Hey sample of helium occupies 235 ml at 788 tour and 25°c. if the sample is condensed into a 0.115 l flask what will be the new pressure assuming constant temperature?

The new pressure of helium gas assuming constant temperature is equal to 1610.26 Torr.

Given the following data:

Conversion:

Initial volume = 235 mL to L =

To determine the new pressure assuming constant temperature, we would apply Boyle's law:

Mathematically, Boyle's law is given by the formula;

Where;

Substituting the given parameters into the formula, we have;

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the system is in constant temperature

so it follows Boyle's law

i.e.P1V1=P2P2

where P1=initial pressure=788 tour

P2=final pressure= ?

V1=initial volume=235 ml

V2=final volume=0.115 ml

it should have an internal chamber and two thermometers sticking out of the top. the internal chamber will also be closed off from the outside.