Question 1

Nitrogen dioxide, NO₂ will react with carbon monoxide, CO, to form nitric oxide, NO, and carbon dioxide, CO₂. A proposed mechanism is: 2NO₂ $\rarr$ NO₃ + NO NO₃ + CO $\rarr$ NO₂ + CO₂ Experiments indicate that the rate of the reaction is independent of the CO concentration. Identify the rate determining step and derive the rate law consistent with the mechanism and experimental observation.

Accepted Answer

Since rate is independent of CO concentration, the second step must be fast and the first slow; rate law is determined from the first step.

Question 2

A proposed mechanism for the following reaction, A₂ + B₂ $\rightarrow$ 2AB, isA₂ 2AA + B₂ $\rightarrow$AB + B slowB +A₂ $\rightarrow$AB + ADetermine the rate law.

Accepted Answer

The answer of A proposed mechanism for the following reaction,...

Question 3

The reaction of nitrogen dioxide and fluorine is:2 NO₂ + F₂ $\rightarrow$ 2 NO₂FOne proposed mechanism has two steps; the first step is rate determining: What is the experimentally determined rate law?

Accepted Answer

The answer of The reaction of nitrogen dioxide and fluorine...

Question 4

The rate law for the reaction2 H₂ (g) + 2 NO (g) $\rightarrow$ N₂ (g) + 2 H₂O (g)is rate = k[H₂ ][NO]². Which of the following mechanisms can be ruled out because the derived rate law is NOT consistent with the observed rate law?Mechanism 1H₂ + NO $\rightarrow$N + H₂O (slow)N + NO $\rightarrow$ N₂ + O (fast)O + H₂ $\rightarrow$H₂O (fast)Mechanism 2H₂ + 2 NO $\rightarrow$N₂O + H₂O (slow)N₂O + H₂ $\rightarrow$N₂ + H₂O (fast)Mechanism 32 NO N₂O₂ (fast equilibrium)N₂O₂+ H₂ $\rightarrow$ N₂O + H₂O (slow)N₂O + H₂ $\rightarrow$ N₂ + H₂O (fast)

Accepted Answer

The answer of The rate law for the reaction2 H₂...

Question 5

For the following reaction A + B $\rightarrow$ C + D, the rate law is determined to be Rate = k[A]²a) Of the five proposed mechanisms shown below, which is consistent with the experimentally determined rate law? 1. 2 A $\rightarrow$ Z (slow)2 B + Z $\rightarrow$ 2 C + 2 D (fast) 2. A + B $\rightarrow$ C + D (slow) 3. 2 B $\rightarrow$ N (slow)2 A + N $\rightarrow$ 2 C + 2 D (fast) 4. A $\rightarrow$ X (slow)B + X $\rightarrow$ C + D (fast) 5. B $\rightarrow$ M (slow)A + M $\rightarrow$ C + D (fast)b) Are there any intermediates in the mechanism you chose and if so what?

Accepted Answer

The answer of For the following reaction A + B...

Question 6

In the formation of dinitrogentetroxide, two NO₂ molecules react to make an N-N bond.2 NO₂ $\rightarrow$ 2 N₂O₄Draw molecular pictures superimposed on a diagram of energy vs. reaction coordinate that illustrates this process.

Accepted Answer

The answer of In the formation of dinitrogentetroxide, two NO₂...

Question 7

The following rate constants were obtained at the stated temperatures for the first-order reaction:A$\rightarrow$ B  Find the activation energy (in kJ/mole) for this reaction.

Accepted Answer

The answer of The following rate constants were obtained at...

Question 8

Nitrogen dioxide molecules undergo oxygen exchange with an activation energy of 100 kJ/mole. By how much will the reaction rate constant increase if temperature is increased from 25^oC to 75^oC?

Accepted Answer

The answer of Nitrogen dioxide molecules undergo oxygen exchange with...

Question 9

A particular first-order reaction is characterized by activation energy of 50 kJ/mole. At what temperature would the rate of the reaction be 10 times that at 298^oK?

Accepted Answer

Need to recognize that for first-order reaction 10 fold increase in rate results from a 10 fold increase in rate constant.

Question 10

The reaction of ozone with oxygen atoms to give oxygen has an activation energy of 17.1 kJ/mole with a rate constant at 298^oK, k = 4.8 x 10⁶ 1/M•s. Calculate the rate constant for this reaction at 315^oK.

Accepted Answer

The answer of The reaction of ozone with oxygen atoms...

Question 11

The reaction of ozone with oxygen atoms to produce molecular oxygen has a rate constant of 4.8x10⁶1/M s at 25^oC. A 20 degree increase in temperature results in a rate constant of 7.4x10⁶1/M s. What is the rate constant at 100^oC?

Accepted Answer

Two step problem: student must first determine the activation energy, then the rate constant at the new temperature.

Question 12

The activation energy for the high temperature conversion cyclopropane to propene is 270 kJ mol^-1. At what temperature would the rate constant for this reaction be ten times that of 500^oC?

Accepted Answer

The answer of The activation energy for the high temperature...

Question 13

The rate constant of the reaction, O (g) + N₂ (g) $\rightarrow$NO (g) + N (g), is 9.7 x 10¹⁰1/M•s at 800^oK and has an activation energy of 315 kJ/mole. What is the value of the rate constant at 700^oK?

Accepted Answer

The answer of The rate constant of the reaction, O...

Question 14

For a large number of reactions in organic chemistry, an increase in temperature 10°C over room temperature will double the rate. What activation energy does this correspond to?

Accepted Answer

The answer of For a large number of reactions in...

Question 15

For a hypothetical reaction, the activation energy is E_act = 50.2 kJ/mol and it has an Arrhenius constant of 22.3 M^-1s^-1. Determine what the rate constant would be if the temperature was 400$\degree$C.

Accepted Answer

The answer of For a hypothetical reaction, the activation energy...

Question 16

Consider the following energy-reaction coordinate diagram.  Give the names for the quantities indicated by A, B and C.

Accepted Answer

The answer of Consider the following energy-reaction coordinate diagram. ...

Question 17

Write the overall equation of reaction for the following mechanism and identify any reaction intermediates and any catalysts. H₂O₂ + I^-1 $\rightarrow$ H₂O + OI^-1 H₂O₂ + OI^-1 $\rightarrow$H₂O+ O₂ + I^-1

Accepted Answer

The answer of Write the overall equation of reaction for...

Quiz 13: Kinetics: Mechanisms and Rates of Reactions

In the formation of dinitrogentetroxide, two NO₂ molecules react to make an N-N bond.2 NO₂ $\rightarrow$ 2 N₂O₄Draw molecular pictures superimposed on a diagram of energy vs. reaction coordinate that illustrates this process.

Nitrogen dioxide molecules undergo oxygen exchange with an activation energy of 100 kJ/mole. By how much will the reaction rate constant increase if temperature is increased from 25^oC to 75^oC?

A particular first-order reaction is characterized by activation energy of 50 kJ/mole. At what temperature would the rate of the reaction be 10 times that at 298^oK?

The reaction of ozone with oxygen atoms to give oxygen has an activation energy of 17.1 kJ/mole with a rate constant at 298^oK, k = 4.8 x 10⁶ 1/M•s. Calculate the rate constant for this reaction at 315^oK.

The reaction of ozone with oxygen atoms to produce molecular oxygen has a rate constant of 4.8x10⁶1/M s at 25^oC. A 20 degree increase in temperature results in a rate constant of 7.4x10⁶1/M s. What is the rate constant at 100^oC?

The activation energy for the high temperature conversion cyclopropane to propene is 270 kJ mol^-1. At what temperature would the rate constant for this reaction be ten times that of 500^oC?

The rate constant of the reaction, O (g) + N₂ (g) $\rightarrow$ NO (g) + N (g), is 9.7 x 10¹⁰1/M•s at 800^oK and has an activation energy of 315 kJ/mole. What is the value of the rate constant at 700^oK?

For a large number of reactions in organic chemistry, an increase in temperature 10°C over room temperature will double the rate. What activation energy does this correspond to?

For a hypothetical reaction, the activation energy is E_act = 50.2 kJ/mol and it has an Arrhenius constant of 22.3 M^-1s^-1. Determine what the rate constant would be if the temperature was 400 $\degree$ C.

Consider the following energy-reaction coordinate diagram. Give the names for the quantities indicated by A, B and C.

Write the overall equation of reaction for the following mechanism and identify any reaction intermediates and any catalysts. H₂O₂ + I^-1 $\rightarrow$ H₂O + OI^-1 H₂O₂ + OI^-1 $\rightarrow$ H₂O+ O₂ + I^-1

Quiz 13: Kinetics: Mechanisms and Rates of Reactions

A proposed mechanism for the following reaction, A2 + B2 →\rightarrow→ 2AB, isA2 2AA + B2 →\rightarrow→ AB + B slowB +A2 →\rightarrow→ AB + ADetermine the rate law.

The reaction of nitrogen dioxide and fluorine is:2 NO2 + F2 →\rightarrow→ 2 NO2FOne proposed mechanism has two steps; the first step is rate determining: What is the experimentally determined rate law?

In the formation of dinitrogentetroxide, two NO2 molecules react to make an N-N bond.2 NO2 →\rightarrow→ 2 N2O4Draw molecular pictures superimposed on a diagram of energy vs. reaction coordinate that illustrates this process.

The following rate constants were obtained at the stated temperatures for the first-order reaction:A →\rightarrow→ B Find the activation energy (in kJ/mole) for this reaction.

Nitrogen dioxide molecules undergo oxygen exchange with an activation energy of 100 kJ/mole. By how much will the reaction rate constant increase if temperature is increased from 25oC to 75oC?

A particular first-order reaction is characterized by activation energy of 50 kJ/mole. At what temperature would the rate of the reaction be 10 times that at 298oK?

The reaction of ozone with oxygen atoms to give oxygen has an activation energy of 17.1 kJ/mole with a rate constant at 298oK, k = 4.8 x 106 1/M•s. Calculate the rate constant for this reaction at 315oK.

The reaction of ozone with oxygen atoms to produce molecular oxygen has a rate constant of 4.8x106 1/M s at 25oC. A 20 degree increase in temperature results in a rate constant of 7.4x106 1/M s. What is the rate constant at 100oC?

The activation energy for the high temperature conversion cyclopropane to propene is 270 kJ mol-1. At what temperature would the rate constant for this reaction be ten times that of 500oC?

The rate constant of the reaction, O (g) + N2 (g) →\rightarrow→ NO (g) + N (g), is 9.7 x 10101/M•s at 800oK and has an activation energy of 315 kJ/mole. What is the value of the rate constant at 700oK?

For a large number of reactions in organic chemistry, an increase in temperature 10°C over room temperature will double the rate. What activation energy does this correspond to?

For a hypothetical reaction, the activation energy is Eact = 50.2 kJ/mol and it has an Arrhenius constant of 22.3 M-1s-1. Determine what the rate constant would be if the temperature was 400 °\degree° C.

Consider the following energy-reaction coordinate diagram. Give the names for the quantities indicated by A, B and C.

Write the overall equation of reaction for the following mechanism and identify any reaction intermediates and any catalysts. H2O2 + I-1 →\rightarrow→ H2O + OI-1 H2O2 + OI-1 →\rightarrow→ H2O + O2 + I-1

In the formation of dinitrogentetroxide, two NO₂ molecules react to make an N-N bond.2 NO₂ $\rightarrow$ 2 N₂O₄Draw molecular pictures superimposed on a diagram of energy vs. reaction coordinate that illustrates this process.

Nitrogen dioxide molecules undergo oxygen exchange with an activation energy of 100 kJ/mole. By how much will the reaction rate constant increase if temperature is increased from 25^oC to 75^oC?

A particular first-order reaction is characterized by activation energy of 50 kJ/mole. At what temperature would the rate of the reaction be 10 times that at 298^oK?

The reaction of ozone with oxygen atoms to give oxygen has an activation energy of 17.1 kJ/mole with a rate constant at 298^oK, k = 4.8 x 10⁶ 1/M•s. Calculate the rate constant for this reaction at 315^oK.

The reaction of ozone with oxygen atoms to produce molecular oxygen has a rate constant of 4.8x10⁶1/M s at 25^oC. A 20 degree increase in temperature results in a rate constant of 7.4x10⁶1/M s. What is the rate constant at 100^oC?

The activation energy for the high temperature conversion cyclopropane to propene is 270 kJ mol^-1. At what temperature would the rate constant for this reaction be ten times that of 500^oC?

The rate constant of the reaction, O (g) + N₂ (g) $\rightarrow$ NO (g) + N (g), is 9.7 x 10¹⁰1/M•s at 800^oK and has an activation energy of 315 kJ/mole. What is the value of the rate constant at 700^oK?

For a hypothetical reaction, the activation energy is E_act = 50.2 kJ/mol and it has an Arrhenius constant of 22.3 M^-1s^-1. Determine what the rate constant would be if the temperature was 400 $\degree$ C.

Write the overall equation of reaction for the following mechanism and identify any reaction intermediates and any catalysts. H₂O₂ + I^-1 $\rightarrow$ H₂O + OI^-1 H₂O₂ + OI^-1 $\rightarrow$ H₂O+ O₂ + I^-1