A spray can containing a propellant gas at twice atmospheric pressure (202 kPa) and having a volume of 119.00 cm is at 27°C. It is then tossed into an open fire. (Warning: Do not do this experiment; it is very dangerous.) When the temperature of the gas in the can reaches 195°C, what is the pressure inside the can? Assume any change in the volume of the can is negligible. SOLUTION Conceptualize Intuitively, you should expect that the pressure of the gas in the container increases because of the increasing temperature. Categorize We model the gas in the can as ideal and use the ideal gas law to calculate the new pressure. Analyze Rearrange PV = nRT (Use the following as necessary: n and R.): (1) PV = nR No air escapes during the compression, so that n, and therefore nR, remains constant. Hence, set the initial value of the left side of Equation (1) equal to the final value (Use the following as necessary: PF VAT and T;. Do not substitute numerical values; use variables only.): ay may Because the initial and final volumes of the gas are assumed to be equal, cancel the volumes (Use the following as necessary: PF TF, and T;. Do not substitute numerical values; use variables only.): Solve for Pf(in kPa): | kPa