Question

What pressure (in atm) is required to compress 1.00 L of gas at 670.Mm Hg pressure to a volume of 50.0 mL. Please note that units need to be converted to match each other BEFORE you calculate.

Answer 1

The new pressure is 17.63 atm or 13398.798 mmHg

Step-by-step explanation:

Step 1: Data given

Volume of the gas = 1.00 L

Pressure of the gas = 670 mmHg = 670 / 760 atm = 0.881579 atm

The volume is decreased to 50.0 mL = 0.050 L

Step 2: Calculate the new volume

P1*V1 = P2*V2

⇒with P1 = the initial pressure = 670 mm Hg = 0.881579 atm

⇒with V1 = the initial volume = 1.00 L

⇒with P2 = the new pressure ⇒ TO BE DETERMINED

⇒with V2 = the new decreased volume = 0.050 L

0.881579 atm * 1.00L = P2 * 0.050 L

P2 = 17.63 atm = 13398.798 mmHg

The new pressure is 17.63 atm or 13398.798 mmHg