Nitrogen gas leaves a compressor at 2 MPa and 120 °C, and is collected in three different cylinders, each of volume 0.3 m3. In each case the cylinder is to be filled to a pressure of 2 MPa. Cylinder 1 is initially evacuated, cylinder 2 contains nitrogen at 0.1 MPa and 20 °C, and cylinder 3 contains nitrogen at 1 MPa and 20 °C. Find the final temperature of nitrogen in each cylinder, assuming nitrogen to be an ideal gas with a constant-pressure heat capacity of 29.3 J/molK. In each case assume the gas does not exchange heat with the cylinder walls.

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i think? ?

when the volume of gas is   changed from   717.73 ml   to 852 ml   the temperature will   change   from 315   c to 452   c

    calculation

this is calculated using the charles law formula

that is,   v1/t1 = v2/t2

          v1=?

        t1 = 315 c   into   kelvin = 315 +273 = 588 k

        v2 = 852   ml

        t2 = 425c + 273 =698 k

make v1   the subject of the formula ( by   multiplying both side by t1)

  v1=( v2 xt1) / t2

v1= (852 ml   x 588 k)/ 698 k= 717.73 ml