Ammonium cyanate (NH4CNO) reacts to form urea (NH2CONH2). At 65°C the rate constant, k, is 3.60 L mol-1s-1. What is the rate law for this reaction?

A) Rate = 3.60 L mol-1s-1[NH4CNO] B) Rate = 3.60 L mol-1s-1[NH4CNO]2 C) Rate = 0.28 mol L-1 s-1[NH4CNO] D) Rate = 0.28 mol L-1 s-1[NH4CNO]2 E) Rate = 3.60 L mol-1s-1[NH2CONH2]-1 A) Rate = 3.60 L mol-1s-1[NH4CNO] B) Rate = 3.60 L mol-1s-1[NH4CNO]2 C) Rate = 0.28 mol L-1 s-1[NH4CNO] D) Rate = 0.28 mol L-1 s-1[NH4CNO]2 E) Rate = 3.60 L mol-1s-1[NH2CONH2]-1

The decomposition of dinitrogen pentaoxide has an activation energy of 102 kJ/mol and F1F1F1S1F1F1F10H°rxn = + 55 kJ/mol. What is the activation energy for the reverse reaction?

A) 27 kJ/mol B) 47 kJ/mol C) 55 kJ/mol D) 102 kJ/mol E) More information is needed, since this is a Hess's law calculation. A) 27 kJ/mol B) 47 kJ/mol C) 55 kJ/mol D) 102 kJ/mol E) More information is needed, since this is a Hess's law calculation.

In the collision theory of reaction rates, the rate constant for a bimolecular reaction can be written as k = zF1F1F1S1F1F1F10pF1F1F1S1F1F1F10exp(-Ea/RT) In one sentence each, clearly explain the physical meaning (interpretation) of the following three factors which appear in the above expression: a. z b. p c. exp(-Ea/RT)

a. z is a collision rate constant, such

The reaction CH3NC(g) F1F1F1S1F1F1F10 CH3CN(g) is first-order with respect to methyl isocyanide, CH3NC. If it takes 10.3 minutes for exactly one quarter of the initial amount of methyl isocyanide to react, what is the rate constant in units of min-1?

A) -0.135 min-1 B) 0.0279 min-1 C) 0.089 min-1 D) 0.135 min-1 E) 35.8 min-1 A) -0.135 min-1 B) 0.0279 min-1 C) 0.089 min-1 D) 0.135 min-1 E) 35.8 min-1

Briefly outline the key arguments in the collision theory of reaction rates for the elementary reaction C + D F1F1F1S1F1F1F10 products Show that this theory predicts a second-order rate law, and how it predicts the form of the rate constant k.

For reaction to occur, the molecules mus

The rate law for the reaction 3A F1F1F1S1F1F1F10 C is Rate = 4.36 × 10-2 L mol-1 hr-1[A]2 What is the half-life for the reaction if the initial concentration of A is 0.250 M?

A) 0.0109 hr B) 0.0629 hr C) 15.9 hr D) 23.9 hr E) 91.7 hr A) 0.0109 hr B) 0.0629 hr C) 15.9 hr D) 23.9 hr E) 91.7 hr

What is the molecularity of the following elementary reaction? NH2Cl(aq) + OH-(aq) F1F1F1S1F1F1F10 NHCl-(aq) + H2O(l)

A) unimolecular B) bimolecular C) termolecular D) tetramolecular E) Need to know the reaction order before molecularity can be determined. A) unimolecular B) bimolecular C) termolecular D) tetramolecular E) Need to know the reaction order before molecularity can be determined.

Exam 16: Kinetics: Rates and Mechanisms of Chemical Reactions

Ammonium cyanate (NH₄CNO) reacts to form urea (NH₂CONH₂). At 65°C the rate constant, k, is 3.60 L mol^-1s^-1. What is the rate law for this reaction?

(Multiple Choice)

4.9/5

(40)

Question 61

For the reaction 3A(g) + 2B(g)  2C(g) + 2D(g) The following data were collected at constant temperature. Determine the correct rate law for this reaction.

(Multiple Choice)

4.8/5

(45)

Question 62

A catalyst accelerates a reaction because

(Multiple Choice)

5.0/5

(38)

Question 63

The compound RX₃ decomposes according to the equation 3RX₃  R + R₂X₃+ 3X₂ In an experiment the following data were collected for the decomposition at 100°C. What is the average rate of reaction over the entire experiment?

(Multiple Choice)

4.8/5

(31)

Question 64

In going from room temperature (25.0 °C) to 10 °C above room temperature, the rate of a reaction doubles. Calculate the activation energy for the reaction.

(Multiple Choice)

4.7/5

(38)

Question 65

A gas-phase decomposition is first-order with respect to the reactant, R. If the initial concentration of R is 1.0 × 10^-4 mol L^-1 and the rate constant k = 1.08 × 10^-6 s^-1, what concentration of R remains after 25 days?

(Multiple Choice)

4.8/5

(37)

Question 66

Cyclobutane decomposes to ethene in a first-order reaction. From measurements of the rate constant (k) at various absolute temperatures (T), the accompanying Arrhenius plot was obtained (ln k versus 1/T). a. Calculate the energy of activation, E_a. b. Determine the value of the rate constant at 740. K. (In the plot, the units of k are s^-1.)

(Essay)

4.8/5

(41)

Question 67

Briefly list the features/properties common to all catalysts and how they work. Draw a labeled reaction energy diagram as part of your answer.

(Essay)

4.7/5

(34)

Question 68

The units of the rate of reaction depend on the order of the reaction.

(True/False)

4.9/5

(32)

Question 69

The decomposition of dinitrogen pentaoxide has an activation energy of 102 kJ/mol and H°_rxn = + 55 kJ/mol. What is the activation energy for the reverse reaction?

(Multiple Choice)

4.7/5

(29)

Question 70

The rate constant for a reaction is 4.65 L mol^-1s^-1. What is the overall order of the reaction?

(Multiple Choice)

4.9/5

(34)

Question 71

In the collision theory of reaction rates, the rate constant for a bimolecular reaction can be written as k = zpexp(-E_a/RT) In one sentence each, clearly explain the physical meaning (interpretation) of the following three factors which appear in the above expression: a. z b. p c. exp(-E_a/RT)

(Essay)

4.9/5

(34)

Question 72

A transition state is a species (or state) corresponding to an energy maximum on a reaction energy diagram.

(True/False)

4.9/5

(32)

Question 73

The radioactive isotope tritium decays with a first-order rate constant k of 0.056 year^-1. What fraction of the tritium initially in a sample is still present 30 years later?

(Multiple Choice)

4.9/5

(34)

Question 74

The reaction CH₃NC(g)  CH₃CN(g) is first-order with respect to methyl isocyanide, CH₃NC. If it takes 10.3 minutes for exactly one quarter of the initial amount of methyl isocyanide to react, what is the rate constant in units of min^-1?

(Multiple Choice)

4.8/5

(37)

Question 75

Briefly outline the key arguments in the collision theory of reaction rates for the elementary reaction C + D  products Show that this theory predicts a second-order rate law, and how it predicts the form of the rate constant k.

(Essay)

4.7/5

(30)

Question 76

For the reaction 2A + B + 2C  D + E The following initial rate data were collected at constant temperature. Determine the correct rate law for this reaction. All units are arbitrary.

(Multiple Choice)

4.7/5

(37)

Question 77

The rate law for the reaction 3A  C is Rate = 4.36 × 10^-2 L mol^-1hr^-1[A]² What is the half-life for the reaction if the initial concentration of A is 0.250 M?

(Multiple Choice)

4.8/5

(34)

Question 78

The rate of a reaction is determined by the rate of the fastest step in the mechanism.

(True/False)

4.7/5

(35)

Question 79

What is the molecularity of the following elementary reaction? NH₂Cl(aq) + OH^-(aq)  NHCl^-(aq) + H₂O(l)

(Multiple Choice)

4.8/5

(34)

Question 80

Showing 61 - 80 of 88

Exam 16: Kinetics: Rates and Mechanisms of Chemical Reactions

Ammonium cyanate (NH4CNO) reacts to form urea (NH2CONH2). At 65°C the rate constant, k, is 3.60 L mol-1s-1. What is the rate law for this reaction?

For the reaction 3A(g) + 2B(g)  2C(g) + 2D(g) The following data were collected at constant temperature. Determine the correct rate law for this reaction.

A catalyst accelerates a reaction because

The compound RX3 decomposes according to the equation 3RX3  R + R2X3 + 3X2 In an experiment the following data were collected for the decomposition at 100°C. What is the average rate of reaction over the entire experiment?

In going from room temperature (25.0 °C) to 10 °C above room temperature, the rate of a reaction doubles. Calculate the activation energy for the reaction.

A gas-phase decomposition is first-order with respect to the reactant, R. If the initial concentration of R is 1.0 × 10-4 mol L-1 and the rate constant k = 1.08 × 10-6 s-1, what concentration of R remains after 25 days?

Briefly list the features/properties common to all catalysts and how they work. Draw a labeled reaction energy diagram as part of your answer.

The units of the rate of reaction depend on the order of the reaction.

The decomposition of dinitrogen pentaoxide has an activation energy of 102 kJ/mol and H°rxn = + 55 kJ/mol. What is the activation energy for the reverse reaction?

The rate constant for a reaction is 4.65 L mol-1s-1. What is the overall order of the reaction?

In the collision theory of reaction rates, the rate constant for a bimolecular reaction can be written as k = zpexp(-Ea/RT) In one sentence each, clearly explain the physical meaning (interpretation) of the following three factors which appear in the above expression: a. z b. p c. exp(-Ea/RT)

A transition state is a species (or state) corresponding to an energy maximum on a reaction energy diagram.

The radioactive isotope tritium decays with a first-order rate constant k of 0.056 year-1. What fraction of the tritium initially in a sample is still present 30 years later?

The reaction CH3NC(g)  CH3CN(g) is first-order with respect to methyl isocyanide, CH3NC. If it takes 10.3 minutes for exactly one quarter of the initial amount of methyl isocyanide to react, what is the rate constant in units of min-1?

Briefly outline the key arguments in the collision theory of reaction rates for the elementary reaction C + D  products Show that this theory predicts a second-order rate law, and how it predicts the form of the rate constant k.

For the reaction 2A + B + 2C  D + E The following initial rate data were collected at constant temperature. Determine the correct rate law for this reaction. All units are arbitrary.

The rate law for the reaction 3A  C is Rate = 4.36 × 10-2 L mol-1 hr-1[A]2 What is the half-life for the reaction if the initial concentration of A is 0.250 M?

The rate of a reaction is determined by the rate of the fastest step in the mechanism.

What is the molecularity of the following elementary reaction? NH2Cl(aq) + OH-(aq)  NHCl-(aq) + H2O(l)

Keys to the Study of Chemistry

The Components of Matter

Stoichiometry of Formulas and Equations

The Major Classes of Chemical Reactions

Gases and the Kinetic-Molecular Theory

Thermochemistry: Energy Flow and Chemical Change

Quantum Theory and Atomic Structure

Electron Configuration and Chemical Periodicity

Models of Chemical Bonding

The Shapes of Molecules

Theories of Covalent Bonding

Intermolecular Forces: Liquids, Solids, and Phase Changes

The Properties of Mixtures: Solutions and Colloids

Periodic Patterns in the Main Group Elements: Bonding, Structure, and Reactivity

Organic Compounds and the Atomic Properties of Carbon

Equilibrium: the Extent of Chemical Reactions

Acid-Base Equilibria

Ionic Equilibria in Aqueous Systems

Thermodynamics: Entropy, Free Energy, and the Direction of Chemical Reactions

Electrochemistry: Chemical Change and Electrical Work

The Elements in Nature and Industry

The Transition Elements and Their Coordination Compounds

Nuclear Reactions and Their Applications

Filters

Ammonium cyanate (NH₄CNO) reacts to form urea (NH₂CONH₂). At 65°C the rate constant, k, is 3.60 L mol^-1s^-1. What is the rate law for this reaction?

The compound RX₃ decomposes according to the equation 3RX₃  R + R₂X₃+ 3X₂ In an experiment the following data were collected for the decomposition at 100°C. What is the average rate of reaction over the entire experiment?

A gas-phase decomposition is first-order with respect to the reactant, R. If the initial concentration of R is 1.0 × 10^-4 mol L^-1 and the rate constant k = 1.08 × 10^-6 s^-1, what concentration of R remains after 25 days?

The decomposition of dinitrogen pentaoxide has an activation energy of 102 kJ/mol and H°_rxn = + 55 kJ/mol. What is the activation energy for the reverse reaction?

The rate constant for a reaction is 4.65 L mol^-1s^-1. What is the overall order of the reaction?

The radioactive isotope tritium decays with a first-order rate constant k of 0.056 year^-1. What fraction of the tritium initially in a sample is still present 30 years later?

The reaction CH₃NC(g)  CH₃CN(g) is first-order with respect to methyl isocyanide, CH₃NC. If it takes 10.3 minutes for exactly one quarter of the initial amount of methyl isocyanide to react, what is the rate constant in units of min^-1?

The rate law for the reaction 3A  C is Rate = 4.36 × 10^-2 L mol^-1hr^-1[A]² What is the half-life for the reaction if the initial concentration of A is 0.250 M?

What is the molecularity of the following elementary reaction? NH₂Cl(aq) + OH^-(aq)  NHCl^-(aq) + H₂O(l)