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Chemistry: Post your doubts here!

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in an experiment a sample of a pure gas is put into a gas syringe at a temperature of 300K and pressure of 16 kpa. the gas is compressed until the volume occupied by the gas is halved.
after the compression, the temperature of the gas in syringe is 375 and the pressure is 40 kpa.
is the gas is ideal
No it is not ideal as for a gas to be ideal it has to have high temperature and low pressure even though the temperature has rised its pressure has increased greatly.
 
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Umm i have a question i know its pretty silly etc but what do we do for a diatomic molecule like for example O2(oxygen) i get that it will have a Mr of 32 but what about the moles and volume would we consider 1 mol and 24dm3 for it?
 
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Umm i have a question i know its pretty silly etc but what do we do for a diatomic molecule like for example O2(oxygen) i get that it will have a Mr of 32 but what about the moles and volume would we consider 1 mol and 24dm3 for it?
Yes Mr will be 32 and will be considered 1 mol occupying 24dm³ of volume at room temp and pressure
 
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No it is not ideal as for a gas to be ideal it has to have high temperature and low pressure even though the temperature has rised its pressure has increased greatly.
It is ideal. If you use the equation. P1V1/T1 = P2V2/T2 you get that they are equal.

WORKING
----------------
V2 = v1/2(volume halved)

16V/300 = (40v/2)/375

You get the answer that both are equal
 
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oct nov 2008

Q 38. Which of the following would be suitable for use in a fire extinguisher?
1 CBrF 3
2 CH3(CH2)5CH2Br
3 HCl

Only statement 1 is correct, how come 2 isn't?
 
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oct nov 2008

Q 38. Which of the following would be suitable for use in a fire extinguisher?
1 CBrF 3
2 CH3(CH2)5CH2Br
3 HCl

Only statement 1 is correct, how come 2 isn't?

statement 2 also have a long hydrocarbon chain which is more flammable.
Thus provide no use as a fire extinguisher.
 
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