Thermodynamics

The Zeroth Law of Thermodynamics is essentially a law of:

Which property is common to all systems in thermal equilibrium with one another?

If System A is at $10 \, ^\circ C$ and System B is at $50 \, ^\circ F$, are they in thermal equilibrium?

An ideal thermos flask aims to behave as which type of boundary?

Which statement correctly describes the Zeroth Law's role in measuring temperature?

If System A and System B are separated by a diathermic wall, and System B and System C are separated by a diathermic wall, but System A and System C are separated by an adiabatic wall, will A and C eventually reach thermal equilibrium?

Which of the following is a diathermic material?

What is the relationship between the Zeroth Law and the state variables $(P, V, T)$ of an ideal gas?

If system $A$ is in thermal equilibrium with $B$, and $B$ is in thermal equilibrium with $C$, does this imply that $A$, $B$, and $C$ must have the same pressure?

If the Zeroth Law defines temperature $T$, what does the existence of $T$ allow us to do with isotherms on a $P-V$ diagram?

The concept that 'Internal energy is a function of state' means its change depends only on:

During a process, if the work done by the system is exactly equal to the heat supplied, the change in internal energy must be:

If a gas absorbs 500 J of heat and its internal energy increases by 200 J, how much work was performed by the gas?

Heat added to a system ($Q$) is used to increase internal energy ($U$) and perform work ($W$). If $U$ increases by 20 J and $W$ is 30 J, find $Q$.

If a system is completely isolated from its surroundings, which of the following is true according to the First Law?

In an isothermal expansion of an ideal gas, the heat supplied to the gas is used to:

For an ideal gas undergoing a cyclic process, if the net heat absorbed by the system is $Q_{net}$, then the net work done $W_{net}$ by the system is:

The molar heat capacity of a gas at constant volume is $C_v$. If the gas undergoes a process $PV^n = K$, the molar heat capacity is $C = C_v + R/(1-n)$. For an isothermal process, $n=1$, which makes $C$:

Consider a process $P = P_0 [1 + (V/V_0)^2]$. For an ideal gas, the work done in expanding from $V=0$ to $V=V_0$ is:

A certain amount of heat $Q$ is given to a diatomic gas. If the gas expands at constant pressure, the ratio of work done by the gas to the heat given is:

The slope of the P-V curve for an isothermal process is given by:

A gas system is perfectly insulated from its surroundings. If work is done on the system, the process is:

What is the value of $\gamma$ for a triatomic non-linear gas?

For an ideal gas, the change in internal energy depends only on:

Which of the following variables is NOT constant in an isothermal process?

An ideal gas is compressed adiabatically from $V$ to $V/4$. If the initial pressure is $P$, and $\gamma = 1.5$, the final pressure is:

What is the change in internal energy ($ΔU$) for a gas undergoing an adiabatic expansion?

The molar heat capacity of a gas in a process $P V^n = \text{constant}$ is $C = C_v + R/(1-n)$. If $C = C_p$, then $n$ is:

When a gas is compressed adiabatically, its temperature increases because:

In an adiabatic expansion of an ideal gas, which of the following remains constant?

If a system is in a state of maximum entropy, it is in:

When a gas expands adiabatically and reversibly, its entropy:

What is the direction of heat flow in a refrigerator?

The second law of thermodynamics provides the basis for defining:

The Second Law of Thermodynamics is essentially a law of:

If a system absorbs $2000\text{ J}$ of heat at $500\text{ K}$ in a reversible isothermal process, the change in entropy of the system is:

A measure of the degree of disorder of a system is known as:

A Carnot engine works with a source at $500\text{ K}$ and a sink at $T\text{ K}$. Another Carnot engine works with a source at $T\text{ K}$ and a sink at $200\text{ K}$. If the efficiencies of both are equal, $T$ is:

In a reversible process, $\Delta S = 0$ for the universe. In an irreversible process, $\Delta S_{universe} > 0$. This principle is known as:

A gas expands from $V_1$ to $V_2$ along the path $P = a V^2$. The entropy change is:

The First Law of Thermodynamics is a statement of:

Work is a form of energy in:

In which process is the heat exchange $\Delta Q = 0$?

During an adiabatic process, the quantity that remains constant is:

A thermodynamic system undergoes a change of state through a two-step process as shown in the flowchart. In the first step (State 1 to State 2), the system absorbs $100 \text{ J}$ of heat and performs $40 \text{ J}$ of work. In the second step (State 2 to State 3), it releases $30 \text{ J}$ of heat and $10 \text{ J}$ of work is performed on the system. Calculate the net change in internal energy ($\Delta U$) for the overall process from State 1 to State 3.

A gas at pressure $P$ is compressed to half its volume adiabatically. The new pressure will be:

For a cyclic process, which of the following is non-zero?

Work done in an adiabatic process depends on:

A gas mixture contains 1 mole of $H_2$ and 1 mole of $He$. The value of $\gamma$ for the mixture is:

If the degree of freedom of a gas is $f$, then the ratio of work done to heat supplied in an isobaric process is:

When temperature increases, the internal energy of an ideal gas:

Which of the following has the highest heat capacity for a given mass?

The ratio of molar heat capacities for a polyatomic gas (non-linear) is generally close to:

How many joules are in one calorie?

A constant power heater is used to heat two different liquids in separate experiments. First, $100 \text{ g}$ of water is heated, and its temperature increases by $10^\circ\text{C}$ in $4 \text{ minutes}$. Next, $50 \text{ g}$ of an unknown liquid is heated, and its temperature increases by the same $10^\circ\text{C}$ in $1 \text{ minute}$. If the specific heat capacity of water is $4200 \text{ J kg}^{-1} \text{ K}^{-1}$, what is the specific heat capacity of the unknown liquid? (Assume no heat is lost to the surroundings and neglect the heat capacity of the containers).

What is the degree of freedom for a non-linear triatomic gas molecule at moderate temperatures?

Two spheres of the same radius but different materials have heat capacities in the ratio $2:3$. If they are heated to the same temperature and allowed to cool in the same surroundings, the initial rate of cooling will be in the ratio:

A system is provided with 50 J of heat and it does 20 J of work. If the temperature of the system rises by 5°C, and the system consists of 2 moles of a gas, what is the molar heat capacity for this process?

If 1 mole of a monatomic gas is mixed with 1 mole of a diatomic gas, what is the $C_v$ of the mixture?

What is the ratio of $C_p/C_v$ for a gas whose molecules possess 3 translational and 2 rotational degrees of freedom?

The value of $R$ in calories is approximately:

A system that cannot exchange matter or energy with its surroundings is:

The total internal energy of a system is the sum of:

According to Charles's Law, at constant pressure, volume $V$ is proportional to:

An ideal gas is contained in a vessel of fixed volume $V$. A graph is plotted showing the relationship between pressure $P$ on the y-axis and absolute temperature $T$ on the x-axis. If the amount of gas in the vessel is increased from $n$ moles to $2n$ moles, how does the slope of the $P$ vs $T$ graph change?

The equation of state for a specific non-ideal gas is given by the relation $P(V - nb) = nRT$, where $b$ is a constant representing the excluded volume. If $1$ mole of this gas is compressed isothermally from an initial volume $V_1$ and pressure $P_1$ to a final volume $V_2$, what is the expression for the final pressure $P_2$?

Two identical, rigid compartments X and Y are separated by a removable partition. Each compartment contains $n$ moles of an ideal gas at a pressure $P$ and absolute temperature $T$. If the partition is removed and the gases mix to reach a new equilibrium state in the combined volume, what will be the final pressure $P'$ and temperature $T'$ of the system?

A system is in a state where $P, V, T$ are fixed. If we double the amount of substance while keeping $P$ and $T$ constant, what happens to the molar volume $V_m$?

Given $(\partial U / \partial V)_T = T (\partial P / \partial T)_V - P$. For an ideal gas, this expression evaluates to:

For a soap film, the surface tension $\gamma$ is a state variable. The work done to increase the area $A$ is $dW = \gamma dA$. What is the state equation for a film where $\gamma$ depends only on temperature?

In the study of thermodynamic processes, a boundary that allows the exchange of heat energy between a system and its surroundings, leading to thermal equilibrium, is known as a:

In a cyclic process, if the area of the closed loop on a P-V diagram is traversed clockwise, the net work done is:

Which of the following processes is represented by the equation $V/T = \text{constant}$?

The First Law of Thermodynamics can be written as $dU = dQ - dW$. If the system is an ideal gas undergoing an isochoric process, then:

In an adiabatic process, the heat exchanged ($Q$) is:

The slope of an isothermal curve on a P-V diagram is given by:

In a refrigerator, heat is transferred from:

An ideal gas is subjected to a cyclic process involving four thermodynamic states. The net heat exchange is $Q$ and net work done is $W$. For a complete cycle:

A cylinder with a movable piston contains 3 moles of hydrogen at standard temperature and pressure. The walls of the cylinder are made of a heat insulator, and the piston is insulated by having a pile of sand on it. By what factor does the pressure of the gas increase if the gas is compressed to half its original volume?

A system is taken from state $i$ to state $f$ along path $iaf$ and $ibf$. If $Q_{iaf} = 50 cal$ and $W_{iaf} = 20 cal$, and $W_{ibf} = 10 cal$, find $Q_{ibf}$.

A thermodynamic cycle that is perfectly reversible is known as:

The internal energy of an ideal gas depends only on its:

Plastic deformation of a metal wire is an example of:

A gas undergoes a process where no heat enters or leaves. This is:

The statement 'the entropy of the universe tends toward a maximum' is another way of stating:

What happens to the pressure of an ideal gas during a reversible adiabatic expansion?

Which of these processes is reversible?

Which of the following transitions represents an increase in entropy?

In the $T-S$ (Temperature-Entropy) diagram, a reversible adiabatic process is represented by:

What is the change in entropy when $10 g$ of water at $100^{\circ} C$ is converted to steam at $100^{\circ} C$? (Latent heat of vaporization $L = 2260 J/g$)

Isothermal processes in a Carnot cycle are carried out very:

A Carnot engine is operating between $500\,K$ and $250\,K$. What is its efficiency in percentage?

Which statement best describes the Kelvin-Planck statement in relation to a Carnot engine?

In the fourth step of the Carnot cycle (adiabatic compression), the temperature of the gas:

A Carnot engine rejects $1/4$th of the heat it absorbs from the source. The efficiency of the engine is:

A Carnot engine's efficiency is $0.3$. If we double the absolute temperature of both the source and the sink, the efficiency becomes:

In a Carnot cycle, which process results in the maximum temperature drop?

A Carnot engine follows the cycle shown in the diagram, where the process State 1 $\to$ State 2 is an isothermal expansion at temperature $T_1$, and State 2 $\to$ State 3 is an adiabatic expansion ending at temperature $T_2$. If the work done by the ideal gas (with adiabatic exponent $\gamma$) during the isothermal expansion is exactly twice the work done by the gas during the adiabatic expansion, what is the value of the isothermal expansion ratio $r = V_2/V_1$?

A Carnot engine operates between $T_1 = 900\, K$ and $T_2 = 300\, K$. The work done per cycle is $1200\, J$. The heat rejected per cycle is:

In a Carnot cycle, let $W_1, W_2, W_3, W_4$ be the work done during isothermal expansion, adiabatic expansion, isothermal compression, and adiabatic compression respectively. Then: