Question

What volume will 500 mL of gas at 20°C and a pressure of 420 mm Hg occupy if the temperature is reduced to -80°C and the pressure is increased to 650 mm Hg?

Answer 1

Approx. `200*mL`...…...

Explanation:

The combined gas law holds that `(P_1V_1)/T_1=(P_2V_2)/T_2`...we use terms of absolute temperature...we also KNOW that `1*atm` will support a column of mercury that is `760*mm` high...

And so we solve for...`V_2=(P_1V_1)/T_1xxT_2/P_2`

`=((420*mm*Hg)/(760*mm*atm^-1)*500*mL)/(293.15*K)xx(193.15*K)/((650*mm*Hg)/(760*mm*atm^-1))`

`=??*mL`