarr$ P₄(g) + 6H₂(g) Has a half-life of 35.0 s at 680^$\circ$C. Starting with 520 mmHg of pure phosphene in an 8.00-L flask at 680^$\circ$C, how long will it take for the total pressure in the flask to rise to 1.000 atm

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Question 61

For a second order reaction, the half-life is equal to

(Multiple Choice)

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Question 62

In general, to calculate the activation energy for an elementary step given the rate constants at two different temperatures, which equation should be used

(Multiple Choice)

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Question 63

In general, to calculate the rate constant for a second order reaction with respect to A, given an initial and final concentration as well as the time required for this change, which equation should be used

(Multiple Choice)

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Question 64

Nitric oxide gas (NO) reacts with chlorine gas according to the chemical equation given below.NO + 1/2Cl₂ $\rarr$ NOCl The following initial rates of reaction have been measured for the given reagent concentrations. Expt.\# Rate(M/hr) NO(M) () 1 1.19 0.50 0.50 2 4.79 1.00 0.50 3 9.59 1.00 1.00 Which of the following is the rate law (rate equation) for this reaction

(Multiple Choice)

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Question 65

The data below were determined for the reaction shown below.S₂O₈^2- + 3I ^- (aq) $\rarr$ 2SO₄^2- + I₃^- Expt. \# [I-] Initial Rate 1 0.038 0.060 1.4\times1/ 2 0.076 0.060 2.8\times1/ 3 0.076 0.030 1.4\times1/ The rate law for this reaction must be:

(Multiple Choice)

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Question 66

With respect to the figure below, which choice correctly identifies all the numbered positions $With respect to the figure below, which choice correctly identifies all the numbered positions \begin{array}{llll} ~~~~~~~~1.&~2.&~3.&~4.\\ \text { A. catalyst } & \text { intermediate } & \text { activated complex } & \text { product } \\ \text { B. reactants } & \text { activated complex } & \text { intermediate } & \text { product } \\ \text { C. reactants } & \text { activated complex } & \text { catalyst } & \text { product } \\ \text { D. reactants } & \text { intermediate } & \text { activated complex } & \text { product } \\ \text { E. ~~reactants } & \text { intermediate } & \text { activated complex } & \text { catalyst } \end{array}$ \nobreakspace\nobreakspace\nobreakspace\nobreakspace\nobreakspace\nobreakspace\nobreakspace\nobreakspace1. \nobreakspace2. \nobreakspace3. \nobreakspace4. A. \nobreakspace\nobreakspacecatalyst intermediate activated complex product B. \nobreakspace\nobreakspacereactants activated complex intermediate product C. \nobreakspace\nobreakspacereactants activated complex catalyst product D. \nobreakspace\nobreakspacereactants intermediate activated complex product E. \nobreakspace\nobreakspacereactants intermediate activated complex catalyst

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Question 67

The reaction 2A $\rarr$ products is second order with respect toA. If the concentration of A drops from 1.05 M to 0.815 M in a time of 15.0 min, what is the rate constant for this reaction (the same time units may be used)

(Multiple Choice)

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Question 68

The rate determining step in the following mechanism is bimolecular. \rightarrow+ slow +\rightarrow+ fast

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Question 69

Which of the following elementary steps is termolecular

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Question 70

For the chemical reaction system described by the diagram below, which statement is true

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Question 71

A reaction was experimentally determined to follow the rate law, Rate = k[A]² where k = 0.456 s^-1M^-1. Starting with [A]_o = 0.500 M, how many seconds will it take for [A]_t = 0.250 M

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Question 72

At a certain temperature, the data below were collected for the reaction below.2ICl + H₂ $\rarr$ I₂ + 2HCl.Determine the rate constant for the reaction. $At a certain temperature, the data below were collected for the reaction below.2ICl + H<sub>2</sub> \rarr I<sub>2</sub> + 2HCl.Determine the rate constant for the reaction.$

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Question 73

The isomerization of cyclopropane to form propene is a first-order reaction. At 760 K, 85% of a sample of cyclopropane changes to propene in 79.0 min. Determine the rate constant for this reaction at 760 K.

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Question 74

A nuclear stress test utilizes a gamma-emitting radioisotope such as thallium-201 to follow the flow of blood through the heart - first at rest, and then under stress. The first-order rate constant for the decay of thallium-201 is 9.5 x 10^-3 hr^-1. Calculate how long it takes for the amount of thallium-201 to fall to 5.0% of its original value.

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Question 75

The following mechanism has been suggested for the reaction: +2+2\rightarrow+2 +\rightarrow+ +\rightarrow ++\rightarrow+ Identify the molecularity of the rate determining step.

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Question 76

The isomerization of cyclopropane to form propene is a first-order reaction. At 760 K, 15% of a sample of cyclopropane changes to propene in 6.8 min. What is the half-life of cyclopropane at 760 K

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Question 77

For the reaction X + Y $\rarr$ Z, the reaction rate is found to depend only upon the concentration of X. A plot of 1/X verses time gives a straight line. $For the reaction X + Y \rarr Z, the reaction rate is found to depend only upon the concentration of X. A plot of 1/X verses time gives a straight line. What is the rate law for this reaction$ What is the rate law for this reaction

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Question 78

Aspirin, C₉H₈O₄, slowly decomposes at room temperature by reacting with water in the atmosphere to produce acetic acid, HC₂H₃O₂, and 2-hydroxybenzoic acid, C₇H₆O₃ (this is why old bottles of aspirin often smell like vinegar): C₉H₈O₄ + H₂O $\rarr$ HC₂H₃O₂ + C₇H₆O₃ Concentration and rate data for this reaction are given below. 0.0100 0.0200 2.4\times1 0.0100 0.0800 9.6\times1 0.0200 0.0200 4.8\times1 Write the rate law for this reaction and calculate k (be sure to include the correct units).

(Multiple Choice)

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Question 79

For the reaction A + 3B $\rarr$ 2C, the rate of disappearance of B given by ( $\Delta$ [B]/ $\Delta$ t) may also be expressed as

(Multiple Choice)

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Question 80

Showing 61 - 80 of 131

For a second order reaction, the half-life is equal to

In general, to calculate the activation energy for an elementary step given the rate constants at two different temperatures, which equation should be used

In general, to calculate the rate constant for a second order reaction with respect to A, given an initial and final concentration as well as the time required for this change, which equation should be used

The data below were determined for the reaction shown below.S₂O₈^2- + 3I ^- (aq) $\rarr$ 2SO₄^2- + I₃^- Expt. \# [I-] Initial Rate 1 0.038 0.060 1.4\times1/ 2 0.076 0.060 2.8\times1/ 3 0.076 0.030 1.4\times1/ The rate law for this reaction must be:

The reaction 2A $\rarr$ products is second order with respect toA. If the concentration of A drops from 1.05 M to 0.815 M in a time of 15.0 min, what is the rate constant for this reaction (the same time units may be used)

The rate determining step in the following mechanism is bimolecular. \rightarrow+ slow +\rightarrow+ fast

Which of the following elementary steps is termolecular

For the chemical reaction system described by the diagram below, which statement is true

A reaction was experimentally determined to follow the rate law, Rate = k[A]² where k = 0.456 s^-1M^-1. Starting with [A]_o = 0.500 M, how many seconds will it take for [A]_t = 0.250 M

The isomerization of cyclopropane to form propene is a first-order reaction. At 760 K, 85% of a sample of cyclopropane changes to propene in 79.0 min. Determine the rate constant for this reaction at 760 K.

The following mechanism has been suggested for the reaction: +2+2\rightarrow+2 +\rightarrow+ +\rightarrow ++\rightarrow+ Identify the molecularity of the rate determining step.

The isomerization of cyclopropane to form propene is a first-order reaction. At 760 K, 15% of a sample of cyclopropane changes to propene in 6.8 min. What is the half-life of cyclopropane at 760 K

For the reaction A + 3B $\rarr$ 2C, the rate of disappearance of B given by ( $\Delta$ [B]/ $\Delta$ t) may also be expressed as

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Exam 13: Chemical Kinetics

For a second order reaction, the half-life is equal to

In general, to calculate the activation energy for an elementary step given the rate constants at two different temperatures, which equation should be used

In general, to calculate the rate constant for a second order reaction with respect to A, given an initial and final concentration as well as the time required for this change, which equation should be used

The data below were determined for the reaction shown below.S2O82- + 3I - (aq) →\rarr→ 2SO42- + I3- Expt. \# [I-] Initial Rate 1 0.038 0.060 1.4\times1/ 2 0.076 0.060 2.8\times1/ 3 0.076 0.030 1.4\times1/ The rate law for this reaction must be:

The reaction 2A →\rarr→ products is second order with respect toA. If the concentration of A drops from 1.05 M to 0.815 M in a time of 15.0 min, what is the rate constant for this reaction (the same time units may be used)

The rate determining step in the following mechanism is bimolecular. \rightarrow+ slow +\rightarrow+ fast

Which of the following elementary steps is termolecular

For the chemical reaction system described by the diagram below, which statement is true

A reaction was experimentally determined to follow the rate law, Rate = k[A]2 where k = 0.456 s-1M-1. Starting with [A]o = 0.500 M, how many seconds will it take for [A]t = 0.250 M

At a certain temperature, the data below were collected for the reaction below.2ICl + H2 →\rarr→ I2 + 2HCl.Determine the rate constant for the reaction.

The isomerization of cyclopropane to form propene is a first-order reaction. At 760 K, 85% of a sample of cyclopropane changes to propene in 79.0 min. Determine the rate constant for this reaction at 760 K.

The following mechanism has been suggested for the reaction: +2+2\rightarrow+2 +\rightarrow+ +\rightarrow ++\rightarrow+ Identify the molecularity of the rate determining step.

The isomerization of cyclopropane to form propene is a first-order reaction. At 760 K, 15% of a sample of cyclopropane changes to propene in 6.8 min. What is the half-life of cyclopropane at 760 K

For the reaction X + Y →\rarr→ Z, the reaction rate is found to depend only upon the concentration of X. A plot of 1/X verses time gives a straight line. What is the rate law for this reaction

For the reaction A + 3B →\rarr→ 2C, the rate of disappearance of B given by ( Δ\DeltaΔ [B]/ Δ\DeltaΔ t) may also be expressed as

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Atoms Molecules and Ions

Mass Relationships in Chemical Reactions

Reactions in Aqueous Solutions

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Thermochemistry

Quantum Theory and the Electronic Structure of Atoms

Periodic Relationships Among the Elements

Chemical Bonding I: Basic Concepts

Chemical Bonding II: Molecular Geometry and Hybridization of Atomic

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Physical Properties of Solutions

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Acid-Base Equilibria and Solubility Equilibria

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The data below were determined for the reaction shown below.S₂O₈^2- + 3I ^- (aq) $\rarr$ 2SO₄^2- + I₃^- Expt. \# [I-] Initial Rate 1 0.038 0.060 1.4\times1/ 2 0.076 0.060 2.8\times1/ 3 0.076 0.030 1.4\times1/ The rate law for this reaction must be:

The reaction 2A $\rarr$ products is second order with respect toA. If the concentration of A drops from 1.05 M to 0.815 M in a time of 15.0 min, what is the rate constant for this reaction (the same time units may be used)

A reaction was experimentally determined to follow the rate law, Rate = k[A]² where k = 0.456 s^-1M^-1. Starting with [A]_o = 0.500 M, how many seconds will it take for [A]_t = 0.250 M

For the reaction A + 3B $\rarr$ 2C, the rate of disappearance of B given by ( $\Delta$ [B]/ $\Delta$ t) may also be expressed as