State the sign of $W$ for the system.

Calculate the change in internal energy of the system.

Define entropy in terms of microscopic arrangements.

State the SI unit of entropy.

State the second law of thermodynamics in Clausius form.

State the second law of thermodynamics in Kelvin form.

State the second law of thermodynamics in entropy form for an isolated system.

Calculate the work done by the gas.

State whether this work is positive or negative.

Calculate the change in internal energy of the gas.

State whether the answer depends on the path followed between the two temperatures.

Give a reason for your answer to (b).

Calculate the entropy change of the block.

State the sign of the entropy change of the surroundings.

Determine the total number of microstates.

Determine the number of microstates for the macrostate with exactly $3$ counters in the left half.

State why this macrostate is more likely than all 6 counters being in the left half.

State the change in total entropy of the gases.

Explain why the reverse process is not observed.

State why the entropy of the plant itself may decrease.

Explain why this does not contradict the second law.

State the sign of the net work done by the gas.

Explain what the enclosed area represents.

State the net change in internal energy for the cycle.

Identify the process $A \to B$.

State the work done during $A \to B$.

Identify the process $B \to C$.

State the relation between P and V for $B \to C$ if the gas is ideal and the temperature is constant.

State the adiabatic relation for this gas.

Calculate the final pressure.

State whether the temperature increases or decreases.

Calculate the net work output per cycle.

Calculate the efficiency.

State the change in internal energy of the working gas over one complete cycle.

Calculate the Carnot efficiency.

State one practical reason why the actual efficiency is lower.

State the value of $\Delta U$ for the isothermal expansion.

State the value of $Q$ for the adiabatic expansion.

State which curve is steeper on a $P$–$V$ diagram.

Explain the reason for the difference in steepness.

Calculate the Carnot efficiency for these reservoir temperatures.

Evaluate the claim.

State the first law of thermodynamics using the Clausius sign convention, defining each term.

Explain why the temperature of the gas increases during the rapid insulated compression.

Identify the $P$–$V$ graph shape for an isovolumetric and for an isobaric process.

Explain the energy transfers and internal-energy changes for isothermal and adiabatic expansions.

Describe how work done by a gas is obtained from a P–V graph.

Evaluate the student’s method and explain how a correct estimate should be made.

Outline the microscopic meaning of entropy using $S = k_B \ln \Omega$.

Discuss how the entropy increase of the gas can be described both microscopically and macroscopically during the isothermal expansion.

State the Clausius and Kelvin forms of the second law.

Compare these statements with the entropy form of the second law for reversible and irreversible processes in isolated systems.

State how the net work and net change in internal energy are represented over a complete cycle on a P–V diagram.

Evaluate how the three stages could allow the device to operate as a heat engine, including the roles of heat input, heat rejection and irreversibility.

Calculate the maximum efficiency if $T_h = 900\ \text{K}$ and $T_c = 300\ \text{K}$.

Discuss why this maximum efficiency cannot be exceeded and why a real high-power engine will be less efficient.

Distinguish between isolated and non-isolated systems.

Evaluate the claim, referring to local entropy decrease, surroundings, irreversibility and the long-term evolution of the universe.