A 10.0 L balloon contains helium gas at a pressure of 655 mmHg. What is the final pressure, in millimeters of mercury, if the final volume is 13.8 L?

474.64mmHg

Explanation:

From the question given, we obtained the following:

V1 = 10L

P1 = 655mmHg

V2 = 13.8L

P2 =?

P1V1 = P2V2

10 x 655 = P2 x 13.8

Divide both side by the coefficient P2 i.e 13.8

P2 = (10 x 655) / 13.8

P2 = 474.64mmHg

Therefore, the new pressure will be 474.64mmHg

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

explanation: