P2-Topic 6- The rate and extent of chemical change

Question 1

How is rate of reaction

calculated?

Answer 1

amount (grams, cm3) of reactant used or product formed/time

(mol/s) = Moles of reactant used or product formed
time

Question 2

simplified equation for the rate of equation

Answer 2

time taken

time taken

Question 3

What are the various units for rate of reaction?

Answer 3

g/s or cm3/s or mol/s

Generally, mass/time, volume/time,moles/time

Question 4

Name three common ways of measuring rate of reaction

Answer 4

Loss in mass of reactants

• Volume of gas produced
• Time for a solution to become opaque

Question 5

Describe measuring the rate by monitoring mass loss 3

Answer 5

Place the reaction flask on a balance.

In these reactions (e.g. metal carbonate +
acid) a gas is given off, so record the decrease in mass in time intervals (note
hydrogen is too light).

Plot a graph of mass vs time.

Question 6

Describe measuring the rate by monitoring the volume of a gas 2

Answer 6

Connect a gas syringe to a reaction flask and measure the volume of a gas formed in time intervals.

Plot a graph of volume vs time.

Question 7

Describe measuring the rate by monitoring the disappearance of a cross
3

Answer 7

Take a piece of paper and mark a cross (X) on it.

Put the reaction flask on this cross.

Mix the reagents, and measure how long it takes for a cloudy mixture to
conceal a cross.

Question 8

State five factors affecting the rate of a chemical reaction

Answer 8

• Concentration of reactants
• Pressure of gases (volume)
• Surface area
• Temperature
• Catalysts

Question 9

What is the collision theory?

Answer 9

Chemical reactions can occur only when reacting particles collide with each other
with sufficient energy (more than or equal to activation energy).

Question 10

Describe and explain the effect of increasing temperature on the rate of reaction 2

Answer 10

T increases = faster reaction
As T increases, kinetic energy of particles increases, i.e. more energetic collisions

Also, they move faster, so they collide more frequently

However, there is no straight line relationship between rate and temperature,
i.e. they are not directly proportional to each othe

Question 11

Describe and explain the effect of increasing concentration on the rate of reaction 2

Answer 11

Conc. increases = faster reaction,

More reactants = more frequent collisions

Question 12

Describe and explain the effect of increasing pressure of a gas on the rate of reaction
2

Answer 12

Increasing the pressure of reacting gases, is the same as increasing concentration.

It increases the number of gas molecules in the same volume and so increases the frequency of collisions and therefore increases the rate of reaction.

Note that volume and pressure are inversely
proportional to each other.
Increasing the volume retards the reaction.

Question 13

Describe and explain the effect of increasing surface

area 2

Answer 13

If solid reactants are in smaller pieces, they have a greater surface area

Increasing the surface area of solid reactants increases the frequency of collisions
and so increases the rate of reaction, e.g. block of magnesium reacts slower with
acid then magnesium powder.

Question 14

What is a catalyst and how does it work? How

does it affect the reaction profile? 2

Answer 14

A catalyst changes the rate of reaction but is not used up.

It increases rate of reaction by providing a different pathway for the reaction that has a lower
activation energy.

The reaction profile for a catalysed reaction will have a lower maximum of the curve (lower activation energy).

Question 15

What is an enzyme?

Answer 15

An enzyme is a molecule that acts as a catalyst in a biological system

Question 16

What is a reversible reaction?

Answer 16

A reversible reaction occurs when the products of a reaction can react backwards
to produce the original reactants

Question 17

When is dynamic equilibrium reached?

Answer 17

In a closed system, when the forward and reverse reactions occur at the same rate
and the concentrations of reactants and products remain constant.

Question 18

Describe Le Chatelier’s Principle 2

Answer 18

If a system is at equilibrium and a change is made to any of the conditions, then
the system responds to counteract change and restore the equilibrium.

Question 19

Describe the effect of changing the concentration of

reactant and product on the position of the equilibrium 3

Answer 19

If the concentration of one of the reactants or products is changed, the system is no longer at equilibrium and the concentrations of all the substances will change until equilibrium is reached again.

If the concentration of a reactant is increased,
more products will be formed until equilibrium is reached again.

If the concentration of a product is decreased, more reactants will react until equilibrium
is reached again.

Question 20

Describe the effect of changing temperature on the

position of the equilibrium 3

Answer 20

If the temperature of a system at equilibrium is increased:
• the relative amount of products at equilibrium increases for an endothermic reaction
• the relative amount of products at equilibrium decreases for an exothermic
reaction.

Question 21

Describe the effect of changing pressure on the position of the equilibrium 4

Answer 21

This applies to equilibria that involve gases

An increase in pressure causes the equilibrium position to shift towards the side with the smaller number of molecules as shown by the symbol equation for that reaction.

A decrease in pressure causes the equilibrium position to shift towards the side with the larger number of molecules as shown by the symbol equation for that reaction.

Pressure has no effect on the reactions where the numbers of as molecules are equal on both sides of the equation.

Question 22

Describe the effect of a catalyst on the position of the equilibrium

Answer 22

No effect.
It just speeds up both forward and backward reactions equally.
i.e. equilibrium is achieved faster.