factors affecting rate of reaction Archives - Page 2 of 2

How does the collision theory affect the rate of reaction?

Explaining the effect of size of a solid reactant/surface area on the rate of reaction using collision theory

When the size of a fixed mass of a solid reactant decreases, the rate of reaction increases.
This can be explained using the collision theory, as below:
(a) When the size of a fixed mass of a solid reactant becomes smaller, the total surface area exposed to collision with the particles of the other reactants increases, as shown in Figure.
(b) As a result, the frequency of collision among the reacting particles at the surface of the solid reactant increases.
(c) This causes the frequency of effective collision to increase.
(d) Hence, the rate of reaction increases.

Example: Two sets of experiments are carried out as shown below.
Set I: 1.0 g of granulated zinc is added to 20 cm³ of 0.5 mol dm^-3 sulphuric acid at 27.0°C.
Set II: 1.0 g of zinc powder is added to 20 cm³ of 0.5 mol dm^-3 sulphuric acid at 27.0°C.
The initial rate of liberation of hydrogen gas in set II is higher than that in set I. Explain the difference in the rate of reaction using the collision theory.
Solution:

Particle size of zinc powder in set II is smaller than that of granulated zinc in set I.
Thus, the total exposed surface area of 1.0 g of zinc powder in set II is larger than that of 1.0 g of granulated zinc in set I.
As a result, the frequency of collision between the hydrogen ions from sulphuric acid and the zinc atoms at the surface of zinc powder in set II is higher than that occurring at the surface of granulated zinc in set I.
This causes the frequency of effective collision between hydrogen ions and zinc atoms in set II to be higher than that in set I.
Hence, the initial rate of liberation of hydrogen gas in set II is higher than that in set I.

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Explaining the effect of concentration on the rate of reaction using collision theory

When the concentration of a reactant increases, the rate of reaction increases.
This can be explained using the collision theory, as below:
(a) When the concentration of the solution of a reactant increases, the number of particles per unit volume in this solution also increases.
(b) With more particles per unit volume, the frequency of collision among the reacting particles increases, as shown in Figure.
(c) Hence, the frequency of effective collision increases.
(d) As a result, the rate of reaction increases.

Example: Two experiments are carried out as shown below:

Experiment	Reacting conditions
I	50 cm³ of 0.20 mol dm^-3 sodium thiosulphate solution + 5 cm³ of 1.0 mol dm^-3 hydrochloric acid
II	50 cm³ of 0.12 mol dm³ sodium thiosulphate solution + 5 cm³ of 1.0 mol dm^-3 hydrochloric acid

(a) Which of the two experiments shows a higher rate of reaction?
(b) Explain the difference in (a) using collision theory.
Solution:

(a) Rate of reaction of Experiment I is higher than that of Experiment II

(b)

The concentration of sodium thiosulphate solution in Experiment I is higher than that in Experiment II.
So, the number of thiosulphate ions, S₂O₃^2- in one dm³of sodium thiosulphate solution in Experiment I is higher than that in Experiment II.
This causes the frequency of collision between the reacting particles (thiosulphate ions and hydrogen ions) in
Experiment I to be higher than that in Experiment II.
Hence, the frequency of effective collision in Experiment I is higher than that in Experiment II that results iii a higher rate of reaction in Experiment I.

Explaining the effect of pressure of gaseous reactants on the rate of reaction using collison theory

When the pressure of a reaction involving gaseous reactants increases, the rate of reaction increases.
This can be explained using the collision theory, as below:
(a) When particles of gaseous reactants are compressed to occupy a smaller volume, the pressure of the gaseous reactants increases, as shown in Figure.

(b) Thus, the number of gas particles per unit volume increases.
(c) With more gas particles per unit volume, the frequency of collision among the reacting particles increases.
(d) Hence, the frequency of effective collision increases, which results in a higher rate of reaction.

Explaining the effect of temperature on the rate of reaction using collision theory

When the temperature of a reaction increases, the rate of reaction increases.
This can be explained using the collision theory, as below.
(a) An increase in temperature will cause the kinetic energy of the reacting particles to increase.
(b) As a result, it leads to the following two changes:
(i) The reacting particles move faster and collide more often with one another. Hence, the frequency of collision increases, as shown in Figure.

(ii) The increase in kinetic energy causes more colliding particles to possess higher energy that is enough to overcome the activation energy.
(c) The above two changes result in a higher frequency of effective collision, and consequently a higher rate of reaction.

Example: Two sets of experiments are carried out as shown below.
Set X: 2 cm of magnesium ribbon is added to 50 cm³ of 1 mol dm^-3 sulphuric acid at room temperature.
Set Y: 2 cm of magnesium ribbon is added to 50 cm³ of 1 mol dm^-3 hot sulphuric acid at 80°C.
(a) Compare the time taken for the magnesium ribbon to disappear from sight for sets X and Y.
(b) Explain the difference in the time taken using the collision theory.
Solution:

The time taken in set Y is shorter than that in set X.
The temperature of reaction in set Y is higher than that in set X.
Thus, the kinetic energy of the hydrogen ions from the sulphuric acid that collide with the magnesium atoms at the surface of magnesium ribbon in set Y is higher than that in set X.
As a result, it leads to the following two changes:
(i) The hydrogen ions move faster and collide more often with the magnesium atoms in set Y compared to set X. The frequency of collision increases in set Y.
(ii) More collisions between hydrogen ions and magnesium atoms in set Y possess enough energy to overcome the activation energy compared to set X.
The above two changes result in a higher frequency of effective collision, and consequently a higher rate of reaction in set Y compared to set X.
Hence, the time taken for set Y is shorter than that in set X.

Explaining the effect of catalyst on the rate of reaction using collision theory

When a positive catalyst is used in a reaction, the rate of reaction increases.
This can be explained using the collision theory, as below:
(a) When a positive catalyst is used in a chemical reaction, it enables the reaction to occur through an alternative path which requires a lower activation energy, as illustrated in the energy profile diagrams in Figure.

(b) As a result, more colliding particles are able to overcome the lower activation energy.
(c) Hence, the frequency of effective collision increases, and consequently this results in a higher rate of reaction.

Example: Two sets of experiments are carried out as shown below.
Set Q: 2 g of granulated zinc is added to 50 cm³ of 0.2 mol dm^-3 hydrochloric acid at room conditions.
Set R: 2 g of granulated zinc is added to a mixture of 50 cm³ of 0.2 mol dm^-3 hydrochloric acid and 2 cm³ of 1 mol dm^-3 copper(II) sulphate solution at room conditions.
Explain why initial rate of set R is higher than that of set Q using the collision theory.
Solution:

Copper(II) sulphate solution in set R acts as a positive catalyst, whereas no catalyst is used in set Q.
The presence of copper(II) sulphate in set R enables the reaction between zinc and hydrogen ions from hydrochloric acid to occur through an alternative path which requires a lower activation energy.
As a result, more collisions between the hydrogen ions and zinc atoms at the surface of granulated zinc are able to overcome the lower activation energy in set R.
Hence, the frequency of effective collision increases. Consequently, this results in a higher rate of reaction for set R.

Appreciating scientist’s contributions

Scientists always practice problem-solving attitudes.
The patience, hard work and perseverance of scientists in doing their research and development had led to the discovery of the factors affecting the rate of reaction.
With this knowledge, we can control the rate of reaction in many activities in our daily life.
We must be thankful to those scientists for their contributions to improve the quality of life.

What is the collision theory in chemistry?

According to the kinetic theory of matter, particles of matter are in continuous motion and constantly in collision with each other.
For a reaction to occur, the particles of the reactants (atoms, molecules or ions) must touch each other through collision for bond breaking and bond formation to form the products.
However, not all collisions will result in a reaction to form the products.
According to the collision theory, only those collisions which
(a) achieve a minimum amount of energy, called activation energy, and
(b) with the correct orientation,
will result in reaction.
These types of collisions are known as effective collisions.
For particles that collide with energy less than the activation energy needed for reaction or with the wrong orientation, they simply bounce apart without reacting. These collisions are known as ineffective collisions.
An example to illustrate the collision theory
(a) (i) Hydrogen gas reacts with bromine gas to form hydrogen bromide gas
(ii) The chemical equation for the reaction is H₂(g) + Br₂(g) → 2HBr(g)
(b) Table illustrates three different situations that may happen during the collisions of hydrogen molecules with bromine molecules.

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Situations	Will it result in a reaction?
I. A hydrogen molecule and a bromine molecule collide with the correct orientation but the energy of the colliding particles is less than the activation energy, as shown in Figure.	This collision will not result in a reaction (Ineffective collision)
II. A hydrogen molecule and a bromine molecule collide with their total energy greater than or equal to the activation energy but with the wrong orientation, as shown in Figure.	This collision will not result in a reaction (Ineffective collision)
III. A hydrogen molecule and a bromine molecule collide with their total energy greater than or equal to the activation energy and with the correct orientation, as shown in Figure.	An effective collision occurs. This collision results in a reaction to form hydrogen bromide molecules.

What is Activation Energy?

Activation energy:

The meaning of activation energy can be visualised by sketching the energy profile diagrams, as shown in Figure.
The difference in energy between the energy of the reactants and the energy at the peak of the curve is the activation energy.
Activation energy is the energy barrier that must be overcome by the colliding particles of the reactants so that the reaction can occur.

What is the relationship between activation energy and collision theory?

Relationship between the frequency of collision and the activation energy with the rate of reaction:

According to the collision theory, the rate of a reaction is determined by the
(a) frequency of collision
(b) magnitude of activation energy
Frequency of collision
(a) If the frequency of collision for a reaction is high, then the frequency of effective collision that can result in a reaction is also high.
(b) Hence, the rate of reaction is high, and vice versa
(c) Figure illustrates this relationship.
Magnitude of activation energy
(a) The values of are different for different reactions.
(b) If the activation energy of a reaction is high, fewer number of colliding particles are able to achieve this high energy. Hence, the frequency of effective collision is low. As a result, the rate of reaction is low.
(c) Conversely, if the activation energy of a reaction is low, the rate of reaction is high.
The effect of the size of a solid reactant/surface area, concentration, pressure, temperature and catalyst on the rate of reaction can be explained using the collision theory.