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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11 Gases
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
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 to the Celsius temperature.
Identify the final temperature (T2) when the can is exposed to fire: 455 ºC. Convert this temperature to Kelvin as well.
Use the ideal gas law relationship for constant volume, which is expressed as P1/T1 = P2/T2, where P2 is the final pressure we want to find.
Rearrange the equation to solve for the final pressure (P2): P2 = P1 * (T2/T1).
Substitute the known values into the equation: P1 = 1350 torr, T1 = 298.15 K (25 ºC in Kelvin), and T2 = 728.15 K (455 ºC in Kelvin). Calculate the final pressure P2 in torr.
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