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1.8  Second Law of Thermodynamics
                    All the relations developed in the preceding sections are used in making an energy
            accounting for various types of systems.  In addition to being able to write an energy
            balance,  an  engineer  must  be  able  to  predict  how  much  of  the  heat  transferred  to  a
            system may be converted into useful work, or how much work is required to produce a
            certain refrigerating effect, or whether or not a system will undergo a specified change.
            These predictions cannot be made on the basis of the first law alone. For example, it is
            impossible to predict from the first law alone how much of the heat transferred to a heat
            engine may be converted into work. As far as the first law is concerned, all the heat
            transferred could conceivably be converted into work. In  order to obtain  information
            regarding  these  aspects  of  engineering  analysis,  the  second  law  of  thermodynamics
            must be employed.
                  Limitation of the First Law. The First Law of Thermodynamics states that energy is
            conserved. However, we can think of many thermodynamics process, which conserve
            energy but which actually never occur. For example, when a hot body and a cold body
            are put into contact it simply does not happen the hot body gets hotter and the cold body
            gets colder. The Firs Law doesn’t restrict our ability to convert work into heat or heat
            into work, except that energy must be conserved in the process. In practice we cannot
            convert  a  given  quantity  of  heat  completely  into  work.  The  Second  Law  of
            Thermodynamics  deals  with  question  of  whether  process  does  or  doesn’t  occur  in
            nature.
                  There have been many statements of the second law, each emphasizing another facet
            of the law, but all are equivalent to one another.
                  Clausius’s statement: heat cannot flow by itself from a body at lower temperature to
            another one at a higher temperature.
            In a heat engine, heat flows in its natural direction — from a hot body to a cold one.
            During  this  flow,  a  part  of  the  heat  is converted into the work. In a refrigerator, heat
            flows in the reverse direction i.e., from a cold body to a hot one. But in this case, we
            have to do some work for maintaining this natural flow of heat. This work is done on
            the pump of the refrigerator without which the refrigerator cannot operate.
                  Carnot’s  statement:  the  heat  of  a  single  reservoir  cannot  be  converted  into
            mechanical work.
                 It  is  impossible  to  construct  a heat engine, which can take heat from a single heat
            reservoir and convert it completely into useful work. A heat engine must work between
            two temperatures, so that it receives heat from a heat reservoir at a higher temperature
            and  rejects  some  of  this  heat  to  another  heat  reservoir  at  lower  temperature.  This
            explains why we cannot utilize the immense heat energy stored in the seawater or in the
            atmosphere.
                The efficiency of all reversible engines operating between the same two temperatures
            is  the  same,  and  no  irreversible  engines  working  between  the  same  two  temperatures
            can have a greater efficiency than another one.








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