Problem: A 125.0-mL contains a gas at 27°C and 760 mm Hg of pressure. The gas is pumped into an empty 1.50-L flask also at a temperature of 27°C. What is the pressure (in atm) of the gas in the new flask? Show your work for partial credit.P1 V1/T1 = P2V2/T2 1 atm = 760 Torr = 760 mmHg = 101325 Pa = 1.01325 bar

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A 125.0-mL contains a gas at 27°C and 760 mm Hg of pressure. The gas is pumped into an empty 1.50-L flask also at a temperature of 27°C. What is the pressure (in atm) of the gas in the new flask? Show your work for partial credit.

P1 V1/T1 = P2V2/T2 


1 atm = 760 Torr = 760 mmHg = 101325 Pa = 1.01325 bar

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What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Chemistry Gas Laws concept. If you need more Chemistry Gas Laws practice, you can also practice Chemistry Gas Laws practice problems.

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Based on our data, we think this problem is relevant for Professor Randles' class at UCF.