Final answer:
Heating the gas-sealed canister to -5.0°C and 713 mmHg is the action most likely to bring the gas to STP. High temperatures can cause increased pressure leading to rupture, and the ideal gas law can calculate new pressures when temperatures change.
Step-by-step explanation:
The action that would most likely bring the gas to standard temperature and pressure (STP), from its initial condition of -5.0°C and 713 mmHg would be Option 2: Heating the canister. STP is defined as a temperature of 0°C (273.15 K) and a pressure of 760 mmHg (1 atmosphere). Heating the canister will increase the temperature of the gas towards STP. The other options may change the pressure, but they would not result in reaching both the standard temperature and pressure simultaneously.
(a) The warning not to store the can at temperatures above 120 °F (48.8 °C) or incinerate it is because high temperatures can cause the pressure inside the can to increase, potentially leading to rupture or explosion. As the temperature increases, the pressure increases proportionately in a sealed container due to the gas laws, and since isobutane is combustible, incineration poses a significant risk of explosion.
(b) To calculate the new pressure when a gas can is left in a car that reaches 50 °C, we use the ideal gas law in the form of the combined gas law equation, assuming the volume and amount of gas remain constant:
P1/T1 = P2/T2, where
- P1 is the initial pressure (360 kPa)
- T1 is the initial temperature in Kelvin (24 °C + 273.15 = 297.15 K)
- P2 is the final pressure
- T2 is the final temperature in Kelvin (50 °C + 273.15 = 323.15 K)
Therefore, P2 can be found by rearranging the equation to P2 = P1 * (T2/T1), giving us the new pressure.