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mihalych1998 [28]
3 years ago
6

A compound is found to consist of 34.5% sodium, 16.4% boron, and 48.6% oxygen. What is the empirical formula?

Chemistry
1 answer:
NARA [144]3 years ago
7 0

Answer: The empirical formula is NaBO_2

Explanation:

If percentage are given then we are taking total mass is 100 grams.

So, the mass of each element is equal to the percentage given:

Mass of Na= 34.5 g

Mass of B= 16.4 g

Mass of O = 48.6 g

Step 1 : convert given masses into moles.

Moles of Na =\frac{\text{ given mass of Na}}{\text{ molar mass of Na}}= \frac{34.5g}{23g/mole}=1.5moles

Moles of B =\frac{\text{ given mass of B}}{\text{ molar mass of B}}= \frac{16.4g}{11g/mole}=1.5moles

Moles of O =\frac{\text{ given mass of O}}{\text{ molar mass of O}}= \frac{48.6g}{16g/mole}=3moles

Step 2 : For the mole ratio, divide each value of moles by the smallest number of moles calculated.

For Na = \frac{1.5}{1.5}=1

For B = \frac{1.5}{1.5}=1

For O =\frac{3}{1.5}=2

The ratio of Na: B: O= 1: 1: 2

Hence the empirical formula is NaBO_2

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