Thirty moles of helium (Mr = 4) occupy a volume of 0.20 m3 at a pressure...
Thirty moles of helium (Mr = 4) occupy a volume of 0.20 m3 at a pressure of 4.0 × 105 Pa. If the volume is halved and the temperature is increased by 40 K, what is the new pressure of the gas?
Homework Answers
To describe the behaviour of Helium at various conditions, we can use the ideal Gas Law
where 
is the universal gas constant, equal to 
in SI units.
When the conditions are changed, the temperature is said to be
increased by 
from the original temperature.
However, we do not know the original temperature, so we use the ideal gas relation temperature to find it.
Thus, the final temperature is 
The final volume occupied is 
Rearranging the equation for pressure, we get
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Thirty moles of helium (Mr = 4) occupy a volume of 0.20 m3 at a
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