Question

11) A sample of gas has a volume of 823.7 mL and a pressure of 351.8 torr. What volume (in mL) will the gas occupy at 752.9 torr if the temperature of the gas doesn't change? Keep the answer with one decimal place

Answer 1

384.9 mL.

Step-by-step explanation:

What is given?

Volume 1 (V1) = 823.7 mL.

Pressure 1 (P1) = 351.8 torr.

Pressure 2 (P2) = 752.9 torr.

What do we need? Volume 2 (V2).

Step-by-step solution:

This is a Boyle's Law problem. Boyle's law states that the volume of a given mass of gas varies inversely with the pressure when the temperature is kept constant. An inverse relationship is described in this way. As one variable increases in value, the other variable decreases.

The formula of the law is:

`P_1V_1=P_2V_2.`

Where P is pressure and V is volume. We want to find volume 2, 'V2'. So let's solve for 'V2' and replace the given data that we have in the new formula:

`V_2=(P_1V_1)/(P_2)=\frac{351.8\text{ torr}\cdot823.7\text{ mL}}{752.9\text{ torr}}=384.882\text{ mL}\approx384.9\text{ mL.}`

The new volumewill be 3384.9 mL You can note as the pressure is increasing, the volume is decreasing.