Question 1

For the following exothermic reaction, the rate law at 298 K is rate = k [H₂][I₂]. H₂(g)+ I₂(g)$\rarr$ 2HI(g) Predict the effect of each of the following changes on the initial rate of the reaction: a.Addition of hydrogen gas at constant temperature and volume b.Increase in volume of the reaction vessel at constant temperature c.Addition of a catalyst d.Increase in temperature

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Question 2

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?

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Question 3

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?

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Question 4

The reaction 2A + B $\rarr$ products is second order with respect to A and zero-order with respect to B.Starting with 0.135 M of A, what is the concentration of A after 35 min if the rate constant is 0.11 M^-1s^-1?

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Question 5

The rate constant for the first-order decomposition of C₄H₈ at 500°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°C?

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Question 6

The rate constant for a certain first-order reaction is 0.40/min.What is the initial rate in mole/L·min, if the initial concentration of the compound involved is 0.50 mol/L?

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Question 7

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

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Question 8

The oxidation of iodide ions by arsenic acid in acidic aqueous solution occurs according to the net reaction H₃AsO₄ + 3I^-+ 2 H₃O⁺ $\rarr$ H₃AsO₃ + I₃^-+ H₂O.The experimental rate law for this reaction is Rate = k [H₃AsO₄] [I^-] [H₃O⁺]. According to the rate law for the reaction, an increase in the concentration of hydronium ion has what effect on this reaction?

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Question 9

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.

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Question 10

Hydrogen peroxide decomposes to water and oxygen gas, and the activation energy for this process is 42 kJ/mol.The hydrogen peroxide formed in biological processes is harmful to tissue, but the enzyme catalase catalyzes the decomposition of hydrogen peroxide by lowering the activation energy to 7.0 kJ/mol.Assuming the frequency factor is the same for both processes and independent of temperature, calculate the temperature required for the uncatalyzed decomposition to proceed at the same rate as the enzyme-catalyzed decomposition at 37°C (normal human body temperature).Is this a reasonable temperature for a biological organism?

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Question 11

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 12

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?

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Question 13

An experimental drug, D, is known to decompose in the blood stream.Tripling the concentration of the drug increases the decomposition rate by a factor of nine.Write the rate law for decomposition of D and give the units of the rate constant.

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Question 14

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

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Question 15

For the first-order reaction 2N₂O₅ $\rarr$2N₂O₄ + O₂ at a particular temperature, the half-life of N₂O₅ is 0.90 hr.What fraction of the initial concentration of N₂O₅ will remain after 2.4 hours?

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Question 16

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)?

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Question 17

Nitrogen pentoxide decomposes by a first-order process yielding N₂O₄ and oxygen. 2N₂O₅ $\rarr$2N₂O₄ + O₂ At a given temperature, the half-life of N₂O₅ is 0.90 hr.What is the first-order rate constant for N₂O₅ decomposition?

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Question 18

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.

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Question 19

Nitric acid is formed by the gas-phase hydrolysis of N₂O₅.Draw an energy profile curve for the reaction N₂O₅ + H₂O $\rarr$2HNO₃ given that E_a(forward)= 15 kJ and E_a(reverse)= 51 kJ/mol.Label the activation energies of the forward and reverse reactions and label $\Delta$H for the reaction.

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Question 20

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

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Quiz 13: Chemical Kinetics

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?

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 2A + B $\rarr$ products is second order with respect to A and zero-order with respect to B.Starting with 0.135 M of A, what is the concentration of A after 35 min if the rate constant is 0.11 M^-1s^-1?

The rate constant for the first-order decomposition of C₄H₈ at 500°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°C?

The rate constant for a certain first-order reaction is 0.40/min.What is the initial rate in mole/L·min, if the initial concentration of the compound involved is 0.50 mol/L?

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?

An experimental drug, D, is known to decompose in the blood stream.Tripling the concentration of the drug increases the decomposition rate by a factor of nine.Write the rate law for decomposition of D and give the units of the rate constant.

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

For the first-order reaction 2N₂O₅ $\rarr$ 2N₂O₄ + O₂ at a particular temperature, the half-life of N₂O₅ is 0.90 hr.What fraction of the initial concentration of N₂O₅ will remain after 2.4 hours?

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)?

Nitrogen pentoxide decomposes by a first-order process yielding N₂O₄ and oxygen. 2N₂O₅ $\rarr$ 2N₂O₄ + O₂ At a given temperature, the half-life of N₂O₅ is 0.90 hr.What is the first-order rate constant for N₂O₅ decomposition?

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.

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

Quiz 13: Chemical Kinetics

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?

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 2A + B →\rarr→ products is second order with respect to A and zero-order with respect to B.Starting with 0.135 M of A, what is the concentration of A after 35 min if the rate constant is 0.11 M-1s-1?

The rate constant for the first-order decomposition of C4H8 at 500°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°C?

The rate constant for a certain first-order reaction is 0.40/min.What is the initial rate in mole/L·min, if the initial concentration of the compound involved is 0.50 mol/L?

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

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 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?

An experimental drug, D, is known to decompose in the blood stream.Tripling the concentration of the drug increases the decomposition rate by a factor of nine.Write the rate law for decomposition of D and give the units of the rate constant.

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

For the first-order reaction 2N2O5 →\rarr→ 2N2O4 + O2 at a particular temperature, the half-life of N2O5 is 0.90 hr.What fraction of the initial concentration of N2O5 will remain after 2.4 hours?

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)?

Nitrogen pentoxide decomposes by a first-order process yielding N2O4 and oxygen. 2N2O5 →\rarr→ 2N2O4 + O2 At a given temperature, the half-life of N2O5 is 0.90 hr.What is the first-order rate constant for N2O5 decomposition?

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.

Nitric acid is formed by the gas-phase hydrolysis of N2O5.Draw an energy profile curve for the reaction N2O5 + H2O →\rarr→ 2HNO3 given that Ea(forward)= 15 kJ and Ea(reverse)= 51 kJ/mol.Label the activation energies of the forward and reverse reactions and label Δ\DeltaΔ H for the reaction.

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

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?

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 2A + B $\rarr$ products is second order with respect to A and zero-order with respect to B.Starting with 0.135 M of A, what is the concentration of A after 35 min if the rate constant is 0.11 M^-1s^-1?

The rate constant for the first-order decomposition of C₄H₈ at 500°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°C?

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

For the first-order reaction 2N₂O₅ $\rarr$ 2N₂O₄ + O₂ at a particular temperature, the half-life of N₂O₅ is 0.90 hr.What fraction of the initial concentration of N₂O₅ will remain after 2.4 hours?

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)?

Nitrogen pentoxide decomposes by a first-order process yielding N₂O₄ and oxygen. 2N₂O₅ $\rarr$ 2N₂O₄ + O₂ At a given temperature, the half-life of N₂O₅ is 0.90 hr.What is the first-order rate constant for N₂O₅ decomposition?

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.

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