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QveST [7]
3 years ago
7

A sample of a compound contains 3.21 g of sulfur and 11.4 g of fluorine. Which of the following represents the empirical formula

of the compound?
(A) SF2 (B) SF3 (C) SF4 (D) SF5 (E) SF6
Chemistry
1 answer:
Sergeeva-Olga [200]3 years ago
7 0

Answer:

The empirical formula is SF6 (option E)

Explanation:

Step 1: Data given

Mass of sulfur = 3.21 grams

Mass of fluorine = 11.4 grams

Molar mass sulfur = 32.065 g/mol

Molar mass fluorine = 19.00 g/mol

Step 2: Calculate moles

Moles = mass /molar mass

Moles sulfur = 3.21 grams / 32.065 g/mol

Moles sulfur = 0.100 moles

Moles fluorine = 11.4 grams / 19.00 g/mol

Moles fluorine = 0.600 moles

Step 3: Calculate mol ratio

We divide by the smallest amount of moles

S: 0.100 / 0.100 = 1

F : 0.600 / 0.100 = 6

The empirical formula is SF6 (option E)

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Which of the following pairs of elements could possibly be in the same group? X has a 1+ ion; Y has a 1- ion. X tends to form a
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What is the molarity of solution that is 5.50 percentage by mass oxalic acid and has a density of 1.024 g/ml
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Answer:

0.6257 M is the molarity of solution that is 5.50 percentage by mass oxalic acid.

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Mass percentage of oxalic acid = 5.50%

This means that in 100 grams of solution there are 5.50 grams of oxalic acid.

Mass of solution , m = 100

Volume of the solution = V

Density of the solution = d = 1.024 g/mL

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=\frac{0.06111 mol}{0.09766  L}=0.6257M

0.6257 M is the molarity of solution that is 5.50 percentage by mass oxalic acid.

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