What is the unit of specific heat capacity?
a) Joules per kilogram per degree Celsius (J/kg°C)
b) Joules per kilogram (J/kg)
c) Watts per square meter (W/m²)
d) Newtons per square meter (N/m²)
What does the specific heat capacity of a substance depend on?
a) The mass of the substance
b) The temperature of the substance
c) The type of material
d) All of the above
Which of the following equations represents the relationship for specific heat capacity?
a) Q = mcΔT
b) Q = mvΔT
c) Q = mgh
d) Q = PΔt
In a calorimeter, what is measured to determine the heat absorbed or released?
a) Pressure
b) Mass
c) Temperature change
d) Volume
What is the heat required to raise the temperature of 1 kg of a substance by 1°C known as?
a) Latent heat
b) Specific heat capacity
c) Heat of fusion
d) Heat of vaporization
When a substance undergoes a phase change, which of the following remains constant?
a) Temperature
b) Pressure
c) Volume
d) Heat
What does the principle of calorimetry rely on?
a) Conservation of mass
b) Conservation of energy
c) Conservation of momentum
d) Law of reflection
If the temperature of a substance increases, what happens to the internal energy of the substance?
a) It decreases
b) It remains the same
c) It increases
d) It becomes zero
What is the specific heat capacity of water?
a) 1000 J/kg°C
b) 4200 J/kg°C
c) 2000 J/kg°C
d) 5000 J/kg°C
In a calorimeter, if a substance absorbs 500 J of heat and its temperature increases by 2°C, what is the mass of the substance?
a) 0.25 kg
b) 0.50 kg
c) 1.25 kg
d) 2.00 kg
Which of the following represents a substance with a high specific heat capacity?
a) Lead
b) Iron
c) Water
d) Copper
What does calorimetry measure?
a) Mass of a substance
b) Heat transfer during a chemical reaction or physical process
c) The density of a substance
d) The pressure of a substance
In a calorimeter, when the temperature increases, it indicates that the substance is: a) Losing heat
b) Absorbing heat
c) Freezing
d) Boiling
What is the heat required to change the temperature of a substance by 1 degree Celsius called?
a) Heat of vaporization
b) Specific heat capacity
c) Latent heat
d) Internal energy
Which of the following materials has the highest specific heat capacity?
a) Copper
b) Lead
c) Water
d) Iron
If 2 kg of water is heated and its temperature increases by 5°C, how much heat is required? (Specific heat of water = 4200 J/kg°C)
a) 4200 J
b) 42,000 J
c) 8400 J
d) 21000 J
When water changes from liquid to gas at its boiling point, what is the heat absorbed during the phase change called?
a) Latent heat of fusion
b) Latent heat of vaporization
c) Specific heat capacity
d) Specific latent heat
Which of the following is used to calculate the heat gained or lost by a substance?
a) ΔE = mcΔT
b) Q = mcΔT
c) Q = PΔV
d) Q = mgh
The heat of fusion is the heat required to change a substance from: a) Solid to gas
b) Liquid to gas
c) Solid to liquid
d) Liquid to solid
The unit of heat is: a) Joule
b) Newton
c) Watt
d) Pascal
Which method is used to measure the specific heat capacity of a solid material?
a) Calorimeter method
b) Latent heat method
c) Specific heat method
d) Calorimetry method
What is the heat required to melt a unit mass of a substance called?
a) Latent heat of fusion
b) Specific heat capacity
c) Latent heat of vaporization
d) Heat of combustion
Which of the following correctly defines the calorimeter?
a) A device to measure the temperature of an object
b) A device to measure the mass of an object
c) A device to measure the heat transfer in a process
d) A device to measure the pressure of gases
In calorimetry, what is the relationship between heat lost and heat gained?
a) Heat lost = Heat gained
b) Heat lost > Heat gained
c) Heat lost < Heat gained
d) Heat lost = Work done
Which of the following factors does NOT affect the specific heat capacity of a material?
a) Type of material
b) Temperature
c) Pressure
d) Mass
What is the specific heat capacity of lead?
a) 200 J/kg°C
b) 1300 J/kg°C
c) 0.16 J/g°C
d) 0.90 J/g°C
What happens to the temperature of a substance during a phase change?
a) It increases
b) It decreases
c) It remains constant
d) It becomes unpredictable
What does the principle of calorimetry assume about the system and surroundings?
a) The system loses energy and the surroundings gain it
b) The energy is neither created nor destroyed, only transferred
c) The energy is created in the system
d) There is no energy transfer between system and surroundings
