Topic 6: The Rate and Extent of Chemical Change

Question 1

How is rate of reaction calculated? (2 variations)

Answer 1

1. Rate of reaction = amount (e.g. grams, cm3) of reactant used or product formed/time
2. Rate of reaction (mol/s) = Moles of reactant used or product formed time

Question 2

What are the various units for rate of reaction?

Answer 2

• Can include g/s or cm3/s or mol/s
• Generally, mass/time, volume/time, moles/time

Question 3

Name three common ways of measuring rate of reaction

Answer 3

• Loss in mass of reactants
• Volume of gas produced
• Time for a solution to become opaque

Question 4

Describe measuring the rate by monitoring mass loss

Answer 4

• 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 5

Describe measuring the rate by monitoring the volume of a gas

Answer 5

• 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 6

Describe measuring the rate by monitoring the disappearance of a cross

Answer 6

• 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 7

How to find a rate of reaction at some time, t, from a graph of amount of reactant vs time?

Answer 7

• Pick a point corresponding to the time t, and find the tangent to the curve at this point.
• The tangent is the gradient of this graph - it tells you how fast the reaction proceeds at this point.
• The steeper the tangent line, the faster the rate.
• Gradient of tangent can be expressed in change in y values over change in x values.

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

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 other

Question 11

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

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

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 (slows down) the reaction.

Question 13

Describe and explain the effect of increasing surface area

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?

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

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

Answer 19

• Changing the concentration of reactants or products disrupts equilibrium; system adjusts to restore it.
• Increasing reactant concentration leads to more products forming until equilibrium is restored.
• Decreasing product concentration causes more reactants to react until equilibrium is restored.

Question 20

Describe the effect of changing temperature on the position of the equilibrium

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

Answer 21

• Applies to equilibria involving gases.
• Increase in pressure shifts equilibrium to side with fewer molecules (per symbol equation).
• Decrease in pressure shifts equilibrium to side with more molecules (per symbol equation).
• No effect on equilibrium if the number of gas molecules is equal on both sides.

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.

Question 23

What is a closed system?

Answer 23

A closed system is where a chemical reaction happens (for e.g. in a container) where none of the reactants or products can escape.

So in summary:

CLOSED SYSTEM:
-all energy stays
-all reactants stays
-all products stays