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.
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Ответ:
The new pressure is 17.63 atm or 13398.798 mmHg
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
Ответ:
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