WorksheetsThermal Energy Quiz
Total questions: 85
Worksheet time: 43mins
Which chapter of the learning material focuses on the laws that govern thermal energy?
Chapter Ten
Chapter Eleven
Chapter Twelve
Chapter Nine
What is the main subject of Chapter Eleven in the provided material?
Electromagnetism
Thermodynamics
Optics
Quantum Mechanics
What is the process called when work is converted into heat and vice versa?
Radiation
Thermodynamics
Conduction
Magnetism
According to the introduction, what happens when you rub your palms together in winter?
You feel colder
You feel warmer
Nothing happens
Your palms get wet
What did Benjamin Thomson’s experiment in 1798 demonstrate about heat?
Heat is produced only by sharp drills
Heat is a form of energy and not a fluid
Heat cannot boil water
Heat is produced by cold objects
Which of the following is NOT a topic listed in the contents of Chapter Eleven?
Thermal equilibrium
Carnot engine
Quantum tunneling
Specific heat capacity
What is the modern view of heat according to the introduction?
Heat is a fluid
Heat is a form of energy
Heat is a type of light
Heat is a magnetic force
What does the experiment by Benjamin Thomson suggest about the conversion of energy?
Energy cannot be converted from one form to another
Energy can be converted from work to heat
Energy is only present in fluids
Energy conversion is impossible
Which of the following is NOT a macroscopic variable used in thermodynamic description of a gas?
Pressure
Volume
Temperature
Molecular distribution of velocities
In thermodynamics, what is meant by the equilibrium state of a system?
The system is moving at a constant speed
The macroscopic variables do not change with time
The system is undergoing chemical reactions
The system is being heated continuously
What is the main difference between an adiabatic wall and a diathermic wall as shown in the diagram?
Adiabatic wall allows heat flow, diathermic wall does not
Both walls allow heat flow
Adiabatic wall does not allow heat flow, diathermic wall allows heat flow
Both walls are insulating
Which of the following statements best describes the focus of thermodynamics in mechanics?
It is concerned with the motion of the system as a whole
It is concerned with the internal macroscopic state of the body
It is concerned with the molecular structure of the system
It is concerned with the chemical composition of the system
Which of the following is a measure of disorder in a thermodynamic system?
Pressure
Volume
Entropy
Enthalpy
Suppose two gases A and B are separated by a diathermic wall. What will eventually happen?
The gases will remain at different temperatures
Thermal equilibrium will be attained
The gases will mix completely
The pressure will decrease in both containers
What is the function of an adiabatic wall in thermodynamics?
It allows energy flow between systems.
It insulates systems, preventing energy (heat) flow.
It increases the temperature of the system.
It conducts electricity between systems.
Which type of wall allows energy (heat) to flow from one system to another?
Adiabatic wall
Diathermic wall
Insulating wall
Reflective wall
According to the Zeroth Law of Thermodynamics, if system A is in thermal equilibrium with system C, and system B is also in thermal equilibrium with system C, what can be concluded about systems A and B?
They are not related in any way.
They are in thermal equilibrium with each other.
They must have different temperatures.
They cannot be in equilibrium with each other.
What is the thermodynamic variable whose value is equal for two systems in thermal equilibrium?
Pressure
Volume
Temperature
Density
Suppose two gases are separated by an adiabatic wall and then the wall is replaced by a diathermic wall. What happens to the macroscopic variables of the systems?
They remain unchanged.
They change until both systems reach equilibrium.
They decrease to zero.
They increase indefinitely.
What does the diagram illustrate about the process of achieving thermal equilibrium?
Only one system can reach equilibrium at a time.
Systems in contact via a conducting wall can reach thermal equilibrium.
Adiabatic walls always prevent equilibrium.
Thermal equilibrium is independent of wall type.
What does the Zeroth Law of Thermodynamics help us understand?
The concept of temperature and direction of heat flow
The concept of pressure in gases
The concept of volume in liquids
The concept of chemical reactions
When does the flow of heat between two bodies stop?
When the bodies are at different temperatures
When the bodies are in thermal equilibrium
When the bodies are moving
When the bodies are in a vacuum
Which of the following is NOT included in the internal energy of a system?
Kinetic energy due to random motion of molecules
Potential energy of molecules
Kinetic energy of the system as a whole moving with velocity
Vibrational energy of molecules
Internal energy of a system is an example of which type of thermodynamic variable?
State variable
Path variable
Control variable
External variable
Which variables describe the state of a gas for determining its internal energy?
Pressure, volume, and temperature
Mass, density, and color
Shape, size, and texture
Speed, direction, and altitude
Why does the internal energy of a system not depend on the path taken to arrive at a state?
Because it is a state variable
Because it is a path variable
Because it is a control variable
Because it is an external variable
In Fig. 11.3, what type of energy is NOT included in the internal energy U when the box is moving as a whole?
Kinetic energy due to random motion of molecules
Rotational energy of molecules
Vibrational energy of molecules
Kinetic energy of the box as a whole
What distinguishes heat transfer from work transfer in thermodynamics?
Heat transfer is due to temperature difference; work transfer is not
Heat transfer is due to pressure difference; work transfer is not
Heat transfer is due to volume change; work transfer is not
Heat transfer is due to chemical reaction; work transfer is not
Which of the following is NOT a way to change the internal energy of a gas in a cylinder with a movable piston?
Putting the cylinder in contact with a hotter body
Pushing the piston down to do work on the system
Placing the cylinder in a vacuum
Allowing heat to flow from the gas to the surroundings
According to the First Law of Thermodynamics, which equation correctly represents the relationship between heat supplied, work done, and change in internal energy?
ΔQ = ΔU + ΔW
ΔQ = ΔU - ΔW
ΔQ = ΔU × ΔW
ΔQ = ΔU / ΔW
What is the main distinction between heat and work in thermodynamics?
Heat and work are both state variables
Heat and work are modes of energy transfer to a system
Heat and work are both forms of internal energy
Heat and work are always path independent
If a system is taken through a process in which ΔU = 0, what does the First Law of Thermodynamics imply?
ΔQ = ΔU
ΔQ = ΔW
ΔQ = 0
ΔQ = ΔU + ΔW
Why is it incorrect to say "a gas in a given state has a certain amount of heat"?
Because heat is a state variable
Because heat is not a state variable
Because heat is the same as internal energy
Because heat is always zero
Which of the following combinations is path independent according to the First Law of Thermodynamics?
ΔQ + ΔW
ΔQ - ΔW
ΔU + ΔQ
ΔU - ΔW
What is the formula for work done by a system against a constant pressure?
W = P + V
W = P/V
W = P × V
W = PΔV
Which equation represents the change in internal energy for 1 g of water when it goes from liquid to vapour phase at atmospheric pressure?
ΔU = ΔQ + PΔV
ΔU = ΔQ - PΔV
ΔU = ΔQ × PΔV
ΔU = ΔQ / PΔV
What is the unit of specific heat capacity?
J kg⁻¹ K⁻¹
J mol⁻¹ K⁻¹
J K⁻¹
J kg K
Which of the following best describes the specific heat capacity of a substance?
It is the amount of heat required to raise the temperature of 1 kg of the substance by 1 K.
It is the amount of heat required to raise the temperature of 1 mol of the substance by 1 K.
It is the amount of heat required to melt the substance.
It is the amount of heat required to vaporize the substance.
Given the formula for molar specific heat capacity, C = S/μ = (1/μ) (ΔQ/ΔT), what does μ represent?
Mass in grams
Number of moles
Volume in liters
Temperature in Kelvin
Refer to Table 11.1. Which substance has the highest specific heat capacity at room temperature and atmospheric pressure?
Carbon
Aluminium
Silver
Lead
Refer to Table 11.1. Which substance has the lowest specific heat capacity at room temperature and atmospheric pressure?
Lead
Tungsten
Silver
Copper
If the average energy of a solid atom in three dimensions is 3 k_B T, what is the total energy for a mole of a solid?
U = 2 k_B T × N_A
U = 3 k_B T × N_A = 3 R T
U = k_B T × N_A
U = 3 R / T
What is the relationship between the change in internal energy (ΔU) and the change in temperature (ΔT) for a solid at constant pressure?
ΔU/ΔT = 2R
ΔU/ΔT = 3R
ΔU/ΔT = R
ΔU/ΔT = k_B
What is the specific heat capacity of water in SI units?
4186 J kg⁻¹ K⁻¹
1000 J kg⁻¹ K⁻¹
273 J kg⁻¹ K⁻¹
1 J kg⁻¹ K⁻¹
Which of the following best describes the term "mechanical equivalent" in the context of heat?
It is the amount of work needed to produce 1 cal of heat.
It is the amount of heat needed to produce 1 J of work.
It is the amount of energy required to raise the temperature of 1 kg of water by 1°C.
It is the amount of heat required to melt 1 g of ice.
What is the difference between specific heat capacity at constant volume and specific heat capacity at constant pressure for an ideal gas?
Specific heat at constant pressure is greater than at constant volume.
Specific heat at constant volume is greater than at constant pressure.
Both are always equal.
Specific heat at constant pressure is always zero.
Which equation represents the relationship between pressure, volume, and temperature for one mole of an ideal gas?
PV = RT
PV = nRT
P = V/T
PV = R/T
If ΔQ is absorbed at constant volume, which equation correctly expresses the molar specific heat capacity at constant volume (Cv)?
Cv = (ΔQ/ΔT)v
Cv = (ΔQ/ΔT)p
Cv = (ΔU/ΔT)p
Cv = (ΔV/ΔT)p
What does the graph in Fig. 11.5 illustrate?
The variation of specific heat capacity of water with temperature.
The boiling point of water at different pressures.
The melting point of ice at different temperatures.
The density of water at different temperatures.
Why is it preferable to use the unit joule (J) instead of calorie for heat in SI units?
Joule is the SI unit for energy and is more universally applicable.
Calorie is not a unit of energy.
Joule is easier to measure than calorie.
Calorie is only used for measuring food energy.
Which equation gives the desired relation between Cp and Cv for an ideal gas?
Cp - Cv = R
Cp + Cv = R
Cp × Cv = R
Cp / Cv = R
What is an equilibrium state of a thermodynamic system?
A state described by specific values of pressure, volume, temperature, and mass.
A state where temperature is always zero.
A state where pressure and volume are not defined.
A state where only mass is considered.
Which of the following best describes an extensive variable in thermodynamics?
Indicates the 'size' of the system
Remains unchanged when the system is divided into two equal parts
Refers to pressure and temperature
Is always independent of the system's mass
What is the equation of state for an ideal gas?
P = μRT
ΔQ = ΔU + PΔV
PV = nRT
U = mRT
Which of the following is an example of an intensive variable?
Volume
Pressure
Mass
Internal energy
What happens to a gas when the partition in a box is suddenly removed?
The gas immediately reaches equilibrium
The gas undergoes free expansion and is not in equilibrium
The temperature and pressure remain uniform throughout
The gas condenses into a liquid
Why is it convenient to imagine an idealised process in thermodynamics?
Because real processes are always reversible
Because every stage is an equilibrium state
Because temperature and pressure are always constant
Because it eliminates the need for equations of state
Which of the following statements is true about non-equilibrium states in thermodynamics?
They have well-defined pressure and temperature
They are easy to describe using state variables
They do not have well-defined pressure and temperature
They are always extensive
According to the text, what is an isotherm?
A curve of constant pressure
A pressure-volume curve for a fixed temperature
A line of constant volume
A temperature-density curve
Which equation is used to check the consistency of thermodynamic equations using extensive and intensive variables?
PV = μRT
ΔQ = ΔU + PΔV
U = mRT
P = nRT
What is a quasi-static process in thermodynamics?
A process that occurs very rapidly
A process that is infinitely slow and nearly static
A process with large temperature gradients
A process with accelerated motion of the piston
In a quasi-static process, how does the temperature of the surrounding reservoir compare to the system?
The temperature difference is very large
The temperature difference is infinitesimally small
The temperature is always equal
The temperature difference is unpredictable
Which type of thermodynamic process keeps the temperature constant throughout?
Isobaric process
Isochoric process
Isothermal process
Adiabatic process
What is the defining feature of an isobaric process?
Temperature constant
Pressure constant
Volume constant
No heat flow
What happens in an adiabatic process?
Temperature remains constant
Pressure remains constant
No heat flows between the system and the surroundings
Volume remains constant
According to Boyle’s Law, what happens to the pressure of a given mass of gas if its volume increases during an isothermal process?
Pressure increases
Pressure remains constant
Pressure decreases
Pressure fluctuates randomly
Which equation represents the work done by an ideal gas during an isothermal process?
W = PΔV
W = μRT ln(V2/V1)
W = mgh
W = ½mv²
Which equation represents the relationship between pressure and volume for an adiabatic process in an ideal gas?
P₁V₁ = P₂V₂
P1V1γ=P2V2γ
P₁V₁/T₁ = P₂V₂/T₂
P₁V₁ + P₂V₂ = constant
What is the value of ΔU (change in internal energy) for a cyclic process?
ΔU > 0
ΔU < 0
ΔU = 0
ΔU = infinity
In an isochoric process, what remains constant?
Pressure
Volume
Temperature
Internal energy
During an adiabatic process, what happens to the temperature of the gas if work is done by the gas (W > 0)?
Temperature increases
Temperature decreases
Temperature remains constant
Temperature becomes zero
Which process involves the system being insulated from the surroundings, with no heat absorbed or released?
Isothermal process
Isochoric process
Adiabatic process
Isobaric process
In an isobaric process, which variable is held constant?
Pressure
Volume
Temperature
Internal energy
What is the equation for work done by the gas in an isobaric process?
W = P(V₂ - V₁)
W = μR(T₂ - T₁)
W = 0
W=P1V1γ−P2V2γ
What does the First Law of Thermodynamics imply for an isothermal process?
Heat supplied equals the work done by the gas
No work is done by the gas
Internal energy increases
Temperature decreases
Which specific heat ratio is represented by γ in the context of adiabatic processes?
γ = C_v / C_p
γ = C_p / C_v
γ = R / C_v
γ = C_v / R
Which law states that the efficiency of a heat engine can never be unity?
First Law of Thermodynamics
Second Law of Thermodynamics
Law of Conservation of Mass
Law of Universal Gravitation
What is the main principle described by the First Law of Thermodynamics?
Conservation of mass
Conservation of energy
Conservation of momentum
Conservation of charge
Why can't the base of a vessel on an oven get cooler spontaneously and warm up the base?
It violates the First Law of Thermodynamics
It violates the Second Law of Thermodynamics
It violates the Law of Conservation of Mass
It violates the Law of Universal Gravitation
Which of the following is an example of an irreversible process?
A gas returning to its cylinder after diffusion
The base of a vessel on an oven cooling spontaneously
The combustion reaction of a mixture of petrol and air in a kitchen
A liquid stirring in thermal contact with a reservoir and converting work into heat
If a moving body comes to a stop and loses its mechanical energy as heat, what type of process is this?
Reversible
Irreversible
Equilibrium
Isothermal
Why can the efficiency of a refrigerator never be infinite according to the Second Law of Thermodynamics?
Because energy is always conserved
Because the coefficient of performance can never be infinite
Because heat engines are always perfect
Because mass is always conserved
Which of the following best describes a reversible thermodynamic process?
A process that increases the temperature of the system
A process that can be turned back so both the system and surroundings return to their original states with no other change in the universe
A process that only changes the surroundings
A process that always involves heat loss
What is required for a process to be reversible in thermodynamics?
The process must be adiabatic
The process must be quasi-static and non-dissipative
The process must be isochoric
The process must be irreversible
Why does the Second Law of Thermodynamics rule out the possibility of a perfect heat engine with 100% efficiency?
Because heat engines always operate at low temperatures
Because irreversible processes are always present in practical engines
Because heat cannot be converted into work
Because all processes are reversible
