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Collision Theory & Reaction Mechanism: Gr12 Chem Unit 4 Kinetics: Lesson 5 - Rate Determining Step

The document discusses a reaction mechanism involving nitrogen monoxide and hydrogen gas. It provides the steps of the reaction mechanism and asks to determine the overall balanced equation and identify any reaction intermediates. It also asks about why most molecular collisions do not lead to reactions and how a manager would assign work to employees in a fast food restaurant based on the time taken for different steps.

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Atulya Bharadwaj
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89 views2 pages

Collision Theory & Reaction Mechanism: Gr12 Chem Unit 4 Kinetics: Lesson 5 - Rate Determining Step

The document discusses a reaction mechanism involving nitrogen monoxide and hydrogen gas. It provides the steps of the reaction mechanism and asks to determine the overall balanced equation and identify any reaction intermediates. It also asks about why most molecular collisions do not lead to reactions and how a manager would assign work to employees in a fast food restaurant based on the time taken for different steps.

Uploaded by

Atulya Bharadwaj
Copyright
© © All Rights Reserved
We take content rights seriously. If you suspect this is your content, claim it here.
Available Formats
Download as DOCX, PDF, TXT or read online on Scribd
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Gr12 Chem Unit 4 Kinetics: Lesson 5_Rate Determining Step

Collision Theory & Reaction Mechanism

1. Nitrogen monoxide reacts with hydrogen gas to produce nitrogen gas and water vapour. The mechanism is
believed to be:

Step 1: 2 NO → N2O2

Step 2: N2O2 + H2 → N2O + H2O

Step 3: N2O + H2 → N2 + H2O

For this reaction find the following:

the overall balanced equation

any reaction intermediates

2. Give two reasons why most molecular collisions do not lead to a reaction.

3. An important function for managers is to determine the rate-determining steps in their business processes. In
a certain fast-food restaurant, it takes 3 minutes to cook the food, 1.5 minutes to wrap the food, and 5
minutes to take the order and make change. How would a good manager assign the work to four employees?
Gr12 Chem Unit 4 Kinetics: Lesson 5_Rate Determining Step

Collision Theory & Reaction Mechanism Answers


1. Nitrogen monoxide reacts with hydrogen gas to produce nitrogen gas and water vapour. The mechanism is
believed to be:

Step 1: 2 NO → N2O2

Step 2: N2O2 + H2 → N2O + H2O

Step 3: N2O + H2 → N2 + H2O

For this reaction find the following:

the overall balanced equation

any reaction intermediates

Solution

To find the overall balanced equation, cross out substances that appear in equal numbers on both sides of
the reaction and add together like items on the same side of the equation:

Step 1: 2 NO → N2O2

Step 2: N2O2 + H2 → N2O + H2O

Step 3: N2O + H2 → N2 + H2O

Net Reaction: 2 NO + 2 H2 → N2 + 2 H2O

To identify the reaction intermediates, look for substances that first appear on the product side of the
equation, but then appear in the next step as a reactant. In this example there are two reaction
intermediates - N2O2 and N2O.

2. Give two reasons why most molecular collisions do not lead to a reaction.

Solution:

The collision may not have: 1) the correct orientation or 2) the necessary energy.

3. An important function for managers is to determine the rate-determining steps in their business processes. In
a certain fast-food restaurant, it takes 3 minutes to cook the food, 1.5 minutes to wrap the food, and 5
minutes to take the order and make change. How would a good manager assign the work to four employees?

Solution:

Assign two workers to take the orders, since that is the rate determining step.

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