Question

Reaction of gaseous fluorine with compound x yields a single product y, whose mass percent composition is 61.7% F and 38.3%Cl.

(a) What is a probable molecular formula for product Y, and what is a probable molecular formula for X?

(b) Draw an electron-dot structure for Y, and predict the geometry around the central atom.

(c) Caculate DeltaH for the synthesis of Y using the following information:

2ClF (g) +O2(g) -> Cl2O(g) + OF2 (g) dH=+205.4 kj/mol
2ClF3(l) + 2O2 (g) -> Cl2O(g) + 3OF2 (g) dH=+532.8 kj/mol

(d) How much heat in kj is released or absored in the reaction of 25.0g of X with a stoichiometric amount of F2, assuming 87.5% yield for the reaction?

Answer 1

a. Take a 100 g sample which gives you
61.7g Cl and 38.3 F.

Convert to mols.
61.7/19 = about 3.25
38.3/25.5 = about 1.1

Determine the empirical formula. The easy way to do this is to divide the smaller number by itself and divide the other number by the same small number.
3.25/1.08 = about 3
1.08/1.08 = 1 so the empirical formula is ClF3 and that is the most probable molecular formula.

b. We can't draw electron dot structures on this forum.

c. Add equation 1 to the reverse of equation 2 to find delta H for the reaction to produce ClF3.

d. Knowing the above, try d on your own.

Answer 2

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Answer 3

Binod

Answer 4

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Answer 6

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Answer 7

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