Question

Calculate the empirical formula of a 15g sample of a compound which is found to contain 58.87% sodium and 41.13% sulfur.​

Answer 1

Answer:

You know that your compound contains 2.82 g of sodium, 4.35 g of chlorine, and 7.83 g of oxygen.

What you do next is use each element's molar mass to try and find how many moles of each you get in that sample of the compound.

In this case, you have

For Na:

2.82

g

23.0

g

mol

=

0.1226 moles Na

For Cl:

4.35

g

35.45

g

mol

=

0.1227 moles Cl

For O:

7.83

g

16.0

g

mol

=

0.4894 moles O

Answer 2

Answer:

You are aware of the amounts of 2.82 g of sodium, 4.35 g of chlorine, and 7.83 g of oxygen in your compound.Thus, the empirical formula, which identifies the least integer ratio of atoms in a compound, will be $NaClO4$

Explanation:

Calculate each element's molecular weight in grammes. 2. Dividing each element's mole value by the tiniest mole value will reveal the simplest ratio. A 1 to 1 ratio will be ensured as a result. 3. If any of the mole ratios are not whole numbers, you must multiply them by a whole number to get a whole number ratio. 4. Recognizing the decimal versions of typical fractions and multiplying by the denominator are useful.

You are aware of the amounts of sodium, chlorine, and oxygen in your compound: 2.82 g, 4.35 g, and 7.83 g.The next step is to try and determine how many moles of each element you have in that sample of the compound using the molar masses of each element.You have in this situation

$For Na:\frac{2.82g}{23.0g/mol}=0.1226 moles Na$

$For Cl:\frac{4.35g}{35.45g/mol} =0.1227 moles Cl$

$For O:\frac{7.83g}{16.0g/mol} =0.4894 moles O$

Thus, the empirical formula, which identifies the least integer ratio of atoms in a compound, will be

$Na1Cl1O4, or NaClO4$

To learn more about sodium, visit:

https://brainly.in/question/37750455

To learn more about chlorine, visit:

https://brainly.in/question/605912

#SPJ2