Ten grams of a gas occupies 12.5 liters at a pressure of 42.0 cm hg. what is the volume when the pressure has increased to 75.0 cm hg? 6.00 l 7.00 l 8.00 l none of the above

             7.0 L

              According to Boyle's Law, " The Volume of a given mass of gas at constant temperature is inversely proportinal to the applied Pressure". Mathematically, the initial and final states of gas are given as,

                                     P₁ V₁  =  P₂ V₂     (1)

Data Given;

                  P₁  =  42.0 cm Hg

                  V₁  =  12.5 L

                  P₂  =  75.0 cm Hg

                  V₂  =  ??

Solving equation 1 for V₂,

                   V₂  =  P₁ V₁ / P₂

Putting values,

                   V₂  =  (42.0 cm Hg × 12.5 L) ÷ 75.0 cm Hg

                   V₂  =  7.0 L

          As the Pressure has increased from 42.0 cm Hg to 75.0 cm Hg, therefore, Volume got decreased from 12.5 L to 7.0 L.

14 days is the half-life of phosphorus-32