Posted by Norah on .
A sealed glass bottle containing air at atmospheric pressure (101kPa) and having a volume of 22 cm^3 is at 23 degrees Celsius. It is then tossed into an open fire.
When the temperature of the air in the bottle reaches 391 degrees celsius, what is the pressure inside the bottle? Assume any volume changes of the bottle are negligible. Answer in units of kPa.
Use the ideal gas law PV=nRT
V, n, and R are constant and irrelevant in this situation.
Therefore, use the equation P1/T1 = P2/T2.
101/23+273 = P2/391+273 (adding 273 because you MUST convert to Kelvin)
Solve for P2