# A-level Chemistry Mock QuestionWatch

#1
Can anyone help me out with this chemistry question?

Compound A is an oxide of chlorine that is liquid at room temperature and pressure and has a boiling point of 83 degrees.

When 0.4485g of A is heated to 100 degrees C at 1.00x10^5 Pa, 76.0cm3 of gas is produced.

Determine the molecular formula of compound A.

I've got the number of moles of gas produced from pv=nrt, but I'm not sure how to proceed. :/
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3 weeks ago
#2
Rearrange pv=nrt to find n=pv/rt. From that you can work out the Mr of the compound.
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#3
(Original post by VictiniCup)
Rearrange pv=nrt to find n=pv/rt. From that you can work out the Mr of the compound.
Really sorry would you mind explaining how you work out the molecular formula of the compound after finding the moles from pv=nrt.
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3 weeks ago
#4
(Original post by Eli-Grey)
Really sorry would you mind explaining how you work out the molecular formula of the compound after finding the moles from pv=nrt.
You could use n=m/Mr
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3 weeks ago
#5
you have moles and mass, use mass/moles = Mr then deduce how many Chlorines and Oxygens fit into it (theres probably an easier to do it than that)
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#6
(Original post by amaraub)
you have moles and mass, use mass/moles = Mr then deduce how many Chlorines and Oxygens fit into it (theres probably an easier to do it than that)
oh cool thanks
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