1. A sample of gas under a pressure of 622 kPa has a volume of 233 cm3. The pressure is increased to 988 kPa, while the temperature remains constant. What volume will the gas occupy at this pressure?

2. The pressure exerted by a gas is 2.0 atm while it has a volume of 350 cm3. What would be the volume of this sample of gas at standard atmospheric pressure?

To solve both of these problems, we can use Boyle's Law, which states that the pressure and volume of a gas are inversely proportional at constant temperature.

1. To find the volume of the gas at the increased pressure, we can use the formula:

P1V1 = P2V2

Where P1 and V1 are the initial pressure and volume, and P2 and V2 are the final pressure and volume.

Given:
P1 = 622 kPa
V1 = 233 cm3
P2 = 988 kPa

We need to solve for V2.

Rearranging the formula, we have:

V2 = (P1V1) / P2

Substituting the given values:

V2 = (622 kPa * 233 cm3) / 988 kPa

V2 ≈ 146.98 cm3

Therefore, the gas will occupy approximately 146.98 cm3 at the increased pressure.

2. To find the volume of the gas at standard atmospheric pressure (1 atm), we can use the same formula:

P1V1 = P2V2

Given:
P1 = 2.0 atm
V1 = 350 cm3
P2 = 1 atm

We need to solve for V2.

Rearranging the formula, we have:

V2 = (P1V1) / P2

Substituting the given values:

V2 = (2.0 atm * 350 cm3) / 1 atm

V2 = 700 cm3

Therefore, the volume of the gas at standard atmospheric pressure would be 700 cm3.

(P1V1/T1) = (P2V2/T2)

Remember T must be in kelvin.