Chapter 4 The Second Law of Thermodynamics

# 4.5 The Carnot Cycle

OpenStax and Paula Herrera-Siklody

Learning Objectives

- Describe the Carnot cycle with the roles of all four processes involved
- Outline the Carnot principle and its implications
- Demonstrate the equivalence of the Carnot principle and the second law of thermodynamics

In the early 1820s, Sadi Carnot (1786−1832), a French engineer, became interested in improving the efficiencies of practical heat engines. In 1824, his studies led him to propose a hypothetical working cycle with the highest possible efficiency between the same two reservoirs, known now as the **Carnot cycle**. An engine operating in this cycle is called a **Carnot engine**. The Carnot cycle is of special importance for a variety of reasons. At a practical level, this cycle represents a reversible model for the steam power plant and the refrigerator or heat pump. Yet, it is also very important theoretically, for it plays a major role in the development of another important statement of the second law of thermodynamics. Finally, because only two reservoirs are involved in its operation, it can be used along with the second law of thermodynamics to define an absolute temperature scale that is truly independent of any substance used for temperature measurement.

With an ideal gas as the working substance, the steps of the Carnot cycle, as represented by Figure 4.11, are as follows.

1.* Isothermal expansion*. The gas is placed in thermal contact with a heat reservoir at a temperature [latex]T_\text{h}[/latex]. The gas absorbs heat [latex]Q_\text{h}[/latex] from the heat reservoir and is allowed to expand isothermally, doing work [latex]W_\text{1}[/latex]. Because the internal energy [latex]E_\text{int}[/latex] of an ideal gas is a function of the temperature only, the change of the internal energy is zero, that is, [latex]{\Delta}E_\text{int} = 0[/latex] during this isothermal expansion. With the first law of thermodynamics, [latex]{\Delta}E_\text{int} = Q - W[/latex], we find that the heat absorbed by the gas is

[latex]Q_\text{h} = W_\text{1} = nRT_\text{h}\text{ln}\frac{V_N}{V_M}.[/latex]

*2. Adiabatic expansion*. The gas is thermally isolated and allowed to expand further, doing work [latex]W_\text{2}[/latex]. Because this expansion is adiabatic, the temperature of the gas falls—in this case, from [latex]T_\text{h}[/latex] to [latex]T_\text{c}[/latex]. From [latex]pV^\gamma[/latex]=constant and the equation of state for an ideal gas, [latex]pV = nRT[/latex], we have

[latex]TV^{\gamma - 1} = \text{constant},[/latex]

so that

[latex]T_\text{h}{V_N}^{\gamma-1} = T_\text{c}{V_\text{O}}^{\gamma-1}.[/latex]

*3. Isothermal compression*. The gas is placed in thermal contact with a cold reservoir at temperature [latex]T_\text{c}[/latex] and compressed isothermally. During this process, work [latex]W_\text{3}[/latex] is done on the gas and it gives up heat [latex]Q_\text{c}[/latex] to the cold reservoir. The reasoning used in step 1 now yields

[latex]Q_\text{c} = nRT_\text{c}\text{ln}\frac{V_O}{V_P},[/latex]

where [latex]Q_\text{c}[/latex] is the heat dumped to the cold reservoir by the gas.

*4. Adiabatic compression*. The gas is thermally isolated and returned to its initial state by compression. In this process, work [latex]W_\text{4}[/latex] is done on the gas. Because the compression is adiabatic, the temperature of the gas rises—from [latex]T_\text{c}[/latex] to [latex]T_\text{h}[/latex] in this particular case. The reasoning of step 2 now gives

[latex]T_\text{c}{V_P}^{\gamma-1} = T_\text{h}{V_M}^{\gamma-1}.[/latex]

The total work done by the gas in the Carnot cycle is given by

[latex]W = W_\text{1} + W_\text{2} - W_\text{3} - W_\text{4}.[/latex]

This work is equal to the area enclosed by the loop shown in the *pV* diagram of Figure 4.12. Because the initial and final states of the system are the same, the change of the internal energy of the gas in the cycle must be zero, that is, [latex]{\Delta}E_\text{int} = 0[/latex]. The first law of thermodynamics then gives

[latex]W = Q - {\Delta}E_\text{int} = (Q_\text{h} - Q_\text{c}) - 0,[/latex]

and

[latex]W = Q_\text{h} - Q_\text{c}.[/latex]

To find the efficiency of this engine, we first divide [latex]Q_\text{c}[/latex] by [latex]Q_\text{h}[/latex]:

[latex]\frac{Q_\text{c}}{Q_\text{h}} = \frac{T_\text{c}}{T_\text{h}}\frac{\text{ln}V_O/V_P}{\text{ln}V_N/V_M}.[/latex]

When the adiabatic constant from step 2 is divided by that of step 4, we find

[latex]\frac{V_O}{V_P} = \frac{V_N}{V_M}.[/latex]

Substituting this into the equation for [latex]Q_\text{c}/Q_\text{h}[/latex], we obtain

[latex]\frac{Q_\text{c}}{Q_\text{h}} = \frac{T_\text{c}}{T_\text{h}}.[/latex]

Finally, with Equation 4.2, we find that the efficiency of this ideal gas Carnot engine is given by

e = 1 – \frac{T_\text{c}}{T_\text{h}}.

\end{equation}

An engine does not necessarily have to follow a Carnot engine cycle. All engines, however, have the same net effect, namely the absorption of heat from a hot reservoir, the production of work, and the discarding of heat to a cold reservoir. This leads us to ask: Do all reversible cycles operating between the same two reservoirs have the same efficiency? The answer to this question comes from the second law of thermodynamics discussed earlier: *All reversible engine cycles produce exactly the same efficiency*. Also, as you might expect, all real engines operating between two reservoirs are less efficient than reversible engines operating between the same two reservoirs. This too is a consequence of the second law of thermodynamics shown earlier.

The cycle of an ideal gas Carnot refrigerator is represented by the pV diagram of Figure 4.13. It is a Carnot engine operating in reverse. The refrigerator extracts heat [latex]Q_\text{c}[/latex] from a cold-temperature reservoir at [latex]T_\text{c}[/latex] when the ideal gas expands isothermally. The gas is then compressed adiabatically until its temperature reaches [latex]T_\text{h}[/latex], after which an isothermal compression of the gas results in heat [latex]Q_\text{h}[/latex] being discarded to a high-temperature reservoir at [latex]T_\text{h}[/latex]. Finally, the cycle is completed by an adiabatic expansion of the gas, causing its temperature to drop to [latex]T_\text{c}[/latex].

The work done on the ideal gas is equal to the area enclosed by the path of the *pV* diagram. From the first law, this work is given by

[latex]W = Q_\text{h} - Q_\text{c}[/latex]

An analysis just like the analysis done for the Carnot engine gives

[latex]\frac{Q_\text{c}}{T_\text{c}} = \frac{Q_\text{h}}{T_\text{h}}.[/latex]

When combined with Equation 4.3, this yields

for the coefficient of performance of the ideal-gas Carnot refrigerator. Similarly, we can work out the coefficient of performance for a Carnot heat pump as

We have just found equations representing the efficiency of a Carnot engine and the coefficient of performance of a Carnot refrigerator or a Carnot heat pump, assuming an ideal gas for the working substance in both devices. However, these equations are more general than their derivations imply. We will soon show that they are both valid no matter what the working substance is.

Carnot summarized his study of the Carnot engine and Carnot cycle into what is now known as **Carnot’s principle**:

Carnot’s Principle

No engine working between two reservoirs at constant temperatures can have a greater efficiency than a reversible engine.

This principle can be viewed as another statement of the second law of thermodynamics and can be shown to be equivalent to the Kelvin statement and the Clausius statement.

Example 4.2

**The Carnot Engine**

A Carnot engine has an efficiency of 0.60 and the temperature of its cold reservoir is 300 K.

(a) What is the temperature of the hot reservoir?

(b) If the engine does 300 J of work per cycle, how much heat is removed from the high-temperature reservoir per cycle?

(c) How much heat is exhausted to the low-temperature reservoir per cycle?

**Strategy**

From the temperature dependence of the thermal efficiency of the Carnot engine, we can find the temperature of the hot reservoir. Then, from the definition of the efficiency, we can find the heat removed when the work done by the engine is given. Finally, energy conservation will lead to how much heat must be dumped to the cold reservoir.

**Solution**

a. From [latex]e = 1 - T_\text{c}/T_\text{h}[/latex] we have [latex]0.60 = 1 - \frac{300 \text{K}}{T_\text{h}}[/latex],

so that the temperature of the hot reservoir is [latex]T_\text{h} = \frac{300 \text{K}}{1 - 0.60} = 750 \text{K}.[/latex]

b. By definition, the efficiency of the engine is [latex]e = W/Q[/latex], so that the heat removed from the high-temperature reservoir per cycle is [latex]Q_\text{h} = \frac{W}{e} = \frac{300\text{J}}{0.60} = 500\text{J}.[/latex]

c. From the first law, the heat exhausted to the low-temperature reservoir per cycle by the engine is [latex]Q_\text{c} = Q_\text{h} - W = 500\text{J} - 300 \text{J} = 200\text{J}.[/latex]

**Significance**

A Carnot engine has the maximum possible efficiency of converting heat into work between two reservoirs, but this does not necessarily mean it is 100% efficient. As the difference in temperatures of the hot and cold reservoir increases, the efficiency of a Carnot engine increases.

Example 4.3

**A Carnot Heat Pump**

Imagine a Carnot heat pump operates between an outside temperature of [latex]0^\circ \text{C}[/latex] and an inside temperature of [latex]20.0^\circ \text{C}[/latex]. What is the work needed if the heat delivered to the inside of the house is 30.0 kJ?

**Strategy**

Because the heat pump is assumed to be a Carnot pump, its performance coefficient is given by [latex]K_\text{P} = Q_\text{h}/W = T_\text{h}/(T_\text{h} - T_\text{c})[/latex]. Thus, we can find the work *W* from the heat delivered [latex]Q_\text{h}[/latex].

**Solution**

The work needed is obtained from

[latex]W = Q_\text{h}/K_\text{P} = Q_\text{h}(T_\text{h} - T_\text{c})/T_\text{h} = 30\text{kJ} \times (293\text{K} - 273\text{K})/293\text{K} = 2\text{kJ}.[/latex]

**Significance**

We note that this work depends not only on the heat delivered to the house but also on the temperatures outside and inside. The dependence on the temperature outside makes them impractical to use in areas where the temperature is much colder outside than room temperature.

In terms of energy costs, the heat pump is a very economical means for heating buildings (Figure 4.14). Contrast this method with turning electrical energy directly into heat with resistive heating elements. In this case, one unit of electrical energy furnishes at most only one unit of heat. Unfortunately, heat pumps have problems that do limit their usefulness. They are quite expensive to purchase compared to resistive heating elements, and, as the performance coefficient for a Carnot heat pump shows, they become less effective as the outside temperature decreases. In fact, below about –10°C, the heat they furnish is less than the energy used to operate them.

Check Your Understanding 4.3

A Carnot engine operates between reservoirs at [latex]400^\circ \text{C}[/latex] and [latex]30^\circ \text{C}[/latex].

(a) What is the efficiency of the engine?

(b) If the engine does 5.0 J of work per cycle, how much heat per cycle does it absorb from the high-temperature reservoir?

(c) How much heat per cycle does it exhaust to the cold-temperature reservoir?

(d) What temperatures at the cold reservoir would give the minimum and maximum efficiency?

Check Your Understanding 4.4

A Carnot refrigerator operates between two heat reservoirs whose temperatures are [latex]0^\circ \text{C}[/latex] and [latex]25^\circ \text{C}[/latex].

(a) What is the coefficient of performance of the refrigerator?

(b) If 200 J of work are done on the working substance per cycle, how much heat per cycle is extracted from the cold reservoir?

(c) How much heat per cycle is discarded to the hot reservoir?

### Media Attributions

- Figure 4.11
- Figure 4.12
- Figure 4.13
- Figure 4.14