Question 1

Write the overall equation of reaction for the following mechanism and identify the reaction intermediates: 2 NO₂ $\rightarrow$NO₃ + NO NO₃ + CO $\rightarrow$ CO₂ + NO₂

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Question 2

The industrial production of 2-propanol involves the reaction of propene with sulphuric acid and then water. Write the second step of the mechanism if the following is the first step:

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Question 3

Draw a molecular picture showing the termolecular process in which two NO molecules collide with an O₂ molecule to give two molecules of NO₂.

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Question 4

Hydrogen peroxide decomposes according to the equation: 2 H₂O₂₍_aq₎ $\rightarrow$ 2 H₂O_(l)+ O_2(g) At 27°C and 1 atm, a 50.0 ml sample of hydrogen peroxide decomposes at a rate that produces 10.0 ml/sec of O₂₍_g). Assuming ideal behavioura) Determine the moles of oxygen produced per second.b) Determine the change in molarity of H₂O₂ per second.

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2...

Question 5

The following concentration vs. time data were collected for the reaction:
A + 2B$\rightarrow$C  Calculate  for A, B and C for the following time differences:(a) 0 and 60 s,(b) 900 and 960 s,(c) What is the rate of the reaction for part

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Question 6

Consider the following three molecular pictures that represent the relative numbers of the two reactants involved in one step of the depletion of stratospheric ozone by chlorine atoms: The equation for the elementary reaction and a molecular picture of the reaction process are shown below:Cl• + O₃$\rightarrow$ ClO + O₂ If the three samples represented by A, B and C are at the same temperature, what are the rates of reaction of B and C compared to that of A?

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Question 7

The reaction of NO₂ with CO to give CO₂ and NO can proceed through different mechanisms. What first step would be consistent with the following rate law?Rate = k[NO₂][CO]

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Question 8

What are the units of a rate constant for a reaction that has an overall order of 3?

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Question 9

The reaction of NO₂ with CO to give CO₂ and NO can proceed through different mechanisms. What rate law would be consistent for the following first step? 2 NO₂ $\rightarrow$ NO + NO₃

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Question 10

The rate law for the reaction of NO with O₂ to give NO₂ is shown below:rate = k [NO]²[O₂] a) If all other conditions are kept constant, what will be the effect on the rate if the concentration of NO is doubled? b) If all other conditions are kept constant, what will be the effect on the rate if the concentration of O₂ is doubled?

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Question 11

At moderate temperatures, the rate law for the reaction of NO₂ and CO to give CO₂ and NO follows the rate law shown below:rate = k [NO₂]² In which flask will the reaction be faster and how much faster?

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Question 12

Radioactive decay follows first-order kinetics. Some smoke detectors use the isotope ²⁴¹Am that has a half-life of 432.2 years. In how many years will 95% of the ²⁴¹Am have decayed?

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Question 13

Trioxane undergoes decomposition to formaldehyde at elevated temperatures.C₃H₆O₃(g)$\rightarrow$3 CH₂O (g)The following data was collected for the gas phase reaction at 519ºK: Determine the order of the decomposition in trioxane and the rate constant at 519ºK.

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Question 14

Ammonium cyanate undergoes rearrangement to form urea in aqueous solution.NH₄NCO(aq)$\rightarrow$CO(NH₂)₂ (aq)The following data was collected: Determine the order of the reaction and the rate constant.

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Question 15

Sucrose, cane sugar, reacts with water in acid solution to give glucose and fructose, which have the same chemical formula. C₁₂H₂₂O₁₁ (aq) + H₂O (l) $\rightarrow$2 C₆H₁₂O₆ (aq) The following data were obtained at room temperature for sucrose: Use graphical means to determine the order of the reaction and write the rate law with the numerical value of the rate constant with time units of seconds.

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Question 16

Rate data were collected for the following reaction at a constant temperature.2ClO₂₍_aq₎ + 2 OH^-1₍_aq₎$\rightarrow$ClO₃^-1₍_aq₎+ ClO₂^-1₍_aq₎ + H₂O_(l) a) Determine the rate law for this reaction.b) Determine the rate constant with appropriate units.

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Question 17

Nitrous oxide, N₂O, decomposes on metal surfaces readily at high temperatures following first-order kinetics for the equation: 2 N₂O (g) $\rightarrow$2 N₂ (g) + O₂ (g) The following data are obtained for a reaction at 850°C: Determine the rate constant and half-life for the reaction.

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Question 18

The following are initial rate data for 2 NO + 2 H₂ $\rightarrow$ N₂ + 2 H₂O The rate law is determined to be: rate = k[NO]²[H₂]. With this information determine k using the data from experiment 2.

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Question 19

Assume that the following first-order reaction has a rate constant k = 0.0137/min: SO₂Cl₂ $\rightarrow$ SO₂ + Cl₂ Given the initial [SO₂Cl₂] = 0.42 M, how many minutes will it take for [SO₂Cl₂] = 0.19 M?

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Question 20

The three reactions below, with identical reaction stoichiometry, must all share the same third order rate law found for the reaction of NO and O₂. True or False, and why? 2 NO(g) + O₂(g) $\rarr$ 2 NO₂(g)2 NO(g) + Cl₂(g) $\rarr$ 2 NOCl(g)2 NO(g) + F₂(g) $\rarr$ 2 NOF(g)

Accepted Answer

the stoichiometry and rate law are not related.

Quiz 13: Kinetics: Mechanisms and Rates of Reactions

Write the overall equation of reaction for the following mechanism and identify the reaction intermediates: 2 NO₂ $\rightarrow$ NO₃ + NO NO₃ + CO $\rightarrow$ CO₂ + NO₂

The industrial production of 2-propanol involves the reaction of propene with sulphuric acid and then water. Write the second step of the mechanism if the following is the first step:

Draw a molecular picture showing the termolecular process in which two NO molecules collide with an O₂ molecule to give two molecules of NO₂.

The reaction of NO₂ with CO to give CO₂ and NO can proceed through different mechanisms. What first step would be consistent with the following rate law?Rate = k[NO₂][CO]

What are the units of a rate constant for a reaction that has an overall order of 3?

The reaction of NO₂ with CO to give CO₂ and NO can proceed through different mechanisms. What rate law would be consistent for the following first step? 2 NO₂ $\rightarrow$ NO + NO₃

At moderate temperatures, the rate law for the reaction of NO₂ and CO to give CO₂ and NO follows the rate law shown below:rate = k [NO₂]² In which flask will the reaction be faster and how much faster?

Radioactive decay follows first-order kinetics. Some smoke detectors use the isotope ²⁴¹Am that has a half-life of 432.2 years. In how many years will 95% of the ²⁴¹Am have decayed?

Assume that the following first-order reaction has a rate constant k = 0.0137/min: SO₂Cl₂ $\rightarrow$ SO₂ + Cl₂ Given the initial [SO₂Cl₂] = 0.42 M, how many minutes will it take for [SO₂Cl₂] = 0.19 M?

The three reactions below, with identical reaction stoichiometry, must all share the same third order rate law found for the reaction of NO and O₂. True or False, and why? 2 NO(g) + O₂(g) $\rarr$ 2 NO₂(g)2 NO(g) + Cl₂(g) $\rarr$ 2 NOCl(g)2 NO(g) + F₂(g) $\rarr$ 2 NOF(g)

Quiz 13: Kinetics: Mechanisms and Rates of Reactions

Write the overall equation of reaction for the following mechanism and identify the reaction intermediates: 2 NO2 →\rightarrow→ NO3 + NO NO3 + CO →\rightarrow→ CO2 + NO2

The industrial production of 2-propanol involves the reaction of propene with sulphuric acid and then water. Write the second step of the mechanism if the following is the first step:

Draw a molecular picture showing the termolecular process in which two NO molecules collide with an O2 molecule to give two molecules of NO2.

The following concentration vs. time data were collected for the reaction: A + 2B →\rightarrow→ C Calculate for A, B and C for the following time differences:(a) 0 and 60 s,(b) 900 and 960 s,(c) What is the rate of the reaction for part

The reaction of NO2 with CO to give CO2 and NO can proceed through different mechanisms. What first step would be consistent with the following rate law?Rate = k[NO2][CO]

What are the units of a rate constant for a reaction that has an overall order of 3?

The reaction of NO2 with CO to give CO2 and NO can proceed through different mechanisms. What rate law would be consistent for the following first step? 2 NO2 →\rightarrow→ NO + NO3

At moderate temperatures, the rate law for the reaction of NO2 and CO to give CO2 and NO follows the rate law shown below:rate = k [NO2]2 In which flask will the reaction be faster and how much faster?

Radioactive decay follows first-order kinetics. Some smoke detectors use the isotope 241Am that has a half-life of 432.2 years. In how many years will 95% of the 241Am have decayed?

Trioxane undergoes decomposition to formaldehyde at elevated temperatures.C3H6O3 (g) →\rightarrow→ 3 CH2O (g)The following data was collected for the gas phase reaction at 519ºK: Determine the order of the decomposition in trioxane and the rate constant at 519ºK.

Ammonium cyanate undergoes rearrangement to form urea in aqueous solution.NH4NCO(aq) →\rightarrow→ CO(NH2)2 (aq)The following data was collected: Determine the order of the reaction and the rate constant.

Rate data were collected for the following reaction at a constant temperature.2ClO2(aq) + 2 OH-1(aq) →\rightarrow→ ClO3-1(aq) + ClO2-1(aq) + H2O(l) a) Determine the rate law for this reaction.b) Determine the rate constant with appropriate units.

Nitrous oxide, N2O, decomposes on metal surfaces readily at high temperatures following first-order kinetics for the equation: 2 N2O (g) →\rightarrow→ 2 N2 (g) + O2 (g) The following data are obtained for a reaction at 850°C: Determine the rate constant and half-life for the reaction.

The following are initial rate data for 2 NO + 2 H2 →\rightarrow→ N2 + 2 H2O The rate law is determined to be: rate = k[NO]2[H2]. With this information determine k using the data from experiment 2.

Assume that the following first-order reaction has a rate constant k = 0.0137/min: SO2Cl2 →\rightarrow→ SO2 + Cl2 Given the initial [SO2Cl2] = 0.42 M, how many minutes will it take for [SO2Cl2] = 0.19 M?

The three reactions below, with identical reaction stoichiometry, must all share the same third order rate law found for the reaction of NO and O2. True or False, and why? 2 NO(g) + O2(g) →\rarr→ 2 NO2(g)2 NO(g) + Cl2(g) →\rarr→ 2 NOCl(g)2 NO(g) + F2(g) →\rarr→ 2 NOF(g)

Write the overall equation of reaction for the following mechanism and identify the reaction intermediates: 2 NO₂ $\rightarrow$ NO₃ + NO NO₃ + CO $\rightarrow$ CO₂ + NO₂

Draw a molecular picture showing the termolecular process in which two NO molecules collide with an O₂ molecule to give two molecules of NO₂.

The reaction of NO₂ with CO to give CO₂ and NO can proceed through different mechanisms. What first step would be consistent with the following rate law?Rate = k[NO₂][CO]

The reaction of NO₂ with CO to give CO₂ and NO can proceed through different mechanisms. What rate law would be consistent for the following first step? 2 NO₂ $\rightarrow$ NO + NO₃

At moderate temperatures, the rate law for the reaction of NO₂ and CO to give CO₂ and NO follows the rate law shown below:rate = k [NO₂]² In which flask will the reaction be faster and how much faster?

Radioactive decay follows first-order kinetics. Some smoke detectors use the isotope ²⁴¹Am that has a half-life of 432.2 years. In how many years will 95% of the ²⁴¹Am have decayed?

Assume that the following first-order reaction has a rate constant k = 0.0137/min: SO₂Cl₂ $\rightarrow$ SO₂ + Cl₂ Given the initial [SO₂Cl₂] = 0.42 M, how many minutes will it take for [SO₂Cl₂] = 0.19 M?

The three reactions below, with identical reaction stoichiometry, must all share the same third order rate law found for the reaction of NO and O₂. True or False, and why? 2 NO(g) + O₂(g) $\rarr$ 2 NO₂(g)2 NO(g) + Cl₂(g) $\rarr$ 2 NOCl(g)2 NO(g) + F₂(g) $\rarr$ 2 NOF(g)