A first-order reaction has a rate constant of 7.5 F1F1F1S1F1F1F10 10-3 /s. The time required for the reaction to be 60% complete is

A) 3.8 F1F1F1S1F1F1F10 10-3 s B) 6.9 F1F1F1S1F1F1F10 10-3 s C) 68 s D) 120 s E) 130 s A) 3.8 F1F1F1S1F1F1F10 10-3 s B) 6.9 F1F1F1S1F1F1F10 10-3 s C) 68 s D) 120 s E) 130 s D

The first-order reaction SO2Cl2 F1F1F1S1F1F1F10 SO2 + Cl2 is 10% complete in 80.min. How long would it take for the reaction to be 95% complete?

A) 1.8 min B) 104 min C) 530 min D) 2300 min E) 990 min A) 1.8 min B) 104 min C) 530 min D) 2300 min E) 990 min

The rate law for the reaction 2NO2 + O3 F1F1F1S1F1F1F10 N2O5 + O2 is rate = k[NO2][O3]. Which one of the following mechanisms is consistent with this rate law?

A) NO2 + NO2 F1F1F1S1F1F1F10 N2O4 (fast) N2O4 + O3 F1F1F1S1F1F1F10 N2O5 + O2 (slow) B) NO2 + O3 F1F1F1S1F1F1F10 NO5 (fast) NO5 + NO5 F1F1F1S1F1F1F10 N2O5 + 5/2O2 (slow) C) NO2 + O3 F1F1F1S1F1F1F10 NO3 + O2 (slow) NO3 + NO2 F1F1F1S1F1F1F10 N2O5 (fast) D) NO2 + NO2 F1F1F1S1F1F1F10 N2O2 + O2 (slow) N2O2 + O3 F1F1F1S1F1F1F10 N2O5 (fast) A) NO2 + NO2 F1F1F1S1F1F1F10 N2O4 (fast) N2O4 + O3 F1F1F1S1F1F1F10 N2O5 + O2 (slow) B) NO2 + O3 F1F1F1S1F1F1F10 NO5 (fast) NO5 + NO5 F1F1F1S1F1F1F10 N2O5 + 5/2O2 (slow) C) NO2 + O3 F1F1F1S1F1F1F10 NO3 + O2 (slow) NO3 + NO2 F1F1F1S1F1F1F10 N2O5 (fast) D) NO2 + NO2 F1F1F1S1F1F1F10 N2O2 + O2 (slow) N2O2 + O3 F1F1F1S1F1F1F10 N2O5 (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 one begins with 600.mmHg of pure SO2Cl2 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 activation energy for the following reaction is 60.kJ/mol. Sn2+ + 2Co3+ F1F1F1S1F1F1F10 Sn4+ + 2Co2+ By what factor (how many times)will the rate constant increase when the temperature is raised from 10°C to 28°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

The reaction A + 2B F1F1F1S1F1F1F10 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?

A) 2 B) 4 C) 6 D) 8 E) 9 A) 2 B) 4 C) 6 D) 8 E) 9

The gas phase reaction of nitrogen dioxide and carbon monoxide was found by experiment to be second-order with respect to NO2, and zeroth-order with respect to CO below 25°C. NO2 + CO F1F1F1S1F1F1F10 NO + CO2 Which one of the following mechanisms is consistent with the observed reaction order?

A) NO2 + 2CO N + 2CO2 fast N + NO2 F1F1F1S1F1F1F10 2NO slow B) NO2 + 2CO F1F1F1S1F1F1F10 N + 2CO2 slow N + NO2 F1F1F1S1F1F1F10 2NO fast C) NO2 + NO2 F1F1F1S1F1F1F10 NO3 + NO fast NO3 + CO F1F1F1S1F1F1F10 NO2 + CO2 slow D) NO2 + NO2 F1F1F1S1F1F1F10 NO3 + NO slow NO3 + CO F1F1F1S1F1F1F10 NO2 + CO2 fast A) NO2 + 2CO N + 2CO2 fast N + NO2 F1F1F1S1F1F1F10 2NO slow B) NO2 + 2CO F1F1F1S1F1F1F10 N + 2CO2 slow N + NO2 F1F1F1S1F1F1F10 2NO fast C) NO2 + NO2 F1F1F1S1F1F1F10 NO3 + NO fast NO3 + CO F1F1F1S1F1F1F10 NO2 + CO2 slow D) NO2 + NO2 F1F1F1S1F1F1F10 NO3 + NO slow NO3 + CO F1F1F1S1F1F1F10 NO2 + CO2 fast

Exam 13: Chemical Kinetics

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

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Question 1

Correct Answer:

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-36 kJ/mol

A first-order reaction has a rate constant of 7.5  10^-3/s. The time required for the reaction to be 60% complete is

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Question 2

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At 30°C, by how much is a reaction's activation energy decreased by the addition of a catalyst if the catalyst triples the reaction rate?

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Question 3

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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)

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Question 4

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?

(Short Answer)

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Question 5

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 6

For the following exothermic reaction, the rate law at 298 K is rate = k [H₂][I₂]. H₂(g)+ I₂(g) 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 7

For the reaction represented below, the experimental rate law is given by rate = k [(CH₃)₃CCl]. (CH₃)₃CCl(aq)+ OH^- (CH₃)₃COH(aq)+ Cl^- If some solid sodium hydroxide were added to a solution in which [(CH₃)₃CCl] = 0.01 M and [NaOH] = 0.10 M, which of the following would be true? (Assume the temperature and volume remain constant.)

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Question 8

With respect to the figure below, which choice correctly identifies all the numbered positions?

(Short Answer)

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Question 9

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

(Short Answer)

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Question 10

The first-order reaction SO₂Cl₂  SO₂ + Cl₂ is 10% complete in 80.min. How long would it take for the reaction to be 95% complete?

(Multiple Choice)

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Question 11

The rate law for the reaction 2NO₂ + O₃  N₂O₅ + O₂ is rate = k[NO₂][O₃]. Which one of the following mechanisms is consistent with this rate law?

(Multiple Choice)

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Question 12

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 one begins with 600.mmHg of pure SO₂Cl₂ 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)

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Question 13

For the reaction X + Y  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?

(Multiple Choice)

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Question 14

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

(Multiple Choice)

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Question 15

The reaction A + 2B  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?

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Question 16

At a particular temperature the first-order gas-phase reaction N₂O₅  2NO₂ + ¹/₂O₂ has a half-life for the disappearance of dinitrogen pentoxide of 5130 s. Suppose 0.450 atm of N₂O₅ is introduced into an evacuated 2.00 L flask. What will be the total gas pressure inside the flask after 3.00 hours?

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Question 17

Appropriate units for a second-order rate constant are

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Question 18

For the reaction whose rate law is rate = k[X], a plot of which of the following is a straight line?

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Question 19

The gas phase reaction of nitrogen dioxide and carbon monoxide was found by experiment to be second-order with respect to NO₂, and zeroth-order with respect to CO below 25°C. NO₂ + CO  NO + CO₂ Which one of the following mechanisms is consistent with the observed reaction order?

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Question 20

Showing 1 - 20 of 114

Exam 13: Chemical Kinetics

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

A first-order reaction has a rate constant of 7.5  10-3 /s. The time required for the reaction to be 60% complete is

At 30°C, by how much is a reaction's activation energy decreased by the addition of a catalyst if the catalyst triples the reaction rate?

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 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?

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.

With respect to the figure below, which choice correctly identifies all the numbered positions?

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

The first-order reaction SO2Cl2  SO2 + Cl2 is 10% complete in 80.min. How long would it take for the reaction to be 95% complete?

The rate law for the reaction 2NO2 + O3  N2O5 + O2 is rate = k[NO2][O3]. Which one of the following mechanisms is consistent with this rate law?

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 one begins with 600.mmHg of pure SO2Cl2 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?

For the reaction X + Y  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?

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

The reaction A + 2B  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?

Appropriate units for a second-order rate constant are

For the reaction whose rate law is rate = k[X], a plot of which of the following is a straight line?

The gas phase reaction of nitrogen dioxide and carbon monoxide was found by experiment to be second-order with respect to NO2, and zeroth-order with respect to CO below 25°C. NO2 + CO  NO + CO2 Which one of the following mechanisms is consistent with the observed reaction order?

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

A first-order reaction has a rate constant of 7.5  10^-3/s. The time required for the reaction to be 60% complete is

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 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?

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

The first-order reaction SO₂Cl₂  SO₂ + Cl₂ is 10% complete in 80.min. How long would it take for the reaction to be 95% complete?

The rate law for the reaction 2NO₂ + O₃  N₂O₅ + O₂ is rate = k[NO₂][O₃]. Which one of the following mechanisms is consistent with this rate law?

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 one begins with 600.mmHg of pure SO₂Cl₂ 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?

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

The reaction A + 2B  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?

The gas phase reaction of nitrogen dioxide and carbon monoxide was found by experiment to be second-order with respect to NO₂, and zeroth-order with respect to CO below 25°C. NO₂ + CO  NO + CO₂ Which one of the following mechanisms is consistent with the observed reaction order?