Ammonium ion (NH4+) reacts with nitrite ion (NO2-) to yield nitrogen gas and liquid water. The following initial rates of reaction have been measured for the given reactant concentrations. $\begin{array}{lccc} \text { Expt. \# } & {\left[\mathrm{NH}_{4}{ }^{+}\right]} & {\left[\mathrm{NO}_{2}{ }^{-}\right]} & \text {Initial rate }(\mathrm{M} / \mathrm{hr}) \\ \hline 1 & 0.010 & 0.020 & 0.020 \\ 2 & 0.015 & 0.020 & 0.030 \\ 3 & 0.030 & 0.010 & 0.015 \end{array}$ Which of the following is the rate law (rate equation) for this reaction

A) rate = k [NH4+] [NO2-]4 B) rate = k [NH4+] [NO2-] C) rate = k [NH4+] [NO2-]2 D) rate = k [NH4+]2 [NO2-] E) rate = k [NH4+]1/2 [NO2-]1/4 A) rate = k [NH4+] [NO2-]4 B) rate = k [NH4+] [NO2-] C) rate = k [NH4+] [NO2-]2 D) rate = k [NH4+]2 [NO2-] E) rate = k [NH4+]1/2 [NO2-]1/4

Given the rate law for a reaction, rate = k[A]2, where rate is measured in units of M min-1, what are the units for the rate constant k

A) M-2min-1 B) M-1min-2 C) M1min-1 D) M-1min-1 E) None of the above A) M-2min-1 B) M-1min-2 C) M1min-1 D) M-1min-1 E) None of the above

For the reaction C6H14(g) $\rarr$C6H6(g) + 4H2(g), $\Delta$P(H2)/$\Delta$t was found to be 2.5 * 10-2 atm/s, where $\Delta$P(H2) is the change in pressure of hydrogen. Determine $\Delta$P(C6H14)/$\Delta$t for this reaction at the same time.

A) 2.5 * 10-2 atm/s B) -6.2 * 10-3 atm/s C) -2.5 * 10-2 atm/s D) 0.10 atm/s E) 6.2 * 10-3 atm/s A) 2.5 * 10-2 atm/s B) -6.2 * 10-3 atm/s C) -2.5 * 10-2 atm/s D) 0.10 atm/s E) 6.2 * 10-3 atm/s

The activation energy for the following reaction is 60. kJ/mol.Sn2+ + 2Co3+ $\rarr$ Sn4+ + 2Co2+ By what factor (how many times) will the rate constant increase when the temperature is raised from 10$\circ$C to 28$\circ$C

A) 1.002 B) 4.6 C) 5.6 D) 2.8 E) 696 A) 1.002 B) 4.6 C) 5.6 D) 2.8 E) 696

Nitric acid is formed by the gas-phase hydrolysis of N2O5. For the reaction N2O5 + H2O $\rarr$2HNO3, Ea(forward) = 15 kJ/mol and Ea(reverse) = 51 kJ/mol. Calculate $\Delta$Hrxn.

A) -36 kJ/mol B) -56 kJ/mol C) -76 kJ/mol D) -96 kJ/mol E) None of the above A) -36 kJ/mol B) -56 kJ/mol C) -76 kJ/mol D) -96 kJ/mol E) None of the above

Calculate the activation energy, in kJ/mol, for the redox reaction Sn2+ + 2Co3+ $\rarr$ Sn4+ + 2Co2+. $\begin{array}{cc} \operatorname{Temp}\left({ }^{\circ} \mathrm{C}\right) & \mathrm{k}(1 / \mathrm{M} \cdot \mathrm{~s})\\\hline 2 & 3.12 \times 10^{3} \\ 27 & 27.0 \times 10^{3} \end{array}$

A) 59.2 B) 0.477 C) 5.37 D) 163 kJ E) 48.1 kJ A) 59.2 B) 0.477 C) 5.37 D) 163 kJ E) 48.1 kJ

Given the rate law for a reaction, rate = k[A][B]2, where rate is measured in units of M s-1, what are the units for the rate constant k

A) M-2s-2 B) M-1s C) M-2s D) M2s E) None of the above A) M-2s-2 B) M-1s C) M-2s D) M2s E) None of the above

The peroxodisulfate ion can oxidize iodide ions to iodine according to the balanced equation S2O82- + 2I - $\rarr$ 2SO42- + I2.The reaction is catalyzed by certain chemical species. Identify the catalyst in the following mechanism: Step 1: Fe3+ + 2I - $\rarr$ Fe2+ + I2 Step 2: S2O82- + Fe2+ $\rarr$ 2SO42- + Fe3+

A) Fe3+ B) I - C) S2O82- D) Fe2+ E) SO42- A) Fe3+ B) I - C) S2O82- D) Fe2+ E) SO42-

The rate constant for the first-order decomposition of C4H8 at 500$\circ$C is 9.2 * 10-3 s-1. How long will it take for 10.0% of a 0.100 M sample of C4H8 to decompose at 500$\circ$C

A) 11 s B) 14 s C) 18 s D) 22 s E) None of the above A) 11 s B) 14 s C) 18 s D) 22 s E) None of the above

Exam 13: Chemical Kinetics

Ammonium ion (NH₄⁺) reacts with nitrite ion (NO₂^-) to yield nitrogen gas and liquid water. The following initial rates of reaction have been measured for the given reactant concentrations. Expt. \# Initial rate (/) 1 0.010 0.020 0.020 2 0.015 0.020 0.030 3 0.030 0.010 0.015 Which of the following is the rate law (rate equation) for this reaction

(Multiple Choice)

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Question 101

The activation energy for a certain reaction is 113 kJ/mol. By what factor (how many times) will the rate constant increase when the temperature is raised from 310 K to 325 K

(Multiple Choice)

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Question 102

Given the rate law for a reaction, rate = k[A]², where rate is measured in units of M min^-1, what are the units for the rate constant k

(Multiple Choice)

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Question 103

The reaction A + 2B $\rarr$ products has been found to have the rate law, rate = k[A] [B]². While holding the concentration of A constant, the concentration of B is increased from x to 3x. Predict by what factor the rate of reaction increases.

(Multiple Choice)

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Question 104

The half life for a first order reaction is 45 min. What is the rate constant in units of s^-1

(Multiple Choice)

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Question 105

Which of the following elementary steps is bimolecular

(Multiple Choice)

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Question 106

According to the collision theory, all collisions do not lead to reaction. Which choice gives both reasons why not all collisions between reactant molecules lead to reaction 1. The total energy of two colliding molecules is less than some minimum amount of energy. 2. Molecules cannot react with each other unless a catalyst is present. 3. Molecules that are improperly oriented during collision will not react. 4. Solids cannot react with gases.

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Question 107

For the reaction C₆H₁₄(g) $\rarr$ C₆H₆(g) + 4H₂(g), $\Delta$ P(H₂)/ $\Delta$ t was found to be 2.5 * 10^-2 atm/s, where $\Delta$ P(H₂) is the change in pressure of hydrogen. Determine $\Delta$ P(C₆H₁₄)/ $\Delta$ t for this reaction at the same time.

(Multiple Choice)

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Question 108

The activation energy for the following reaction is 60. kJ/mol.Sn²⁺ + 2Co³⁺ $\rarr$ Sn⁴⁺ + 2Co²⁺ By what factor (how many times) will the rate constant increase when the temperature is raised from 10^$\circ$C to 28^$\circ$C

(Multiple Choice)

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Question 109

The reaction A + 2B $\rarr$ products has the rate law, rate = k[A][B]³. If the concentration of B is doubled while that of A is unchanged, by what factor will the rate of reaction increase

(Multiple Choice)

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Question 110

Nitric acid is formed by the gas-phase hydrolysis of N₂O₅. For the reaction N₂O₅ + H₂O $\rarr$ 2HNO₃, E_a(forward) = 15 kJ/mol and E_a(reverse) = 51 kJ/mol. Calculate $\Delta$ H_rxn.

(Multiple Choice)

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Question 111

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

(Multiple Choice)

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Question 112

The reaction A + 2B $\rarr$ products was found to have the rate law, rate = k[A] [B]². Predict by what factor the rate of reaction will increase when the concentration of A is doubled and the concentration of B is also doubled.

(Multiple Choice)

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Question 113

At a particular temperature the first-order gas-phase reaction 2N₂O₅ $\rarr$ 2N₂O₄ + O₂ has a half-life for the disappearance of dinitrogen pentoxide of 3240 s. If 1.00 atm of N₂O₅ is introduced into an evacuated 5.00 L flask, what will be the total pressure of the gases in the flask after 1.50 hours

(Multiple Choice)

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Question 114

Calculate the activation energy, in kJ/mol, for the redox reaction Sn²⁺ + 2Co³⁺ $\rarr$ Sn⁴⁺ + 2Co²⁺. Temp (1/\cdot) 2 3.12\times1 27 27.0\times1

(Multiple Choice)

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Question 115

Given the rate law for a reaction, rate = k[A][B]², where rate is measured in units of M s^-1, what are the units for the rate constant k

(Multiple Choice)

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Question 116

The peroxodisulfate ion can oxidize iodide ions to iodine according to the balanced equation S₂O₈^2- + 2I ^- $\rarr$ 2SO₄^2- + I₂.The reaction is catalyzed by certain chemical species. Identify the catalyst in the following mechanism: Step 1: Fe³⁺ + 2I ^- $\rarr$ Fe²⁺ + I₂ Step 2: S₂O₈^2- + Fe²⁺ $\rarr$ 2SO₄^2- + Fe³⁺

(Multiple Choice)

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Question 117

Substitute natural gas can be synthesized by passing carbon monoxide and hydrogen over Ni or Co at 400^$\circ$C. $Substitute natural gas can be synthesized by passing carbon monoxide and hydrogen over Ni or Co at 400<sup> \circ </sup>C. This process is an example of homogeneous catalysis.$ This process is an example of homogeneous catalysis.

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Question 118

The rate constant for the first-order decomposition of C₄H₈ at 500^$\circ$C is 9.2 * 10^-3 s^-1. How long will it take for 10.0% of a 0.100 M sample of C₄H₈ to decompose at 500^$\circ$C

(Multiple Choice)

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Question 119

For the chemical reaction A $\rarr$ C, a plot of 1/[A]_t versus time was found to give a straight line with a positive slope. What is the order of reaction

(Multiple Choice)

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Question 120

Showing 101 - 120 of 131

The activation energy for a certain reaction is 113 kJ/mol. By what factor (how many times) will the rate constant increase when the temperature is raised from 310 K to 325 K

Given the rate law for a reaction, rate = k[A]², where rate is measured in units of M min^-1, what are the units for the rate constant k

The reaction A + 2B $\rarr$ products has been found to have the rate law, rate = k[A] [B]². While holding the concentration of A constant, the concentration of B is increased from x to 3x. Predict by what factor the rate of reaction increases.

The half life for a first order reaction is 45 min. What is the rate constant in units of s^-1

Which of the following elementary steps is bimolecular

For the reaction C₆H₁₄(g) $\rarr$ C₆H₆(g) + 4H₂(g), $\Delta$ P(H₂)/ $\Delta$ t was found to be 2.5 * 10^-2 atm/s, where $\Delta$ P(H₂) is the change in pressure of hydrogen. Determine $\Delta$ P(C₆H₁₄)/ $\Delta$ t for this reaction at the same time.

The activation energy for the following reaction is 60. kJ/mol.Sn²⁺ + 2Co³⁺ $\rarr$ Sn⁴⁺ + 2Co²⁺ By what factor (how many times) will the rate constant increase when the temperature is raised from 10^$\circ$C to 28^$\circ$C

The reaction A + 2B $\rarr$ products has the rate law, rate = k[A][B]³. If the concentration of B is doubled while that of A is unchanged, by what factor will the rate of reaction increase

Nitric acid is formed by the gas-phase hydrolysis of N₂O₅. For the reaction N₂O₅ + H₂O $\rarr$ 2HNO₃, E_a(forward) = 15 kJ/mol and E_a(reverse) = 51 kJ/mol. Calculate $\Delta$ H_rxn.

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

The reaction A + 2B $\rarr$ products was found to have the rate law, rate = k[A] [B]². Predict by what factor the rate of reaction will increase when the concentration of A is doubled and the concentration of B is also doubled.

Calculate the activation energy, in kJ/mol, for the redox reaction Sn²⁺ + 2Co³⁺ $\rarr$ Sn⁴⁺ + 2Co²⁺. Temp (1/\cdot) 2 3.12\times1 27 27.0\times1

Given the rate law for a reaction, rate = k[A][B]², where rate is measured in units of M s^-1, what are the units for the rate constant k

The rate constant for the first-order decomposition of C₄H₈ at 500^$\circ$C is 9.2 * 10^-3 s^-1. How long will it take for 10.0% of a 0.100 M sample of C₄H₈ to decompose at 500^$\circ$C

For the chemical reaction A $\rarr$ C, a plot of 1/[A]_t versus time was found to give a straight line with a positive slope. What is the order of reaction

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Exam 13: Chemical Kinetics

The activation energy for a certain reaction is 113 kJ/mol. By what factor (how many times) will the rate constant increase when the temperature is raised from 310 K to 325 K

Given the rate law for a reaction, rate = k[A]2, where rate is measured in units of M min-1, what are the units for the rate constant k

The reaction A + 2B →\rarr→ products has been found to have the rate law, rate = k[A] [B]2. While holding the concentration of A constant, the concentration of B is increased from x to 3x. Predict by what factor the rate of reaction increases.

The half life for a first order reaction is 45 min. What is the rate constant in units of s-1

Which of the following elementary steps is bimolecular

For the reaction C6H14(g) →\rarr→ C6H6(g) + 4H2(g), Δ\DeltaΔ P(H2)/ Δ\DeltaΔ t was found to be 2.5 * 10-2 atm/s, where Δ\DeltaΔ P(H2) is the change in pressure of hydrogen. Determine Δ\DeltaΔ P(C6H14)/ Δ\DeltaΔ t for this reaction at the same time.

The activation energy for the following reaction is 60. kJ/mol.Sn2+ + 2Co3+ →\rarr→ Sn4+ + 2Co2+ By what factor (how many times) will the rate constant increase when the temperature is raised from 10 ∘\circ∘ C to 28 ∘\circ∘ C

The reaction A + 2B →\rarr→ products has the rate law, rate = k[A][B]3. If the concentration of B is doubled while that of A is unchanged, by what factor will the rate of reaction increase

Nitric acid is formed by the gas-phase hydrolysis of N2O5. For the reaction N2O5 + H2O →\rarr→ 2HNO3, Ea(forward) = 15 kJ/mol and Ea(reverse) = 51 kJ/mol. Calculate Δ\DeltaΔ Hrxn.

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

The reaction A + 2B →\rarr→ products was found to have the rate law, rate = k[A] [B]2. Predict by what factor the rate of reaction will increase when the concentration of A is doubled and the concentration of B is also doubled.

Calculate the activation energy, in kJ/mol, for the redox reaction Sn2+ + 2Co3+ →\rarr→ Sn4+ + 2Co2+. Temp (1/\cdot) 2 3.12\times1 27 27.0\times1

Given the rate law for a reaction, rate = k[A][B]2, where rate is measured in units of M s-1, what are the units for the rate constant k

Substitute natural gas can be synthesized by passing carbon monoxide and hydrogen over Ni or Co at 400 ∘\circ∘ C. This process is an example of homogeneous catalysis.

The rate constant for the first-order decomposition of C4H8 at 500 ∘\circ∘ C is 9.2 * 10-3 s-1. How long will it take for 10.0% of a 0.100 M sample of C4H8 to decompose at 500 ∘\circ∘ C

For the chemical reaction A →\rarr→ C, a plot of 1/[A]t versus time was found to give a straight line with a positive slope. What is the order of reaction

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

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

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Metallurgy and the Chemistry of Metals

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Given the rate law for a reaction, rate = k[A]², where rate is measured in units of M min^-1, what are the units for the rate constant k

The reaction A + 2B $\rarr$ products has been found to have the rate law, rate = k[A] [B]². While holding the concentration of A constant, the concentration of B is increased from x to 3x. Predict by what factor the rate of reaction increases.

The half life for a first order reaction is 45 min. What is the rate constant in units of s^-1

For the reaction C₆H₁₄(g) $\rarr$ C₆H₆(g) + 4H₂(g), $\Delta$ P(H₂)/ $\Delta$ t was found to be 2.5 * 10^-2 atm/s, where $\Delta$ P(H₂) is the change in pressure of hydrogen. Determine $\Delta$ P(C₆H₁₄)/ $\Delta$ t for this reaction at the same time.

The activation energy for the following reaction is 60. kJ/mol.Sn²⁺ + 2Co³⁺ $\rarr$ Sn⁴⁺ + 2Co²⁺ By what factor (how many times) will the rate constant increase when the temperature is raised from 10^$\circ$C to 28^$\circ$C

The reaction A + 2B $\rarr$ products has the rate law, rate = k[A][B]³. If the concentration of B is doubled while that of A is unchanged, by what factor will the rate of reaction increase

Nitric acid is formed by the gas-phase hydrolysis of N₂O₅. For the reaction N₂O₅ + H₂O $\rarr$ 2HNO₃, E_a(forward) = 15 kJ/mol and E_a(reverse) = 51 kJ/mol. Calculate $\Delta$ H_rxn.

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

The reaction A + 2B $\rarr$ products was found to have the rate law, rate = k[A] [B]². Predict by what factor the rate of reaction will increase when the concentration of A is doubled and the concentration of B is also doubled.

Calculate the activation energy, in kJ/mol, for the redox reaction Sn²⁺ + 2Co³⁺ $\rarr$ Sn⁴⁺ + 2Co²⁺. Temp (1/\cdot) 2 3.12\times1 27 27.0\times1

Given the rate law for a reaction, rate = k[A][B]², where rate is measured in units of M s^-1, what are the units for the rate constant k

The rate constant for the first-order decomposition of C₄H₈ at 500^$\circ$C is 9.2 * 10^-3 s^-1. How long will it take for 10.0% of a 0.100 M sample of C₄H₈ to decompose at 500^$\circ$C

For the chemical reaction A $\rarr$ C, a plot of 1/[A]_t versus time was found to give a straight line with a positive slope. What is the order of reaction