Question

A container holds 500. mL of CO2 at 20.° C and 735 torr. What will be the volume of the CO2 if the pressure is increased to 807 torr? (0.456 L)

Answer 1

Answer:- 0.456 L

Solution:- Looking at the given information, only volume and pressure are changing and the temperature is constant. We know that, at constant temperature, the volume of the gas is inversely proportional to the pressure.

$P_1V_1=P_2V_2$

$P_1$ = 735 torr

$P_2$ = 807 torr

$V_1$ = 500. mL

$V_2$ = ?

Let's plug in the values in the equation and solve it for final volume.

$735torr(500.mL)=807torr(V_2)$

$V_2=\frac{735torr(500.mL)}{807torr}$

$V_2=456mL$

since, 1 L = 1000 mL

$456mL(\frac{1L}{1000mL})$

= 0.456 L

So, the volume of carbon dioxide at the new pressure will be 456 mL or 0.456 L.