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