Rate of reactions. (Chapter 2)

Сентябрь 6, 2022

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Rate of reactions. (Chapter 2)

Содержание

2. Chapter 2 1. Meaning and Measurement of Rate Lets have closer look to the reaction below.
3. Chapter 2 1. Meaning and Measurement of Rate
4. Chapter 2 1. Meaning and Measurement of Rate Example 1 Find the rate relationship of reactants
5. The decomposition of dinitrogen pentoxide can be represented by the equation; 2N2O5 → 4NO2 + O2
6. RateN2O5 = (0.008 – 0.004)/20 = 0.0002 = 2.10−4 mol/L. s
7. Chapter 2 1. Meaning and Measurement of Rate Example 2 In the following decomposition reaction, 2N2O5
8. Chapter 2 1. Meaning and Measurement of Rate Solution rate NO2 production = 4 × (9.1
9. Chapter 2 3. Rate Expression and Rate Constant Consider the one step following reaction; mA +
10. Chapter 2 3. Rate Expression and Rate Constant Example 10 Write the possible rate expression of
11. Chapter 2 3. Rate Expression and Rate Constant Example 11 Write the rate expression of the
12. Temperature The increase in temperature increases rate of reaction. And rate can be calculated by the
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Слайд 2

Chapter 2
1. Meaning and Measurement of Rate
Lets have closer look to

the reaction below.

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Chapter 2
1. Meaning and Measurement of Rate

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Chapter 2
1. Meaning and Measurement of Rate
Example 1
Find the rate relationship

of reactants and products for the given reaction.
N2(g) + 3H2(g) → 2NH3(g)

Solution

Слайд 5

The decomposition of dinitrogen pentoxide can be represented by the

equation;
2N2O5 → 4NO2 + O2
The concentration of dinitrogen pentoxide decreases from 0,008 M to 0,004 M in 20 seconds. Find the average rate of consumption of dinitrogen pentoxide

Слайд 6

RateN2O5 = (0.008 – 0.004)/20 = 0.0002 = 2.10−4 mol/L. s

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Chapter 2
1. Meaning and Measurement of Rate
Example 2
In the following decomposition

reaction,
2N2O5 → 4NO2 + O2
oxygen gas is produced at the average rate of 9.1 × 10-4 mol · L-1· s-1. Over the same period, what is the average rate of the following:
the production of nitrogen dioxide.
the loss of nitrogen pentoxide.

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Chapter 2
1. Meaning and Measurement of Rate
Solution
rate NO2 production = 4

× (9.1 × 10-4 mol · L-1· s-1)
= 3.6 × 10-3 mol · L-1· s-1
rate loss of N2O5 = 2× (9.1 × 10-4 mol · L-1· s-1)
= 1.8 × 10-3 mol · L-1· s-1

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Chapter 2
3. Rate Expression and Rate Constant
Consider the one step following

reaction;
mA + nB → products
The rate expression is proportional to the product of [A] (to some power m) and [B] (to some power n). To create an equation instead of a proportion, use the rate constant k.
Rate = k[A]m[B]n
m and n are order of reaction with respect to related substance, and k depends only on temperature and activation energy.
Solids and liquids are not included in the expression, only gaseous and aqueous ions are indicated in the rate expression.

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Chapter 2
3. Rate Expression and Rate Constant
Example 10
Write the possible rate

expression of the following reactions.
Cl2(g) + H2(g) → 2HCl(g)
Fe(s) + Cl2(g) → FeCl3(g)
Fe2O3 (s) + 3H2SO4 (aq) → Fe2(SO4)3 (s) + 3H2O(l)
Ca(s) + 2Ag+(aq) → 2Ca+2 (aq) + Ag(s)

Solution

Rate = k[Cl2][H2]
Rate = k[Cl2]

Rate = k[H2SO4]3
Rate = k[Ag+]2

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Chapter 2
3. Rate Expression and Rate Constant
Example 11
Write the rate expression

of the following one step reaction, determine the order of reaction in terms of N2 and H2, and overall order.
N2(g) + 3H2(g) → 2NH3(g)

Solution

Rate = k[N2][H2]3
Order in terms of N2 is 1 and 3 in terms of H2
Overall order is 1+3 = 4

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Temperature
The increase in temperature increases rate of reaction. And rate

can be calculated by the formula below.
Vt2= Vt1.γ (t2 - t1)/10 γ is a constant and given in the question.
Vt1 = velocity at initial temperature,
Vt2 = velocity at final temperature