1.1 rate of reaction
TRANSCRIPT
Chapter 1
Rate of Reaction
Chapter 1: Rate of ReactionChapter 1: Rate of Reaction1.1 Rate of Reaction
Which reaction is faster?
The meaning of rate of reactionThe meaning of rate of reaction
1 A chemical reaction takes place when reactants are mixed together under suitable conditions.
The meaning of rate of reactionThe meaning of rate of reaction
2 The speed of a chemical reaction
is called the rate of reaction.
The meaning of rate of reactionThe meaning of rate of reaction
3. The rate of reaction is inversely proportional to the time taken for the reaction to be completed.
The meaning of rate of reactionThe meaning of rate of reaction
3. The rate of reaction is inversely proportional to the time taken for the reaction to be completed.
Rate of reaction
The reaction is fast if it takes a short time to complete. Conversely, the reaction is
slow if it takes a long time for the reaction to complete.
takenTime
1
The meaning of rate of reactionThe meaning of rate of reaction
4 During a chemical reaction, the reactants are used up as the products are formed. Thus, the amounts of reactants decrease (Figure 1.1(a)) while the amounts of products increase as the reaction proceeds (Figure 1.1(b)).
The meaning of rate of reactionThe meaning of rate of reaction
5 Therefore, the rate of reaction can be determined in one of the following ways:
(a) the rate of disappearance of a reactant, or (b) the rate of formation of a product
The meaning of rate of reactionThe meaning of rate of reaction
6 (a) The rate of reaction can be defined as the amount of a reactant used up per unit time.
Rate of reaction = TakenTime
upusedtreacofAmount tan
The meaning of rate of reactionThe meaning of rate of reaction
6 (b) The rate of reaction can also be defined as the amount of a product obtained per unit time.
Rate of reaction =TakenTime
obtainedproductofAmount
The meaning of rate of reactionThe meaning of rate of reaction
7 Methods of measuring reaction rates (a) The amount of a reactant used up or a product
obtained can be measured in terms of the mass of the substance or the concentration of the substance.
The meaning of rate of reactionThe meaning of rate of reaction
7 Methods of measuring reaction rates (b) For chemical reactions that produce gases, the
rate of reactions can be measured as the volume of gas produced per unit time.
Rate of reaction =TakenTime
producedofVolume
The meaning of rate of reactionThe meaning of rate of reaction
8 Reaction between calcium carbonate and dilute hydrochloric acid.
(a) The reaction between calcium carbonate (marble chips) and dilute hydrochloric acid can be represented by the equation:
The meaning of rate of reactionThe meaning of rate of reaction
(b) During the reaction, the following observable changes take place.
(i) The mass of calcium carbonate (the reactant) decreases.
(ii) The concentration of hydrochloric acid (the reactant) decreases.
(iii) The volume of carbon dioxide (the product) produced increases.
The meaning of rate of reactionThe meaning of rate of reaction
(c) Thus, the rate of reaction between calcium carbonate and hydrochloric acid can be determined by measuring
(i) the decrease in mass of calcium carbonate per unit time, or
(ii) the increase in volume of carbon dioxide per
unit time.
The meaning of rate of reactionThe meaning of rate of reaction
9 (a) Besides changes in the mass of the reactants or the changes in the volume of the gaseous products, other changes that can be observed are as follows:
(i) changes in colour (ii) formation of precipitates
The meaning of rate of reactionThe meaning of rate of reaction
(b) Therefore, the time taken for the colour of a reactant to change or a certain amount of precipitate to form can be used to measure the rate of reaction.
The meaning of rate of reactionThe meaning of rate of reaction
10 The units used for the rate of reaction will depend on the changes measured.
For example (a) cm3 per unit time (second or minute) for a
gas evolved
The meaning of rate of reactionThe meaning of rate of reaction
10 The units used for the rate of reaction will depend on the changes measured.
For example (b) g per unit time or mol per unit time for a
solid reactant
The meaning of rate of reactionThe meaning of rate of reaction
10 The units used for the rate of reaction will depend on the changes measured.
For example (c) mol dm-3 per unit time for a reactant in
aqueous solution
The meaning of rate of reactionThe meaning of rate of reaction
11 Different chemical reactions take place at different rates. Some reactions occur very rapidly and some very slowly. Table 1.1 shows some examples of very fast reactions and very slow reactions.
The meaning of rate of reactionThe meaning of rate of reaction
Fast SlowCombustion RustingPrecipitation of silver chloride PhotosynthesisReaction between reactive metal and water
Fermentation
Measuring reaction ratesMeasuring reaction rates
1. The rate of reaction can be express in two ways:
(a) the average rate of reaction over a period of time, or
(b) the rate of reaction at any given time.
Measuring reaction ratesMeasuring reaction rates
2 The average rate of reaction is the average of the reaction rates over a given period of time. We can measure the average rate of reaction by measuring the change in amount (or
concentration) of a reactant or a product over a period of time.
Measuring reaction ratesMeasuring reaction rates
Example 1 A piece of magnesium ribbon weighing 0.1 g is
added to dilute hydrochloric acid. After 5 seconds, all the magnesium had dissolved. What is the average rate of reaction?
average rate of reaction=10.1
0.025
ggs
s
Measuring reaction ratesMeasuring reaction rates
Example 2 Calcium carbonate reacts with dilute hydrochloric
acid according to the equation: CaCO3(s) + 2HCl(aq) CaCl2(aq) + H2O(l) +
CO2(g) After 1.2 minutes, the volume of gas produced is
100 cm3. Calculate the average rate of reaction in the units of
(a) cm3 min-1, (b) cm3 s-1.
Measuring reaction ratesMeasuring reaction rates
Example 2Solution:
min83.3cm (min)2.1
)100(cm
takentime
produced CO of volume ratereaction average
13
3
2
Measuring reaction ratesMeasuring reaction rates
Example 2Solution:
takentime
producedCOofvolumerateAverage 2
133
39.172
100 scms
cm
Measuring reaction ratesMeasuring reaction rates
3 The rate of reaction at any given time is the actual rate of reaction at a given time. The reaction rate at any given time is also known as the instantaneous rate of reaction.
Measuring reaction ratesMeasuring reaction rates
4. The rate of reaction at a given time can
determined by measuring the gradient of the
graph mass of reactant against time (Figure1.2)
Measuring reaction ratesMeasuring reaction rates
Determining the gradient of the tangent time t: Rate of reaction at time t (gs-1) = Gradient of the graph
=
b
a
Solving numerical problems Solving numerical problems involving rate of reactioninvolving rate of reaction
Example 3: Hydrogen peroxide decomposes according to the
equation: 2H 2O2 (aq) 2H2O(l) + O2(g) The results of an experiment on the decomposition
of hydrogen peroxide are given below.
Calculate the rate of reaction at 40 seconds in the units of (a) cm3 s-1, (b) cm3 min -1.
Time(s) 0 15 30 45 60 90Volume of O2(cm3)
0 16 30 40 48 56
Solving numerical problems Solving numerical problems involving rate of reactioninvolving rate of reaction
Example 3: Solution (a) The rate of reaction at 40 s = Gradient at 40 s
1370.01858
2149
scmb
a
49
21
5818
Solving numerical problems Solving numerical problems involving rate of reactioninvolving rate of reaction
Example 4: Solution (b) time =
Rate in cm3 min-1
Rate of reaction in cm3 min-1
= min3
228 3cm
= 42cm3 min-1
(58 18) 40 2min min min
60 60 3
Measuring reaction ratesMeasuring reaction rates
5 Analysing a reaction rate curve: (a) The steeper the gradient, the faster the
rate of reaction.
Steeper
Measuring reaction ratesMeasuring reaction rates
5 Analysing a reaction rate curve:
(b) Figure 1.5 shows that the rate of reaction at t2,
is slower than the rate of reaction at t1. The
gradient at t2 is less steep than the gradient at t1. As the reaction proceeds, the curve becomes less steep because the rate of reaction decreases.
Measuring reaction ratesMeasuring reaction rates
6 Comparing reaction rates at a give time
Measuring reaction ratesMeasuring reaction rates
Activity: To find the reaction rates at (a) 90 s, (b)180 s a (c) the average rate of the reaction between zinc and dilute sulphuric
acid
Measuring reaction ratesMeasuring reaction rates
Apparatus: Conical flask, measuring cylinder, delivery
tube, burette, basin, retort stand, retort clamp and stopwatch.
Measuring reaction ratesMeasuring reaction rates
Materials: Granulated zinc and 0.3 mol dm-3 sulphuric acid.
Measuring reaction ratesMeasuring reaction rates
Procedure: 1 The burette is filled with water and inverted over a
basin of water.
Measuring reaction ratesMeasuring reaction rates
Procedure: 2 Using a measuring cylinder, 20.0 cm3 of 0.3 mol
dm-3 sulphuric acid is measured out and poured into a conical flask.
Measuring reaction ratesMeasuring reaction rates
Procedure: 3 5.0 g of granulated zinc are then added to the
sulphuric acid in the conical flask.
Measuring reaction ratesMeasuring reaction rates
Procedure: 4 The conical flask is then closed and the hydrogen
gas produced is collected in the burette by the displacement of water as shown in Figure 1.5.
Measuring reaction ratesMeasuring reaction rates
Procedure: 5 The stopwatch is started immediately. 6 The volume of hydrogen gas collected in the burette is
recorded at 30-second intervals.
Measuring reaction ratesMeasuring reaction rates
Results:
Measuring reaction ratesMeasuring reaction rates
Calculation: (a) The rate of reaction at 90 s
= slope at 90 s
XY
YZ
s
cm
)30180(
)2052( 3
s
cm
150
32 3
13213.0 scm
Measuring reaction ratesMeasuring reaction rates
Calculation: (b) The rate of reaction at 180 s = slope at 180 s
XY
YZ
s
cm
)18240(
)3048( 3
s
cm
222
18 3
13081.0 scm
Measuring reaction ratesMeasuring reaction rates
Calculation: (c) The average rate of reaction
13
2
157.0300
47
taken timetotal
produced H of volumetotal
scm
Measuring reaction ratesMeasuring reaction rates
Conclusion:
The rate of reaction decreases as the reaction proceeds.
Measuring reaction ratesMeasuring reaction rates
Activity: To measure the rate of reaction between calcium carbonate (CaCO3) and excess hydrochloric acid
Measuring reaction ratesMeasuring reaction rates
Apparatus: Conical flask, electronic balance, measuring
cylinder and stopwatch.
Measuring reaction ratesMeasuring reaction rates
Material: Calcium carbonate (CaCO3) pieces, 2.0 mol dm-3
hydrochloric acid and cotton wool.
Measuring reaction ratesMeasuring reaction rates
Procedure 1 Using a measuring cylinder, 50 cm3 of 2 mol dm-3
hydrochloric acid are measured out and poured in a dry conical flask. The mouth of the conical flask covered with some of cotton wool. The cotton wool is inserted into the mouth of the conical flak is prevent liquid from splashing out during the reaction.
Measuring reaction ratesMeasuring reaction rates
Procedure 2 The conical flask is placed on the electronic balance
as shown in Figure 1.6.
Measuring reaction ratesMeasuring reaction rates
Procedure 3 The mass of conical flask and its contents (calcium
carbonate, hydrochloric acid and cotton wool) is recorded.
Measuring reaction ratesMeasuring reaction rates
Procedure 4 The calcium carbonate is then transferred to the
hydrochloric acid in the conical flask and the stopwatch is started immediately.
Measuring reaction ratesMeasuring reaction rates
Procedure 5 The mass of the conical flask (and its contents) is
recorded at one-minute intervals.
Measuring reaction ratesMeasuring reaction rates
Results:
Time(s) 0 1 2 3 4 5 6 7 8Mass of conical flask + content(g)
60.0 59.1 58.3 57.9 57.4 57.0 56.8 56.5 56.3
Measuring reaction ratesMeasuring reaction rates
Based on the experimental results, a graph of the mass of conical flask and its contents against time is plotted (Figure 1.7)
Measuring reaction ratesMeasuring reaction rates
Calculation The average rate of reaction for the first minute. Decrease in mass = mass of carbon dioxide produced = (60.0-59.1) g = 0.9g Average rate of reaction for the first minute
12 min9.0min0.1
9.0
takentime
produced CO of mass gg
Time(s) 0 1 2 3 4 5 6 7 8Mass of conical flask + content(g)
60.0 59.1 58.3 57.9 57.4 57.0 56.8 56.5 56.3
Measuring reaction ratesMeasuring reaction rates
Calculation the average rate of reaction between 1.4 minutes and 2.2
minutes Rate of decrease in mass
1min625.04.12.2
3.588.58
g
Measuring reaction ratesMeasuring reaction rates
Calculation (c) The reaction rate at the 5th minute =Gradient of the graph at 5.0 minutes =
b
a
1min306.03.6
1.1Gradient
minutes6.34.30.71.14.565.57
g
bga
Measuring reaction ratesMeasuring reaction rates
Conclusion: The rate of reaction decreases as the reaction
proceeds. Finally, the reaction will stop when all the calcium carbonate added have reacted.
Solving numerical problems Solving numerical problems involving rate of reactioninvolving rate of reaction
Example 4: 3.0 g of excess marble (CaCO3) are added to 100 cm3 of
dilute hydrochloric acid. Figure 1.8 shows the graph of volume of carbon dioxide produced against time.
Solving numerical problems Solving numerical problems involving rate of reactioninvolving rate of reaction
Example 4: Calculate (a) the average rate of reaction (b) the concentration of hydrochloric acid in mol dm-3. (1 mole of any gas occupies 24 dm3 at room conditions).
Solving numerical problems Solving numerical problems involving rate of reactioninvolving rate of reaction
Example 4: Solution (a) Total volume of carbon dioxide evolved = 360 cm 3
Time taken = 8.0 minutes Average rate of reaction
= 13 min458
360 cm
Solving numerical problems Solving numerical problems involving rate of reactioninvolving rate of reaction
Example 4: Solution (b) Number of moles of CO2 evolved
CaCO3 + 2HCl CaCl2 + H2O + CO2
Mole ratio of HCl : CO2 =2: 1
mol015.0100024
360
Solving numerical problems Solving numerical problems involving rate of reactioninvolving rate of reaction
Example 4: Solution (b) According to the equation, number of moles of
hydrochloric acid used
CaCO3 + 2HCl CaCl2 + H2O + CO2
2 moles HCl produces 1 mol CO2
? moles HCl produces 0.015 mol CO2
= 2 x 0.015 = 0.03 mole
Solving numerical problems Solving numerical problems involving rate of reactioninvolving rate of reaction
Example 4: Solution (b) According to the equation, number of moles of
hydrochloric acid used = 2 x 0.015 = 0.03 mole
Concentration of hydrochloric acid, M
3
3
3.01.0
03.0
)dmin volume(
moles ofnumber
moldm
MVN V
NM
V = 100 cm3 =0.1 dm3