P6 - Particles and Matter

Question 1

Describe the structure of a solid according to the Kinetic theory of matter:

Answer 1

The particles are in a fixed shape and vibrate around a fixed position. Therefore, a solid cannot flow and keeps the same volume.

Question 2

Describe the structure of a liquid according to the Kinetic theory of matter:

Answer 2

The particles in a liquid are close together but not fixed in positon. The particles can move around but stay close together. Therefore, a liquid can flow and takes the shape of a container. A liquid keeps the same volume and cannot be compressed.

Question 3

Describe the structure of a gas according to the Kinetic theory of matter:

Answer 3

The particles are far apart and move around very fast. As a result of the particles being far apart, gases can be compressed and expanded to fill a container. Gases can flow.

Question 4

How can you change the physical state of a substance? What are the names of the 6 changes of state?

Answer 4

By heating or cooling the substance.

• Solid to Liquid = Melting
• Liquid to Gas = Vapourising or Boiling
• Gas to Liquid = Condensation
• Liquid to Solid = Freezing/ Solidification
• Solid to Gas = Sublimation
• Gas to Solid = Desublimation

Question 5

When a substance changes state, why does its mass stay the same?

Answer 5

Because the number of particles stays the same.

Question 6

What happens to particles in any state when the temperature is increased?

Answer 6

The particles move faster - gain kinetic energy.

Question 7

Why do the particles of a substance have different energy amounts when it’s in a solid, liquid or gas state?

Answer 7

For a given amount of a substance, its particles will always have more energy in the gas state than in the liquid state, and they have more energy in the liquid state than in the solid state.

Question 8

What is the temperature at which a solid changes to a liquid called?

Answer 8

Melting point

Question 9

What is the temperature at which a liquid turns into a gas called?

Answer 9

Boiling point

Question 10

What is Density?

Answer 10

The amount of mass in a set volume.

Question 11

What is the equation for Density?

Answer 11

Density = mass / volume

*p=m/v

(g/cm^3)=g/ cm^3 OR kg/cm^3

*p= rho-greek letter for density

Question 12

What is Archimides’ Principle?

Answer 12

When an object is submerged in a body of water, the volume of the water displaced is the same as the volume of the object displacing it.

Question 13

What is the aim of RP5 - Density?

Answer 13

To carry out a number of density tests to calculate the density of objects my weighing the object and calculating its volume.
A body of water was used to calculate the volume of irregular shaped objects.
(Archimides’ Principle).

Question 14

What did you find in terms of the relationship between density and whether an object will sink or float?

Answer 14

An object should float if its density is less than 1g/сm^3.

Question 15

What happens in terms of tempearture as pure ice is melted?

Answer 15

Its temperature will stay at 0°C until ALL the ice has melted.

Question 16

What is the rule for a pure substance’s temperature when undergoing a change of state?

Answer 16

For a pure substance undergoing a change of state, its temperature stays the same while the change is taking place.

Question 17

What is the temperature at which a liquid changes to a solid called?

Answer 17

The Freezing Point

Question 18

What is the relationship between melting point and freezing point? Why?

Answer 18

They are the same. Because it is the same transition of matter either way.

Question 19

What is the relationship between boiling point and condensation point? Why?

Answer 19

They are the same. Because it is the same transition of matter either way.

Question 20

How do impurities within solids and liquids impact changes of state?

Answer 20

The MP of a solid AND the BP of a liquid can be affected by impurities in the substance.

E.g Melting point (and therefore freezing point) of water is lowered if you add salt to the water. This is why salt is added to the grit that’s used for grititing roads in freezing weather - it means roads don’t get icy until they are colder, as ice / frost is prevented from forming.

Question 21

Explain what would happen to a beaker of ice below 0°C that is steadily heated to melt the ice and then boil the water. Describe how it would look on a temp vs time graph.

Answer 21

The temperature of the ice increases until it reaches 0°C. The ice starts to melt and the temperature stays constant untill all the ice has melted.
The temperature then increases to 100°C when the water starts to boil. The water stays at 100°C until all the water is boiled (if it is continued to be heated).

Graph:

Diagonal, then a flat line for MP. Then another diagonal, then another flat line for ВР.

Question 22

What is Latent Heat and Specific Latent Heat?

Answer 22

Latent Heat is the energy transferred to a substance when it changes state.
Specific Latent Heat is the energy required to change the state of 1kg of a material, without changing its temperature.

Question 23

What is the difference between Specific Latent Heat and Specific Heat Capacity?

Answer 23

Specific Heat capacity is the energy required for a particular temperature change, without a change of state.
Specific Latent Heat is the energy required for a particular change in state, without a temperature change.

Question 24

How many specific latent heats does a material have and why?

Answer 24

Every material has 2 specific latent heats as there are 2 boundaries - solid/liquid and liquid/gas.

Question 25

What are the 2 specific latent heats?

Answer 25

The 2 specific latent heats are: 1) Latent Heat of fusion U/kg) - the amount of energy needed to melt or freeze the material at its melting point (same as freezing point). 2) Latent Heat of vaporisation /kg) - the amount of energy needed to boil or condense the material at its boiling point (same as condensation point).

Question 26

What is the equation, involving specific latent heat, used to calculate the amount of energy stored/released as the temperature of a system changes?

Answer 26

Change in Thermal Energy = mass x specific latent heat E= m x L (J) = (kg) × J/kg)

Question 27

What are the similarities & differences between boiling and evaporation?

Answer 27

Both evaporation and boiling are processes where a liquid changes into a gas. • Boiling happens to all of a liquid at once when a liquid is heated to its boiling point - the temperature where a liquid becomes a gas (or vice versa). • Evaporation can happen in a liquid at any temperature below the boiling point of the liquid. It can only happen to particles at the surface of a liquid.

Question 28

What is Internal Energy?

Answer 28

The energy stored by the particles of a substance.

Question 29

What is the internal energy of a substance the sum of?

Answer 29

Internal Energy = Kinetic Energy + Potential Energy

Question 30

What does internal energy not include?

Answer 30

It does not include the kinetic energy caused by the motion of the whole substance or the gravitational potential energy of the susbtance (how high up it iS).

Question 31

How does the internal energy of a substance change when it is heated?

Answer 31

The Internal energy of a substance increases when it is heated as the energy of the particles increases. This is because either: -The temperature of the substance increases OR -Its physical state changes (if it is heated enough).

Question 32

When energy is given to raise the temperature, particles gain what type of energy and why?

Answer 32

They gain Kinetic Energy. They gain kinetic energy as heating causes the particles to speed up and move faster. This energy, i.e the energy needed to change the temperature of a substance by 1°C, without changing its state, can be calculated by E = mcAt (specific heat capacity equation).

Question 33

When the substance changes state (melts or boils) what energy do particles gain and why?

Answer 33

They gain Potential Energy This is because the particles have gained energy through breaking away from their structure. The energy needed to change a substances state is called latent heat and can be calculated by E = mL.

Question 34

Why does the potential energy of a substance change when a substance is changing state, but the kinetic energy does not?

Answer 34

The kinetic energy stays the same because the temperature stays the same when a substance changes state. The particles do not gain speed when they are changing state.

Question 35

Exam Question: What happens to both Potential Energy and Kinetic Energy when a substance is: i) freezing ii) vaporising

Answer 35

i) Potential energy decreases, as particles are getting closer together (liquid to solid). Kinetic energy stays the same. ii) Potential energy increases, as particles are getting further apart. Kinetic energy stays the same.

Question 36

How does a cooling curve show changes in internal energy?

Answer 36

Cooling Curve = Time (x-axis) vs Temp (y-axis) -Looks a bit like a stair case. 1) Diagonal line (substance is a solid), kinetic energy is increasing as is the temperature of the particles. 2) Flat line (melting point), potential energy increases as the substance moves from solid to liquid. The kinetic energy stays the same and there is no change in temperature. 3) Diagonal line (substance is liquid), kinetic energy increases as the liquid is heated to a higher temperature. 4) Flat line (boiling point), the potential energy increases as the substance moves from liquid to gas. The kinetic energy stays the same as does the temperature. 5) Diagonal line (substance is a gas), the kinetic energy of the particles is increasing as the temperature increases. This can be reversed: Gas to Liquid (condensation) - potential energy decreases as particles moving closer together. Kinetic energy stays the same as does the temperature. Liquid to Solid (freezing) - potential energy decreases as particles moving closer together. Kinetic energy stays the same as does the temperature.

Question 37

How are the forces of attraction in a solid?

Answer 37

There are strong forces of attraction between these particles. These forces bond the particles in fixed positions. When a solid melts (or sublimates), its because its particles have gained enough energy to break away from the structure.

Question 38

How are the forces of attraction in a liquid?

Answer 38

They are weaker than in a solid. When a liquid is heated, some of its particles gain enough energy to break away from other particles. These molecules are in a gas state above the liquid.

Question 39

What is Brownian motion?

Answer 39

The random movements of particles in a fluid (liquid or gas), as observed by Robert Brown in 1785. You can observe Brownian Motion using smoke. The smoke particles move about randomly due to random impacts that the air (gas) particles make on each smoke particle.

Question 40

Why does increasing the temperature of any sealed gas can increase the pressure? Essentially, why does pressure increase when temperature is increased.

Answer 40

Because: -Energy transferred to the gas when it's heated increases the energy of its particles. This increases the kinetic energy which means there will be more frequent collisions between the gas particles and the internal surface (walls) of the container. The can will probably EXPLODE due to the fact that there will be millions of tiny particles smashing the walls of the container simultaneously. P = F / A (solid & gases) P= hpg (liquids)

Question 41

Why will a heated can with a little bit of water in it suddenly implode when dunked upside down in cold water?

Answer 41

It IMPLODES because the hot gas water molecules (reason why you put water in the can) are cooled rapidly which dramatically decreases the pressure in the can, causing the external pressure to be much greater than the internal pressure. The can collapses / IMPLODES.

Question 42

What is the relationship between temperature and pressure?

Answer 42

The relationship is directly proportional as long as the volume stays the same (is constant).

Question 43

What is Boyle's Law about Pressure and Volume?

Answer 43

Pressure x Volume = Constant P× V = constant (as long as the temperatue remains the same). P1 (Initial Pressure) × V1 (Initial Volume) = P2 (Final Pressure) × (Final Volume) V2 P1V1 = P2V2 What this means is that the relationship between volume and pressure of a gas is inversely proportional (y=1/x). As volume decreases, pressure increases and vice versa.

Question 44

What would a graph look like with pressure vs volume?

Answer 44

As the relationship is inversely proportional, it would be a curve. As volume (x-axis) increases, pressure (y-axis) decreases - and vice verca.

Question 45

If you were asked to calculate the final pressure of something what would you do?

Answer 45

Because P1V1 = P2V2, If you know P1, V1 and V2: P2 = P1 x V1 / V2 Essentially just re-arrange the formula.

Question 46

What is the equation for temperature and pressure calculation?

Answer 46

P1 / T1 = P2 / T2 So e.g, Initial Pressure = Final Pressure x Initial Temperature / Final Temperature

Question 47

According to Boyle's Law, pressure and volume are inversely proportional. But what is the particle theory behind this?

Answer 47

If the volume of gas at a fixed temperature is reduced: • the space the molecules move in is smaller. • Collide with container inner surface more so the total force of the impacts per m^2 is greater.

Question 48

How can the temperature of a gas be increased by reducing the volume?

Answer 48

If a gas is rapidly compressed, work is done on it, therefore energy isn't transferred quick enough to the surroundings. The temperature of the gas increases.