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If a container of compressed gas has a volume of 500mL with pressure of 1285 torr is opened and gas escapes into the atmosphere with pressure of 768 torr What will the new volume of the gas be?
Demetrifairy
Ideal gas law is represented as pV = nRT
where p is absolute pressure
and V is volume of the container holding the gas
and n is the amount of gas in moles (a molecular unit of measure in chemistry)
and R is known as the universal gas constant
and T is the temperature of the gas in Kelvins (absolute temperature)
R is a constant (always), and so is 'n' in your particular scenario, since no gas is being added or subtracted during the compression of a closed Volume. You did not give a temperature, nor a change in temperature, so let T also be a constant in this case. The change in T is considered negligible (let's say it was compressed very slowly.)
Now let us solve the ideal gas law equation algebraically for p (pressure.)
pV = nRT
divide both sides by V, therefore
p = (nRT/V)
We have established that n, R, and T are constants for this problem. Let us set nRT equal to 1, for simplicity. 1 is a good constant, refusing to be anything but itself as no addition or subtraction is involved in our equation.
p = (1/V) or p is inversely proportional to Volume in our ideal gas scenario.
Solving for oneness (multiply both sides by V) to make our simplified equation: 1 = pV
p2V2 = p1V1
solving for p2
p2 = (p1V1/V2)
p2 = 3.4 Torr X (500 mL/302 mL)
p2 = 3.4 Torr x 1.656
p2 = 5.6 Torr
Wiki User
∙ 13y ago
Wiki User
∙ 15y agoThis question is a simple ratio Vi*Pi=Vf*Pf this equation can be re-written as:
Vf = (Vi*Pi)/Pf
Therefore:
Vf = (500mL*1285torr)/768torr = 836.59mL
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thrust
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Thrust (apex)
What happens to gas if it is not in a container?
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