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The already familiar direction of heat transfer from hot to cold is the basis of our first version of the second law of thermodynamics    .

The second law of thermodynamics (first expression)

Heat transfer occurs spontaneously from higher- to lower-temperature bodies but never spontaneously in the reverse direction.

Another way of stating this: It is impossible for any process to have as its sole result heat transfer from a cooler to a hotter object.

Heat engines

Now let us consider a device that uses heat transfer to do work. As noted in the previous section, such a device is called a heat engine, and one is shown schematically in [link] (b). Gasoline and diesel engines, jet engines, and steam turbines are all heat engines that do work by using part of the heat transfer from some source. Heat transfer from the hot object (or hot reservoir) is denoted as Q h size 12{Q rSub { size 8{h} } } {} , while heat transfer into the cold object (or cold reservoir) is Q c size 12{Q rSub { size 8{c} } } {} , and the work done by the engine is W size 12{W} {} . The temperatures of the hot and cold reservoirs are T h size 12{T rSub { size 8{h} } } {} and T c size 12{T rSub { size 8{c} } } {} , respectively.

Part a of the figure shows the spontaneous heat transfer from a hot system to a cold system. The hot reservoir at temperature T sub h is represented by a rectangular section in the top and the cold reservoir at temperature T sub c is shown as a rectangular section at the bottom. Heat is shown to flow from hot reservoir to cold reservoir as shown by a bold arrow pointing downward. Part b of the figure shows a heat engine represented as a circle. The hot reservoir at temperature T sub h is represented by a rectangular section at the top and a cold reservoir at temperature T sub c is shown as a rectangular section at the bottom. Heat Q sub h is transferred out of the hot reservoir, work W is the output equals Q sub h minus Q sub c, and heat Q sub c is the heat transferred into the cold reservoir. All these are shown using bold arrows.
(a) Heat transfer occurs spontaneously from a hot object to a cold one, consistent with the second law of thermodynamics. (b) A heat engine, represented here by a circle, uses part of the heat transfer to do work. The hot and cold objects are called the hot and cold reservoirs. Q h size 12{Q rSub { size 8{h} } } {} is the heat transfer out of the hot reservoir, W size 12{W} {} is the work output, and Q c size 12{Q rSub { size 8{c} } } {} is the heat transfer into the cold reservoir.

Because the hot reservoir is heated externally, which is energy intensive, it is important that the work is done as efficiently as possible. In fact, we would like W size 12{W} {} to equal Q h size 12{Q rSub { size 8{h} } } {} , and for there to be no heat transfer to the environment ( Q c = 0 size 12{Q rSub { size 8{c} } =0} {} ). Unfortunately, this is impossible. The second law of thermodynamics    also states, with regard to using heat transfer to do work (the second expression of the second law):

The second law of thermodynamics (second expression)

It is impossible in any system for heat transfer from a reservoir to completely convert to work in a cyclical process in which the system returns to its initial state.

A cyclical process    brings a system, such as the gas in a cylinder, back to its original state at the end of every cycle. Most heat engines, such as reciprocating piston engines and rotating turbines, use cyclical processes. The second law, just stated in its second form, clearly states that such engines cannot have perfect conversion of heat transfer into work done. Before going into the underlying reasons for the limits on converting heat transfer into work, we need to explore the relationships among W size 12{W} {} , Q h size 12{Q rSub { size 8{h} } } {} , and Q c size 12{Q rSub { size 8{c} } } {} , and to define the efficiency of a cyclical heat engine. As noted, a cyclical process brings the system back to its original condition at the end of every cycle. Such a system’s internal energy U is the same at the beginning and end of every cycle—that is, Δ U = 0 size 12{ΔU=0} {} . The first law of thermodynamics states that

Δ U = Q W , size 12{ΔU=Q - W} {}

where Q size 12{Q} {} is the net heat transfer during the cycle ( Q = Q h Q c size 12{Q=Q rSub { size 8{h} } - Q rSub { size 8{c} } } {} ) and W size 12{W} {} is the net work done by the system. Since Δ U = 0 size 12{ΔU=0} {} for a complete cycle, we have

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Source:  OpenStax, College physics. OpenStax CNX. Jul 27, 2015 Download for free at http://legacy.cnx.org/content/col11406/1.9
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