Rate Of Chemical Reaction

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The Rate of a Chemical Reaction

  
The rate of a chemical reaction can be defined as the amount of the reaction which occurs in unit time. The rate of a reaction is measured by choosing certain properties of the reaction which will indicate how far the reaction has gone, and whose magnitude can be observed with time without disturbing the reaction.

For example, a reaction which shows color change: the rate of such reaction can be measured by observing how the intensity of color formed changes with time. In a similar way, a reaction which involves gases can have its rate measured by collecting the gas and observing the way its volume or mass increases with time. Note: increase in rate of reaction corresponds to decrease in time taken for the reaction, and vice versa.

I.e., rate of reaction is inversely proportional to time,

R α1/T

Factors which affect the Rate of Chemical Reactions

Factors which can affect the rate of a chemical reaction include:

1. Temperature

By the kinetic theory, chemical reactions occur due to collisions of Molecules, atoms or ions involved in the reaction. When the temperature of a reacting system is increased by way of heating, the reacting particles gain energy and are able to move faster, resulting in increased collisions, which increases the rate of the reaction.

An illustration of this can be found in the reaction between sodium trioxo sulphur sulphate(VI) solution and hydrochloric acid. The reaction leads to the Precipitation of sulphur.

By observing the precipitation of sulphur at various temperatures with time, the result obtainable would indicate that: as the temperature of the reaction is increased, the time taken to precipitate sulphur is decreased (i.e. rate of reaction increases).

Note: the way by which the intensity of the precipitate can be measured is to carry out the entire reaction in a beaker, and by placing the beaker and its contents on a white piece of paper with a cross marked on it. The time for the disappearance of the cross when the contents of the beaker are viewed from above will give a measure of the time taken for a certain fraction of the reaction to occur (i.e. the rate of the reaction) – a stop clock or a watch is used to note this time.

By plotting the graph of temperature over time of reaction, we obtain the curve:

Note: the curve slopes from left to right indicating that increase in temperature leads to decrease in time (i.e., increase in rate of reaction) and vice versa. Thus, temperature is inversely proportional to time (Temp α 1/Time).

In general, increase in temperature of a reaction by 100 results in doubly the rate of reaction (i.e. decrease in time taken by half).

2. Concentration of Reactants

The concentration or density of reacting substances affect their closeness to one another, and consequently the frequency of their collision – this ultimately affects the rate of reaction. The higher the concentration of reactants, the greater the rate of reaction and vice-versa.

To investigate the effect of concentration on the rate of reaction, the reaction between dilute HCl and sodium trioxo sulphur sulphate (VI) solution to precipitate sulphur may be studied.

By observing the reactions of different concentrations of sodium trioxo sulphur sulphate(VI) with fixed concentration of HCl, it would be observed, from the result of the reaction that the higher the concentration, the shorter will be the time taken for sulphur to precipitate, i.e., the higher the concentration, the greater the rate of reaction.

To observe the intensity of sulphur produced at any given moment (this represents the extent of the reaction, i.e. the rate of the reaction), the reaction is carried out in a beaker, placed on a piece of paper with a cross marked on it. The time taken for the cross to be invisible when the content of the beaker is viewed from above is noted using a stop clock or a watch – this is the time taken for a certain fraction of the reaction to occur.

By plotting the graph of concentration against time of reaction, the following curve is obtained:

The curve indicates concentration varying inversely with time, i.e., conc. α 1/T. Hence, increasing the concentration of reacting masses leads to decrease in time of reaction (i.e. increase in rate of reaction). Decreasing the concentration of reacting masses leads to increase in the time of reaction (i.e. decrease in rate of reaction).

Another study to show the effect of concentration of reactants on the rate of reaction is “the iodine-clock reaction” – this is the reaction between hydrogen peroxide solution and acidified potassium iodide solution. Iodine is produced and is indicated by the observation of a dark-blue coloration with starch.

2I^–(aq),+ 2H⁺(aq) + H₂O₂(aq) → 2H₂O (l) + I₂(aq)

The procedure is to use a fixed concentration of one reactant together with a variable concentration of the other, and to observe the rate of reaction in each combination.

The result of the study would show that the rate of reaction increases with increase in concentration of the reactants. For gaseous reactions, increase of pressure implies increase of concentration – the rate of the reaction tends to increase as a result of increase in collisions.

Note: generally, increase in the concentration (in moles per dm³ or mmHg for gases) of reactants will result in increase in rate of reaction – i.e. decrease in reaction time – and vice versa. The graph above applies to all similar cases.

3. Surface Area of Reactants

In heterogeneous reactions – reactions in which all the reactants are not in the same phase (i.e. different states) – the surface area of the reactants have been found to affect the rate of the reactions. For example, comparing the rate of reactions of:

(i) Dilute HCl and marble chips.

(ii) Dilute HCl and powdered marble of the same mass as

(i). CaCO₃(s) + 2HCl(aq → CaCl₂(aq) + CO₂(s) + H₂O

(l) Both reactions produce CO₂ gas. This causes a reduction in the mass of the reacting vessel with time, and this may be taken as a measure of the rate of the reaction.

The result of both reactions would show that the rate of reaction of the powdered marble is greater than that of the chip (as shown in the graph below – the mass of the reacting vessel of the powdered marble reduces at shorter time than the mass of the reacting vessel of the lump of marble).

The reason for this is that the surface area of the powdered marble, being very large compared with that of the chip is responsible for the difference in their reaction rates.

The graph of the mass of reacting vessel against time of reaction is similar to the diagram below:

Note: The two curves level off at the same point. The reason for this is that the chip (or large piece) completely dissolves after some time, then the rate of its reaction becomes equal to that of the powdered one.

In general, for heterogeneous reactions, reactants of large surface areas have greater rates of reaction (i.e., reactions occur at shorter time) than reactants of small surface areas. The surface area of powder is greater than that of lumps or large piece.

Another way the rates of the above reactions can be measured is to measure their increasing volume of CO₂ produced with time. The graph of volume of CO₂ produced against time will give:

4. The Use of Catalyst

The presence of catalysts in chemical reactions would increase their rate.

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The rate of a chemical reaction is the speed at which the reactants are converted into products. It is usually measured as the change in concentration of one of the reactants or products per unit time.

The rate law is an equation that expresses the relationship between the rate of a reaction and the concentrations of the reactants. The order of a reaction is the power to which the concentration of each reactant is raised in the rate law.

The rate constant is a constant that appears in the rate law and is characteristic of the reaction. It is a measure of the frequency with which collisions between reactant molecules result in a reaction.

The temperature dependence of reaction rate is a consequence of the fact that the rate of a reaction is proportional to the frequency of collisions between reactant molecules. As the temperature increases, the Average kinetic energy of the molecules increases, and the frequency of collisions increases. This results in an increase in the rate of reaction.

The concentration dependence of reaction rate is a consequence of the fact that the rate of a reaction is proportional to the concentration of the reactants. As the concentration of the reactants increases, the Probability of a collision between reactant molecules increases, and the rate of reaction increases.

The effect of catalysts on reaction rate is a consequence of the fact that catalysts provide an alternative pathway for the reaction that has a lower activation energy. This results in an increase in the rate of the reaction.

Elementary reactions are reactions that occur in a single step. They are the simplest type of reaction and are often used to model more complex reactions.

Complex reactions are reactions that occur in multiple steps. They are more difficult to study than elementary reactions, but they can be understood by breaking them down into a series of elementary reactions.

Chain reactions are reactions that are initiated by a single event and then propagate through a series of steps. They are often used in industrial processes, such as the production of ammonia.

Photochemical reactions are reactions that are initiated by Light. They are important in many biological processes, such as Photosynthesis.

Biochemical reactions are reactions that occur in living organisms. They are essential for life and are responsible for many of the processes that take place in the body.

Combustion reactions are reactions that occur between a fuel and Oxygen. They are exothermic reactions, which means that they release heat. Combustion reactions are used in many industrial processes, such as the production of electricity.

Nuclear reactions are reactions that involve the nucleus of an atom. They are often very energetic and can release large amounts of energy. Nuclear reactions are used in nuclear power Plants and nuclear weapons.

The rate of a chemical reaction is a complex phenomenon that is influenced by many factors. The rate law, order of reaction, rate constant, temperature dependence of reaction rate, concentration dependence of reaction rate, effect of catalysts on reaction rate, elementary reactions, complex reactions, chain reactions, photochemical reactions, biochemical reactions, combustion reactions, and nuclear reactions are all important concepts that can be used to understand and predict the rate of a chemical reaction.

What is a chemical reaction?

A chemical reaction is a process that changes one or more substances into new substances.

What are the different types of chemical reactions?

There are many different types of chemical reactions, but some of the most common include:

• Synthesis reactions: These reactions combine two or more substances to form a new substance.
• Decomposition reactions: These reactions break down a substance into two or more simpler substances.
• Single replacement reactions: These reactions replace one element in a compound with another element.
• Double replacement reactions: These reactions exchange ions between two compounds.
• Combustion reactions: These reactions combine a substance with oxygen to produce heat and light.

What are the factors that affect the rate of a chemical reaction?

The rate of a chemical reaction can be affected by many factors, including:

• The concentration of the reactants: The higher the concentration of the reactants, the faster the reaction will occur.
• The temperature: The higher the temperature, the faster the reaction will occur.
• The presence of a catalyst: A catalyst is a substance that speeds up the rate of a reaction without being consumed by the reaction.
• The surface area of the reactants: The larger the surface area of the reactants, the faster the reaction will occur.
• The nature of the reactants: The type of reactants can also affect the rate of the reaction.

What are some examples of chemical reactions?

Some examples of chemical reactions include:

• The burning of wood: This is a combustion reaction that produces heat and light.
• The rusting of iron: This is a decomposition reaction that forms iron oxide.
• The digestion of food: This is a series of chemical reactions that break down food into smaller molecules that can be absorbed by the body.
• The photosynthesis of plants: This is a process that uses sunlight to convert carbon dioxide and water into glucose and oxygen.

What are some applications of chemical reactions?

Chemical reactions are used in a wide variety of applications, including:

• The production of energy: Chemical reactions are used to produce electricity, heat, and light.
• The manufacture of products: Chemical reactions are used to make products such as plastics, pharmaceuticals, and Fertilizers.
• The treatment of waste: Chemical reactions are used to treat wastewater and other types of waste.
• The cleaning of the Environment: Chemical reactions are used to clean up pollution and other environmental problems.

What are some safety precautions that should be taken when working with chemical reactions?

When working with chemical reactions, it is important to take the following safety precautions:

• Always wear safety goggles and gloves when handling chemicals.
• Never mix chemicals unless you are sure of the reaction that will occur.
• Always work in a well-ventilated area.
• Be aware of the potential hazards of the chemicals you are working with.
• Have a plan in place in case of an accident.

1. The rate of a chemical reaction is affected by the following factors except:
   (A) Temperature
   (B) Concentration
   (C) Pressure
   (D) Catalyst

2. The rate of a chemical reaction is measured in terms of:
   (A) The amount of product formed per unit time
   (B) The amount of reactant consumed per unit time
   (C) The rate of change of concentration of reactant or product
   (D) All of the above

3. The rate of a chemical reaction can be increased by:
   (A) Increasing the temperature
   (B) Increasing the concentration of reactants
   (C) Using a catalyst
   (D) All of the above

4. The rate of a chemical reaction is inversely proportional to the square of the distance between reactant molecules. This is known as:
   (A) The collision theory
   (B) The activation energy
   (C) The rate law
   (D) The equilibrium constant

5. The activation energy is the minimum amount of energy required for reactant molecules to collide and react. It is represented by the symbol $E_a$.
   (A) True
   (B) False

6. The rate of a chemical reaction is affected by the activation energy. The higher the activation energy, the slower the reaction.
   (A) True
   (B) False

7. A catalyst is a substance that increases the rate of a chemical reaction without being consumed in the reaction.
   (A) True
   (B) False

8. A catalyst works by providing an alternative pathway for the reaction that has a lower activation energy.
   (A) True
   (B) False

9. The rate of a chemical reaction is affected by the concentration of reactants. The higher the concentration of reactants, the faster the reaction.
   (A) True
   (B) False

10. The rate of a chemical reaction is affected by the temperature. The higher the temperature, the faster the reaction.
    (A) True
    (B) False