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juin [17]
2 years ago
5

What is the empirical formula of a compound that contains 25.92 percent nitrogen and 74.07 percent oxygen?

Chemistry
2 answers:
kvasek [131]2 years ago
7 0

Answer: N_2O_5

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 N = 25.92 g

Mass of O = 74.07 g

Step 1 : convert given masses into moles.

Moles of N =\frac{\text{ given mass of N}}{\text{ molar mass of N}}= \frac{25.92g}{14g/mole}=1.85moles

Moles of O =\frac{\text{ given mass of O}}{\text{ molar mass of O}}= \frac{74.07g}{16g/mole}=4.63moles

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

For N = \frac{1.85}{1.85}=1

For O =\frac{4.63}{1.85}=2.5

The ratio of Fe : O= 1:2.5

Converting them into whole numbers, the ratio will be 2: 5

Hence the empirical formula is N_2O_5

pychu [463]2 years ago
4 0

<span><span>N2</span><span>O5</span></span>

Explanation! 

When given %, assume you have 100 g of the substance. Find moles, divide by lowest count. In this case you'll end up with

<span><span>25.92 g N<span>14.01 g N/mol N</span></span>=1.850 mol N</span>

<span><span>74.07 g O<span>16.00 g O/mol O</span></span>=4.629 mol O</span>

The ratio between these is <span>2.502 mol O/mol N</span>, which corresponds closely with <span><span>N2</span><span>O5</span></span>.

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