WorksheetsThermal properties
Total questions: 25
Worksheet time: 50mins
The specific heat of platinum is 0.133 J/g°C. How much heat (∆E) is released when a 10 g piece of platinum cools from 100°C to 50°C?
66.5 J
665 J
0.0266 J
0.665 J
20 g of water. specific heat of water is 4.18 J/g°C. temperature changes from 25° C to 20° C, how much heat energy (∆E) moves from the water to the surroundings?
418 J
209 J
83 J
4.18 J
The SI units J/kg°C measures
Specific heat capacity
mass
temperature
heat energy
Define Specific Latent Heat of Fusion
is the amount of thermal energy required to change one kilograms of the substance from liquid state to gaseous state or vice versa, without a change in temperature
is the amount of thermal energy required to change one kilograms of the substance from solid state to liquid state or vice versa, without a change in temperature
is the amount of thermal energy required to change one kilograms of the substance from liquid state to gaseous state or vice versa by one Kelvin or one degree celcius
is the amount of thermal energy required to change the substance of any of any mass from liquid state to solid state or vice versa, without a change in temperature
State what occurs during freezing/condensation?
Internal Kinetic Energy remains constant, Internal Potential Energy decreases
Internal Kinetic Energy remains decreases, Internal Potential Energy decreases
Internal Kinetic Energy remains constant, Internal Potential Energy remains constant
Internal Kinetic Energy remains constant, Internal Potential Energy increases
What is heat capacity ?
The amount of thermal energy required to raise the temperature of a substance by 1K or 1°C
The amount of thermal energy required to raise the temperature of a 1kg mass of substance by 1K or 1°C
The amount of thermal energy required to change a substance from liquid state to gaseous state without a change in temperature
The amount of thermal energy required to change 1kg of the substance from liquid state to gaseous state, without a change in temperature
What is the formula to calculate heat energy required to raise the temperature of any substance?
∆E=mc∆t
∆E=mc
∆E= ½mv
m=∆EC
What is the formula to calculate specific latent heat of vaporisation?
L = ∆E/m
c = ∆E/(mΔƟ)
∆E = mcΔƟ
∆E = m/L
The graph shows the cooling curve of a substance. At which stages the specific latent heat released?
AB and CD
BC and DE
AB and EF
BC and CD
Amount of energy required to increase temperature
Which statement about evaporation is correct?
Evaporation causes the temperature of the remaining liquid to decrease.
Evaporation does not occur from a cold liquid near its freezing point.
Evaporation does not occur from a dense liquid, such as mercury
Evaporation occurs from all parts of a liquid.
The same quantity of thermal energy is supplied to two solid objects X and Y. The temperature increase of object X is greater than the temperature increase of object Y. Which statement explains this?
X has a lower melting point than Y.
X has a lower density than Y.
X has a lower thermal capacity than Y.
X is a better thermal conductor than Y.
Which statement describes what happens as ice at 0°C starts to melt to become water?
Energy is absorbed and the temperature remains constant.
Energy is absorbed and the temperature rises.
Energy is released and the temperature remains constant.
Energy is released and the temperature rises.
State three differences between boiling and evaporation
1) Temperature remains constant during boiling but decreases during evaporation
2) Evaporation does not occur at boiling point of liquid.
3) Evaporation only occurs on the surface while boiling occurs throughout the liquid
1) Evaporation occurs at any temperature while boiling occurs at fixed temperatures
2) Evaporation is a much slower process than boiling
3) Boiling causes air bubbles to appear and form on the surface but evaporation does not
1) Boiling causes air bubbles to appear and form on the surface but evaporation does not
2) Evaporation occurs at any temperature while boiling occurs at fixed temperatures
3) Evaporation is not a change of state, boiling is the change of state from liquid to gaseous state.
1) Evaporation does not require a gain in thermal energy for particles to evaporate.
2) Evaporation occurs at any temperature while boiling occurs at fixed temperatures
3) Boiling causes air bubbles to appear and form on the surface but evaporation does not
State what occurs during boiling/melting?
Internal Kinetic Energy increases, Internal Potential Energy decreases
Internal Kinetic Energy remains constant, Internal Potential Energy remains constant
Internal Kinetic Energy remains constant, Internal Potential Energy decreases
Internal Kinetic Energy remains constant, Internal Potential Energy increases
As temperature increases, what are the changes in internal energy?
Internal Kinetic Energy increases, Internal Potential Energy remains constant
Internal Kinetic Energy increases, Internal Potential Energy decreases
Internal Kinetic Energy increases, Internal Potential Energy increases
Internal Kinetic Energy decreases, Internal Potential Energy remains constant
A piece of solid ice at -20 degree celcius is melted and boiled off completely.
Given : Mass of Ice : 500g
Specific Heat capacity of ice : 420 J/kg°C
Specific Latent heat of fusion of ice : 500 J/kg
Specific Heat capacity of water : 4200 J/kg°C
Specific Latent heat of vaporisation of water : 600 J/kg
What is the thermal energy required?
21475 J
2147500 J
214750 J
0.00000021475 J
Jimmy got another piece of solid ice at 0°C and he heated it on a pan until it was boiled off.
Given : Mass of Ice : 500g
Specific Heat capacity of ice : 420 J/kg°C
Specific Latent heat of fusion of ice : 500 J/kg
Specific Heat capacity of water : 4200 J/kg°C
Specific Latent heat of vaporisation of water : 600 J/kg
Power of Heater : 1000 W
How much time is needed to boil the ice off?
Assume no energy is lost to surroundings or gained from heater.
211 seconds (3 s.f)
21.1 seconds (3 s.f)
9.23 seconds (3 s.f)
54.5 seconds (3 s.f)
What is heat capacity ?
The amount of thermal energy required to raise the temperature of a substance by 1K or 1°C
The amount of thermal energy required to raise the temperature of a 1kg mass of substance by 1K or 1°C
The amount of thermal energy required to change a substance from liquid state to gaseous state without a change in temperature
The amount of thermal energy required to change 1kg of the substance from liquid state to gaseous state, without a change in temperature
How does evaporation help cool down objects?
1.Water molecules in the liquid move randomly and vary in kinetic energy, velocity and temperature.
2.More energetic water molecules at the surface gains thermal energy from the surroundings to overcome forces of attraction/break bonds between molecules and overcome atmospheric pressure.
3.Energetic water molecules escape into atmosphere as water vapour
4.Leaving less energetic water molecules behind,average kinetic energy of water decreases, average velocities decreases and reduces temp.
1.Water molecules in the liquid move randomly and vary in kinetic energy, velocity and temperature.
2.More energetic water molecules at the surface gains thermal energy from the surroundings to overcome forces of attraction/break bonds between molecules.
3.Leaving less energetic water molecules behind, kinetic energy of water decreases, velocities decreases and reduces temp.
