Asample containing 4.80 g of o2 gas has an initial volume of 15.0 l. what is the final volume, in liters, when each of the following changes occurs in the quantity of the gas at a constant pressure and temperature?
a. a sample of 0.500 mole of o2 is added to the 4.80 g of o2 in the container.
b. a sample of 2.00 g of o2 is removed.
c. a sample of 4.00 g of o2 is added to the 4.80 g of o2 gas in the container.

yes

explanation:

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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