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Rates of Reaction 2
Check out questions 3 and 4 to see what bumper cars and chemistry have in common!

Rates of Reaction 2

Many factors can increase or decrease rates of chemical reactions - pressure of gases, temperature, surface area of solids, concentration and if there is a catalyst. Anything that will change the probability of particles colliding or change the energy of the collisions will affect the rate of a reaction. This is the second of three GCSE Chemistry quizzes looking at these factors.

Rates of reaction measure the speed at which the reactants change into the products during a chemical reaction. Manufacturers rely on producing large amounts of product quickly, in order for their process to be economically viable. There are a number of factors that need to be taken into consideration and often compromises need to be made. An example of one of these compromises is the temperature - lower temperatures decrease the rate of reaction and higher ones increase it.. If a manufacturer increases the temperature of a chemical reaction, more product will be made in a shorter time but the energy costs will be higher. This energy needs to be generated somehow, if it comes from burning a fuel, it also means more pollutants will be sent into the air. A good understanding of how reactions can be speeded up or controlled is vital to ensure that the best compromises are reached.

Collisions of particles cause reactions. At all temperatures above absolute zero, particles are in motion (the kinetic theory). Therefore, when the particles of two reacting substances are mixed, it is very likely that they will collide with each other. Solids mixed together don't normally react as their particles are fixed in place, however, introduce a gas or liquid and collisions will occur because the particles are free to move around.

If the particles are slow moving, they have less energy, collisions between them will therefore also involve less energy than if they were moving quickly. If particles collide head-on, that will involve more energy than if one collides with the other from behind or if they collide from the side or at an angle. This means that not all collisions between particles will lead to a chemical reaction. If there are high concentrations of particles, there will be more collisions per second which means there will be a greater likelihood of collisions that result in a reaction.

When you studied exothermic and endothermic reactions and energy level diagrams, you will have learnt that for a chemical reaction to happen, bonds between atoms must first be broken and then they can re-form. There is also a minimum level of energy required for a reaction, the activation energy. This represents the energy that is required to break the bonds of the original reactants when they collide. Putting together the two ideas of collisions between particles and bond breaking/making gives an understanding of rates of reaction.

Have a go at this quiz and see how well you understand how rates of reaction can be increased or decreased.

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1.
Increasing the temperature of the reactants in a chemical reaction increases the rate of the chemical reaction. This is because...
particles collide less often, but they have more energy
particles collide more often and they collide with less energy
particles collide more often and they collide with more energy
particles collide less often with less energy
The higher the temperature, the more energy they have and the faster they move
2.
Around room temperature, if we increase the temperature of a reaction by 10°C, the rate of the reaction will approximately...
halve
triple
stay the same
double
It is just an approximation but for most reactions, it is not far wrong
3.
Why does increasing the concentration of reactants increase the rate of a reaction?
If the concentration of reactants is increased, there are more particles available to react
If the concentration of reactants is increased, the particles have more energy
If the concentration of reactants is increased, there are fewer particles available to react
If the concentration of reactants is increased, the particles are at the right angle to collide
Imagine bumper cars at the fair. The more cars there are, the more likely they are to 'bump' into each other
4.
How does increasing the pressure increase the rate of a chemical reaction?
If the pressure is increased, the particles are further away from each other
If the pressure is increased, the particles are moving faster
If the pressure is increased, the particles have more energy
If the pressure is increased, the particles are closer together
Imagine again the bumper cars. If the bumper cars are closer together, they are more likely to collide. Increasing the pressure of a gas is the equivalent of increasing the concentration of a reaction taking place in the liquid state
5.
A catalyst speeds up a chemical reaction by...
reducing the amount of energy required by the particles to react
increasing the amount of energy required by the particles to react
increasing the pressure of the reactants
increasing the temperature of the reactants
If the activation energy is lower, in any given system, more particles will have sufficient energy to react
6.
If the surface area of a solid reactant is increased, why is the rate of reaction increased?
There are fewer particles on the surface of the solid available to react
There are more particles on the surface of the solid available to react
The particles are moving more quickly
The particles have more energy
This is why powders react faster than lumps of chemical
7.
Scientists have developed catalysts that enable reactions to take place at lower temperatures. Why is this advantageous to the manufacturer and the environment?
It is cheaper for the manufacturer because less fuel is needed to provide the high temperatures
It is better for the environment because there is less fuel being burnt and so less carbon dioxide being emitted
It is better for the manufacturer because catalysts are cheap to buy
It is better for the environment because the catalyst does not harm the environment
It is better for the manufacturer because the catalyst can be reused
It is better for the environment because there are more toxic gases being released
It is better for the manufacturer because the catalyst is often very expensive
It is better for the environment because there are fewer toxic emissions
More product can be made in less time, using less energy and producing less pollution - a winning situation for everyone
8.
Chemical reactions eventually stop. What is the usual reason for this?
Reactants run out
Catalyst runs out
Particles have used up all their energy
Products have taken the particles' energy
Reactions become slower and slower as they proceed because there are fewer and fewer particles to collide. When one or the other (or even both) of the reactants are used up, the reaction stops. We say it has reached completion
9.
Why can icing sugar cause an explosion but sugar lumps can't?
The icing sugar has more energy
The icing sugar has more particles
The icing sugar has a larger surface area
The sugar lumps have more energy
These types of explosion are known as powder explosions and can happen in places where fine powders are being handled. Care must be taken that there are no naked flames or sparks
10.
Some chemical reactions may take place twice as quickly if their temperature is raised by 10°C. If a particular reaction takes 32 minutes at 20°C, how long will it take if the temperature is raised to 60°C?
2 minutes
4 minutes
6 minutes
8 minutes
At 20°C = 32 mins, at 30°C = 16 mins, at 40°C = 8 mins, at 50°C = 4 mins, at 60°C = 2 mins

 

Author:  Kate Gardiner

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