3.00 mol of an ideal gas with CV, m=3R/2 undergoes an expansion from an initial state described by T=310.K and P=6.00bar against a constant external pressure of zero bar until the final pressure is equal to one-fifth of its initial value. The state of the surroundings is T=298K, P=0.250bar. a. FInd entropy of surroundings.

b. Find total entropy

Explanation:

The given data is as follows.

          n = 3 mol,  

      > \frac{1}{5} \times P_{1}[/tex]

so,     = 1.2 bar

             T = 310 K

Since, the given piston has no mass and it is friction less. Hence, the system will be completely insulated in nature.

It is given that the state of surrounding is given as follows.

          T = 298 K and P = 0.25 bar

So,     = 0

According to the first law of thermodynamics is as follows.

Since, there is no friction so W = 0. Also, the system is well insulated hence, Q = 0. Therefore,

                           = 0 + 0

                           = 0

For an ideal gas,

As,     = 0 this means that

                    =

                    = 0.2

Now, expression for entropy of the system is as follows.

As,      

so,      

                         = -R ln (0.2)

                         =

                         =

                         = 13.38 mol K

Also,                    

                       =

                       = 40.142 J/K > 0

This means that > 0

                      = 40.142 J/K > 0

This means that the total entropy is immersible and follows second law of thermodynamics.

the answer is 1260

you spend 7 hours in school for 1 school day with 5 school days in 1 school week with 36 school weeks in a school year.

7*5*36= 1260 it's all about multiplying

confused

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