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Leona [35]
2 years ago
9

The empirical formula for this compound that contain 31.14%sulfur and 68.86%chlorine by mass

Chemistry
1 answer:
Kaylis [27]2 years ago
5 0

The empirical formula is SCl_2.

The <em>empirical formula</em> (EF) is the simplest whole-number ratio of atoms in a compound.

The ratio of atoms is the same as the ratio of moles.

So, our job is to calculate the <em>molar ratio </em>of S to Cl.

Assume that you have 100 g of sample.

Then it contains 31.14 g S and 68.86 g Cl.

<em>Step</em> 1. Calculate the <em>moles of each element</em>

Moles of S = 31.14 g S × (1 mol S/(32.06 g S) = 0.971 30 mol S  

Moles of Cl = 68.86 g Cl × (1 mol Cl/35.45 g Cl) = 1.9425 mol Cl

<em>Step 2</em>. Calculate the <em>molar ratio</em> of each element

Divide each number by the smallest number of moles and round off to an integer

S:Cl = 0.971 30: 1.9425 = 1:1.9998 ≈ 1:2

<em>Step 3</em>: Write the <em>empirical formula</em>

EF = SCl_2

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Hello,

In this case, for computing the atom percent, one must obtain the number of atoms of silver, gold and copper as shown below:

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\% atAg=\frac{1.15x10^{26}}{1.15x10^{26}+1.16x10^{26}+2.71x10^{25}}*100\% =44.6\%\\\% atAu=\frac{1.16x10^{26}}{1.15x10^{26}+1.16x10^{26}+2.71x10^{25}}*100\% =44.9\%\\\% atCu=\frac{2.71x10^{25}}{1.15x10^{26}+1.16x10^{26}+2.71x10^{25}}*100\% =10.5\%

Best regards.

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