A sample of nitrogen gas in a 1.94-L container exerts a pressure of 1.54 atm at
ID: 1004438 • Letter: A
Question
A sample of nitrogen gas in a 1.94-L container exerts a pressure of 1.54 atm at 21 C.What is the pressure if the volume of the container is maintained constant and the temperature is raised to 344 C?
The volume of the container is held constant. Pressure is directly proportional with temperature. Use the pressure-temperature law.
P1 / T1 = P2 / T2
P1 = 1.54 atm
T1 = 21°C (301K)
T2 = 344°C (605K)
Asked: P2 (what is the final pressure when the temperature is increased? Expect a higher final pressure).
*** convert Celsius temperatures to Kelvin by adding 273.
Derive the formula for P2.
P2 = P1T2 / T1
= (1.54)(605) / 344
= 2.708 atm (this is the worng answer) Please help
Explanation / Answer
initial final
P1 = 1.54atm P2 =
T1 = 21c0 = 21+273= 294K T2 = 344c0 = 344+273 = 617K
P1/T1 = P2/T2
P2 = P1T2/T1
= 1.54*617/294 = 3.23atm >>>>> answer
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