Multiple Choice
A sample of nitrogen dioxide gas at 130 ºC and 315 torr occupies a volume of 500 mL. What will the gas pressure be if the volume is reduced to 320 mL at 130 ºC?
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8. Gases, Liquids and Solids
The Ideal Gas Law Derivations
Multiple Choice
On most spray cans it is advised to never expose them to fire. A spray can is used until all that remains is the propellant gas, which has a pressure of 1350 torr at 25 ºC. If the can is then thrown into a fire at 455 ºC, what will be the pressure (in torr) in the can?
A
750 torr
B
1800 torr
C
2190 torr
D
2850 torr
E
3300 torr
Verified step by step guidance1
Identify the initial conditions of the gas in the spray can: the initial pressure (P1) is 1350 torr and the initial temperature (T1) is 25 ºC. Convert the temperature from Celsius to Kelvin by adding 273.15, so T1 = 25 + 273.15 = 298.15 K.
Identify the final conditions: the final temperature (T2) is 455 ºC. Convert this temperature to Kelvin as well, T2 = 455 + 273.15 = 728.15 K.
Use the ideal gas law relationship for constant volume, which is given by the formula \( \frac{P1}{T1} = \frac{P2}{T2} \). This equation relates the initial and final pressures and temperatures of the gas.
Rearrange the formula to solve for the final pressure (P2): \( P2 = P1 \times \frac{T2}{T1} \). Substitute the known values into the equation: P1 = 1350 torr, T1 = 298.15 K, and T2 = 728.15 K.
Calculate the final pressure (P2) using the rearranged formula. This will give you the pressure in the can when exposed to the fire, which should match one of the provided options.
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