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    Hi,

    can somebody plzz help me with this q

    C2F4 is obtained from CHClF2 according to the equation:

    2(CHClF2) <===> C2F4 + 2(HCL)

    a 1.0 mol sample of CHCLF2 is placed in a container of volume 18.5dm3 and heated.
    When the equilibrium is reached, the mixture contains 0.20 mol of CHClF2

    i)Calculate the number of moles of C2F4 & no of moles of HCL at equilibrium


    I know that HCL=0.8 and and C2F4 is 0.4 because i checked the mark scheme...but i have absolutely no clue how C2F4 = 0.4...in my answer i put 0.9 thinking it was that.

    Help?:confused:
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    Just consider the molar ratios
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    (Original post by Circularmover)
    Hi,

    can somebody plzz help me with this q

    C2F4 is obtained from CHClF2 according to the equation:

    2(CHClF2) <===> C2F4 + 2(HCL)

    a 1.0 mol sample of CHCLF2 is placed in a container of volume 18.5dm3 and heated.
    When the equilibrium is reached, the mixture contains 0.20 mol of CHClF2

    i)Calculate the number of moles of C2F4 & no of moles of HCL at equilibrium

    0.20 mol of CHClF2 at eqm means that 0.80 mol has reacted to form products. Therefore mol of C2F4 = 1/2 mol of CHClF2 reacted = 0.40 mol

    mol of HCL at eqm = mol of CHCLF2 reacted = 0.80 mol



    I know that HCL=0.8 and and C2F4 is 0.4 because i checked the mark scheme...but i have absolutely no clue how C2F4 = 0.4...in my answer i put 0.9 thinking it was that.

    Help?:confused:
    Hope that helps.
 
 
 
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