A sample of gas contains 0.1600 mol of C2H4(g) and 0.1600 mol of Br2(g) and occu

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A sample of gas contains 0.1600 mol of C2H4(g) and 0.1600 mol of Br2(g) and occupies a volume of 10.4 L. The following reaction takes place:


C2H4(g) + Br2(g)CH2BrCH2Br(g)

Calculate the volume of the sample after the reaction takes place, assuming that the temperature and the pressure remain constant.
May 29th, 2015

Solution:

According with Avogadro's Law (The Volume Amount Law)

(V1 / n1 = V2 / n2)

before the reaction takes place the total number of moles is = 0.16+0.16= 0.32 moles 

and the volume is 10.4 L

According to the balanced chemical equation, 1 mol of C2H4(g) produces 1 mol of CH2BrCH2Br(g)

then 0.16 mol of C2H4(g) produces 0.16 mol of CH2BrCH2Br(g)

then the number of moles after the reaction is 0.16 

Now we can solve the avogadro´s law for V2

V2=V1n2/n1

V2= (10.4L)*(0.16mol)/(0.32mol)= 5.2 L

The Volume after the reaction is 5.2 L



May 29th, 2015

can you do this one for me please! 

A sample of gas contains 0.1200 mol of OF2(g) and 0.1200 mol of H2O(g) and occupies a volume of 7.92 L. The following reaction takes place:

OF2(g) + H2O(g)O2(g) + 2HF(g)

Calculate the volume of the sample after the reaction takes place, assuming that the temperature and the pressure remain constant.

 L

May 29th, 2015

Of course just put the question and select my BID I´ll put the lowest BID=1.00

May 29th, 2015

don't have any cash on me now . 

May 29th, 2015

You can put an easy question (I think is free) and I´ll answer your question

May 29th, 2015

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