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A sample of gas contains 0.1700 mol of OF2(g) and 0.1700 mol of H2O(g) and occupies a volume of 19.5 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

User Cloyd Abad
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1 Answer

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Answer: The volume of the sample after the reaction takes place is 29.25 L.

Step-by-step explanation:

The given reaction equation is as follows.


OF_(2)(g) + H_(2)O(g) \rightarrow O_(2)(g) + 2HF(g)

So, moles of product formed are calculated as follows.


(3)/(2) * 0.17 mol \\= 0.255 mol

Hence, the given data is as follows.


n_(1) = 0.17 mol,
n_(2) = 0.255 mol


V_(1) = 19.5 L,
V_(2) = ?

As the temperature and pressure are constant. Hence, formula used to calculate the volume of sample after the reaction is as follows.


(V_(1))/(n_(1)) = (V_(2))/(n_(2))

Substitute the values into above formula as follows.


(V_(1))/(n_(1)) = (V_(2))/(n_(2))\\(19.5 L)/(0.17 mol) = (V_(2))/(0.255 mol)\\V_(2) = (19.5 L * 0.255 mol)/(0.17 mol)\\= (4.9725)/(0.17) L\\= 29.25 L

Thus, we can conclude that the volume of the sample after the reaction takes place is 29.25 L.

User Zoltan Ersek
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