Final answer:
The warning on the can instructs to store the flammable gases below a certain temperature to prevent explosion and release of harmful fumes. Using the ideal gas law, we can calculate the new pressure in the can when exposed to a higher temperature.
Step-by-step explanation:
(a) The warning on the can instructs to store the flammable gases below 120 °F (48.8 °C) because at higher temperatures, the pressure inside the can can increase significantly, leading to a higher risk of explosion. Additionally, incineration can release harmful fumes and pose a fire hazard.
(b) To determine the new pressure in the can, we can use the ideal gas law, which states that PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature in Kelvin. We first need to convert the initial and final temperatures to Kelvin. The initial temperature is 24 °C + 273.15 = 297.15 K, and the final temperature is 50 °C + 273.15 = 323.15 K. Next, we can rearrange the formula to solve for the new pressure: P2 = (P1 * V1 * T2) / (V2 * T1), where P2 is the new pressure, P1 is the initial pressure, V1 is the initial volume, T2 is the final temperature, V2 is the initial volume, and T1 is the initial temperature. Plugging in the values, we have P2 = (360 kPa * 350 mL * 323.15 K) / (350 mL * 297.15 K). The mL in the numerator and denominator cancel out, resulting in P2 = (360 kPa * 323.15 K) / 297.15 K. Finally, we can calculate P2 to find the new pressure.