The data below were determined for the reaction shown below. S2O82- + 3I - (aq) $\rarr$0 2SO42- + I3- 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 -]

The following reaction in aqueous solution was found to be first order in [OH-], first order in [C2H5Br], and inverse first order in Br-. C2H5Br + OH- $\rarr$C2H5OH + Br- Which one of the following mechanisms is consistent with the observed reaction order?

A) C2H5Br C2H5+ + Br- fast C2H5+ + OH- C2H5OH slow B) C2H5Br +H2O C2H5OH + H+ + Br- slow H+ + OH- H2O fast C) C2H5Br C2H5+ + Br- slow C2H5+ + OH- C2H5OH fast D) C2H5Br C2H5+ + Br- slow OH- + Br- HOBr fast HOBr + C2H5+ C2H5OH + Br- fast A) C2H5Br C2H5+ + Br- fast C2H5+ + OH- C2H5OH slow B) C2H5Br +H2O C2H5OH + H+ + Br- slow H+ + OH- H2O fast C) C2H5Br C2H5+ + Br- slow C2H5+ + OH- C2H5OH fast D) C2H5Br C2H5+ + Br- slow OH- + Br- HOBr fast HOBr + C2H5+ C2H5OH + Br- fast

The first-order decomposition of SO2Cl2 to sulfur dioxide gas and chlorine gas at 320°C has a half-life of 8.75 hr.If 600.mmHg of pure SO2Cl2 is placed in a 5.00-L flask at 320°C, how long does it take for the total pressure in the flask to rise to 1.000 atm?

A) 6.45 hr B) 11.1 hr C) 3.91 hr D) 20.3 hr E) 6.91 hr A) 6.45 hr B) 11.1 hr C) 3.91 hr D) 20.3 hr E) 6.91 hr

The reaction 2NO2(g) $\rarr$2NO(g)+ O2(g)is suspected to be second order in NO2.Which of the following kinetic plots would be the most useful to confirm whether or not the reaction is second order?

A) a plot of [NO2]-1 vs.t B) a plot of ln [NO2] vs.t C) a plot of [NO2] vs.t D) a plot of ln [NO2]-1 vs.t E) a plot of [NO2]2 vs.t A) a plot of [NO2]-1 vs.t B) a plot of ln [NO2] vs.t C) a plot of [NO2] vs.t D) a plot of ln [NO2]-1 vs.t E) a plot of [NO2]2 vs.t

For the following reaction, $\Delta$P(C6H14)/$\Delta$t was found to be -6.2 × 10-3 atm/s. C6H14(g)$\rarr$C6H6(g)+ 4H2(g) Determine $\Delta$P(H2)/$\Delta$t for this reaction at the same time.

A) 6.2 × 10-3 atm/s B) 1.6 × 10-3 atm/s C) 2.5 × 10-2 atm/s D) -1.6 × 10-3 atm/s E) -2.5 × 10-2 atm/s A) 6.2 × 10-3 atm/s B) 1.6 × 10-3 atm/s C) 2.5 × 10-2 atm/s D) -1.6 × 10-3 atm/s E) -2.5 × 10-2 atm/s

The activation energy for the following first-order reaction is 102 kJ/mol. N2O5(g)$\rarr$2NO2(g)+ 1/2O2(g) The value of the rate constant (k)is 1.35 × 10-4 s-1 at 35°C.What is the value of k at 0°C?

A) 8.2 × 10-7 s-1 B) 1.9 × 10-5 s-1 C) 4.2 × 10-5 s-1 D) 2.2 × 10-2 s-1 E) none of these A) 8.2 × 10-7 s-1 B) 1.9 × 10-5 s-1 C) 4.2 × 10-5 s-1 D) 2.2 × 10-2 s-1 E) none of these

Exam 13: Chemical Kinetics

The data below were determined for the reaction shown below. S₂O₈^2- + 3I ^- (aq) $\rarr$ 0 2SO₄^2- + I₃^- $The data below were determined for the reaction shown below. S2O82- + 3I - (aq) \rarr 0 2SO42- + I3- The rate law for this reaction must be:$ The rate law for this reaction must be:

(Multiple Choice)

4.8/5

(76)

Question 101

The Arrhenius equation is k = Ae^-Ea/RT.The slope of a plot of ln k vs.1/T is equal to

(Multiple Choice)

4.8/5

(87)

Question 102

The isomerization of cyclopropane to propene follows first-order kinetics. At 700 K, the rate constant for this reaction is 6.2 × 10^-4min^-1.How many minutes are required for 10.0% of a sample of cyclopropane to isomerize to propene?

(Multiple Choice)

4.7/5

(86)

Question 103

The following reaction in aqueous solution was found to be first order in [OH^-], first order in [C₂H₅Br], and inverse first order in Br^-. C₂H₅Br + OH^- $\rarr$ C₂H₅OH + Br^- Which one of the following mechanisms is consistent with the observed reaction order?

(Multiple Choice)

4.7/5

(78)

Question 104

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)

4.9/5

(80)

Question 105

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

(Multiple Choice)

4.8/5

(83)

Question 106

Use the table of data shown below to calculate the average rate of the reaction A $\rarr$ B between 10 s and 20 s. $Use the table of data shown below to calculate the average rate of the reaction A \rarr B between 10 s and 20 s.$

(Short Answer)

4.8/5

(88)

Question 107

The first-order decomposition of SO₂Cl₂ to sulfur dioxide gas and chlorine gas at 320°C has a half-life of 8.75 hr.If 600.mmHg of pure SO₂Cl₂ is placed in a 5.00-L flask at 320°C, how long does it take for the total pressure in the flask to rise to 1.000 atm?

(Multiple Choice)

4.8/5

(81)

Question 108

Which of the following elementary steps is termolecular?

(Multiple Choice)

4.7/5

(82)

Question 109

Which one of the following changes would alter the rate constant (k)for the reaction 2A + B $\rarr$ products?

(Multiple Choice)

4.8/5

(75)

Question 110

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

(Multiple Choice)

4.7/5

(66)

Question 111

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°C.Starting with 520 mmHg of pure phosphene in an 8.00-L flask at 680°C, how long will it take for the total pressure in the flask to rise to 1.000 atm?

(Multiple Choice)

4.8/5

(91)

Question 112

The reaction 2NO₂(g) $\rarr$ 2NO(g)+ O₂(g)is suspected to be second order in NO₂.Which of the following kinetic plots would be the most useful to confirm whether or not the reaction is second order?

(Multiple Choice)

4.7/5

(82)

Question 113

The reaction 2A $\rarr$ products is second order with respect to A.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)?

(Essay)

4.7/5

(76)

Question 114

For the following reaction, $\Delta$ P(C₆H₁₄)/ $\Delta$ t was found to be -6.2 × 10^-3 atm/s. C₆H₁₄(g) $\rarr$ C₆H₆(g)+ 4H₂(g) Determine $\Delta$ P(H₂)/ $\Delta$ t for this reaction at the same time.

(Multiple Choice)

5.0/5

(76)

Question 115

What is the rate law that corresponds to the data shown for the reaction 2A + B $\rarr$ C? $What is the rate law that corresponds to the data shown for the reaction 2A + B \rarr C?$

(Short Answer)

4.9/5

(81)

Question 116

The activation energy for the following first-order reaction is 102 kJ/mol. N₂O₅(g) $\rarr$ 2NO₂(g)+ ¹/₂O₂(g) The value of the rate constant (k)is 1.35 × 10^-4 s^-1 at 35°C.What is the value of k at 0°C?

(Multiple Choice)

4.8/5

(88)

Question 117

At 25°C the rate constant for the first-order decomposition of a pesticide solution is 6.40 × 10^-3 min^-1.If the starting concentration of pesticide is 0.0314 M, what concentration will remain after 62.0 min at 25°C?

(Multiple Choice)

4.7/5

(77)

Question 118

A city's water supply is contaminated with a toxin at a concentration of 0.63 mg/L.Fortunately, this toxin decomposes to a safe mixture of products by first-order kinetics with a rate constant of 0.27 day^-1.How long will it take for half of the toxin to decompose?

(Multiple Choice)

4.9/5

(86)

Question 119

The rate law predicted by the following two-step mechanism is rate = k[A][B].

(True/False)

4.7/5

(89)

Question 120

Showing 101 - 120 of 130

Exam 13: Chemical Kinetics

The data below were determined for the reaction shown below. S2O82- + 3I - (aq) →\rarr→ 0 2SO42- + I3- The rate law for this reaction must be:

The Arrhenius equation is k = Ae-Ea/RT.The slope of a plot of ln k vs.1/T is equal to

The isomerization of cyclopropane to propene follows first-order kinetics. At 700 K, the rate constant for this reaction is 6.2 × 10-4 min-1.How many minutes are required for 10.0% of a sample of cyclopropane to isomerize to propene?

The following reaction in aqueous solution was found to be first order in [OH-], first order in [C2H5Br], and inverse first order in Br-. C2H5Br + OH- →\rarr→ C2H5OH + Br- Which one of the following mechanisms is consistent with the observed reaction order?

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?

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

Use the table of data shown below to calculate the average rate of the reaction A →\rarr→ B between 10 s and 20 s.

The first-order decomposition of SO2Cl2 to sulfur dioxide gas and chlorine gas at 320°C has a half-life of 8.75 hr.If 600.mmHg of pure SO2Cl2 is placed in a 5.00-L flask at 320°C, how long does it take for the total pressure in the flask to rise to 1.000 atm?

Which of the following elementary steps is termolecular?

Which one of the following changes would alter the rate constant (k)for the reaction 2A + B →\rarr→ products?

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

The reaction 2NO2(g) →\rarr→ 2NO(g)+ O2(g)is suspected to be second order in NO2.Which of the following kinetic plots would be the most useful to confirm whether or not the reaction is second order?

The reaction 2A →\rarr→ products is second order with respect to A.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)?

For the following reaction, Δ\DeltaΔ P(C6H14)/ Δ\DeltaΔ t was found to be -6.2 × 10-3 atm/s. C6H14(g) →\rarr→ C6H6(g)+ 4H2(g) Determine Δ\DeltaΔ P(H2)/ Δ\DeltaΔ t for this reaction at the same time.

What is the rate law that corresponds to the data shown for the reaction 2A + B →\rarr→ C?

The activation energy for the following first-order reaction is 102 kJ/mol. N2O5(g) →\rarr→ 2NO2(g)+ 1/2O2(g) The value of the rate constant (k)is 1.35 × 10-4 s-1 at 35°C.What is the value of k at 0°C?

At 25°C the rate constant for the first-order decomposition of a pesticide solution is 6.40 × 10-3 min-1.If the starting concentration of pesticide is 0.0314 M, what concentration will remain after 62.0 min at 25°C?

A city's water supply is contaminated with a toxin at a concentration of 0.63 mg/L.Fortunately, this toxin decomposes to a safe mixture of products by first-order kinetics with a rate constant of 0.27 day-1.How long will it take for half of the toxin to decompose?

The rate law predicted by the following two-step mechanism is rate = k[A][B].

Chemistry: the Study of Change

Atoms, Molecules, and Ions

Mass Relationships in Chemical Reactions

Reactions in Aqueous Solutions

Gases

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 Orbitals

Intermolecular Forces and Liquids and Solids

Physical Properties of Solutions

Chemical Equilibrium

Acids and Bases

Acid-Base Equilibria and Solubility Equilibria

Entropy Free Energy and Equilibrium

Electrochemistry

Nuclear Chemistry

Chemistry in the Atmosphere

Metallurgy and the Chemistry of Metals

Nonmetallic Elements and Their Compounds

Transition Metal Chemistry and Coordination Compounds

Organic Chemistry

Synthetic and Natural Organic Polymers

Filters

The Arrhenius equation is k = Ae^-Ea/RT.The slope of a plot of ln k vs.1/T is equal to

The isomerization of cyclopropane to propene follows first-order kinetics. At 700 K, the rate constant for this reaction is 6.2 × 10^-4min^-1.How many minutes are required for 10.0% of a sample of cyclopropane to isomerize to propene?

The following reaction in aqueous solution was found to be first order in [OH^-], first order in [C₂H₅Br], and inverse first order in Br^-. C₂H₅Br + OH^- $\rarr$ C₂H₅OH + Br^- Which one of the following mechanisms is consistent with the observed reaction order?

Use the table of data shown below to calculate the average rate of the reaction A $\rarr$ B between 10 s and 20 s. $Use the table of data shown below to calculate the average rate of the reaction A \rarr B between 10 s and 20 s.$

The first-order decomposition of SO₂Cl₂ to sulfur dioxide gas and chlorine gas at 320°C has a half-life of 8.75 hr.If 600.mmHg of pure SO₂Cl₂ is placed in a 5.00-L flask at 320°C, how long does it take for the total pressure in the flask to rise to 1.000 atm?

Which one of the following changes would alter the rate constant (k)for the reaction 2A + B $\rarr$ products?

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

The reaction 2NO₂(g) $\rarr$ 2NO(g)+ O₂(g)is suspected to be second order in NO₂.Which of the following kinetic plots would be the most useful to confirm whether or not the reaction is second order?

The reaction 2A $\rarr$ products is second order with respect to A.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)?

For the following reaction, $\Delta$ P(C₆H₁₄)/ $\Delta$ t was found to be -6.2 × 10^-3 atm/s. C₆H₁₄(g) $\rarr$ C₆H₆(g)+ 4H₂(g) Determine $\Delta$ P(H₂)/ $\Delta$ t for this reaction at the same time.

What is the rate law that corresponds to the data shown for the reaction 2A + B $\rarr$ C? $What is the rate law that corresponds to the data shown for the reaction 2A + B \rarr C?$

The activation energy for the following first-order reaction is 102 kJ/mol. N₂O₅(g) $\rarr$ 2NO₂(g)+ ¹/₂O₂(g) The value of the rate constant (k)is 1.35 × 10^-4 s^-1 at 35°C.What is the value of k at 0°C?

At 25°C the rate constant for the first-order decomposition of a pesticide solution is 6.40 × 10^-3 min^-1.If the starting concentration of pesticide is 0.0314 M, what concentration will remain after 62.0 min at 25°C?

A city's water supply is contaminated with a toxin at a concentration of 0.63 mg/L.Fortunately, this toxin decomposes to a safe mixture of products by first-order kinetics with a rate constant of 0.27 day^-1.How long will it take for half of the toxin to decompose?