Question

a gas has a volume of 95 mL at a pressure of 930 torr. What volume will the gas occupy if the pressure is increased to 970 torr and the temperature remains constant

Answer 1

Boyle's law is a gas law, stating that the pressure and volume of a gas have an inverse relationship, when temperature is held constant i.e PV = constant. Therefore, P1V1 = P2V2--(i) ( P1 = initial pressure, P2= final pressure, V1= initial volume, V2= final volume). P1=930 torr, P2= 970 torr, V1= 95 ml, V2=?. Put these values in equation (i), 930 torr x 95 ml = 970 torr x V2. Therefore, V2 = 91.08 ml.

Answer 2

The volume occupied by the gas at pressure 970 torr is 91.08 mL.

Step-by-step explanation:

To calculate the new pressure, we use the equation given by Boyle's law.

This law states that pressure is directly proportional to the volume of the gas at constant temperature.

The equation given by this law is:

`P_1V_1=P_2V_2` (at constant temperature)

where,

`P_1\text{ and }V_1` are initial pressure and volume.

`P_2\text{ and }V_2` are final pressure and volume.

We are given:

`P_1=930 Torr\\V_1=95 mL\\P_2=970 Torr\\V_2=?`

Putting values in above equation, we get:

`930 Torr* 95 mL=270 Torr * V_2\\\\V_2=(P_1V_1)/(P_2)=(930 Torr* 95 mL)/(270 Torr)=91.08 mL`

The volume occupied by the gas at pressure 970 torr is 91.08 mL.