A 120. mL sample of a gas is at a pressure of 1.50 atm. If the temperature remains constant, what will be its volume at 3.50 atm of pressure?

Boyles law:

P1V1=P2V2 at constant temperature

P1=1.5 atm
V1=120 ml
P2=3.5 atm
V2=?

51.4mL

correct!

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

According to Boyle's Law, the formula is:

P1 * V1 = P2 * V2

Where:
P1 = initial pressure
V1 = initial volume
P2 = final pressure
V2 = final volume

In this case, we are given:
P1 = 1.50 atm
V1 = 120 mL
P2 = 3.50 atm (the final pressure we want to find)
V2 = unknown (the final volume we need to determine)

Plugging in these values, we get:

1.50 atm * 120 mL = 3.50 atm * V2

Simplifying the equation, we have:

180 atm.mL = 3.50 atm * V2

To find V2, we can divide both sides of the equation by 3.50 atm:

180 atm.mL / 3.50 atm = V2

V2 = 51.43 mL

Therefore, the volume of the gas at a pressure of 3.50 atm would be approximately 51.43 mL.