Question

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A 22.98 g sample of a compound contains 7.33 g of potassium, K, 6.65 g of chlorine, Cl, and oxygen, O. Calculate the empirical formula.

Insert subscripts as needed.

Empirical formula: KClO

Answer 1

`KClO_3`

Step-by-step explanation:

Hello!

In this case, as we know the mass of the total sample, we can first compute the mass of oxygen:

`m_O=22.9g-7.33g-6.65g=8.92g`

Next, we compute the moles of each element:

`n_K=(7.33g)/(39.9g/mol)= 0.184mol\\\\n_(Cl)=(6.65g)/(35.45g/mol)=0.188mol \\\\n_O=(8.92g)/(16.00g/mol) =0.5575mol`

Now, we divide the moles by 0.184 moles, the fewest ones, to obtain:

`K=(0.184)/(0.184)=1.0 \\\\Cl=(0.187)/(0.184)=1.0\\\\O=(0.5575)/(0.184) =3.0`

Therefore, the empirical formula is:

`KClO_3`

Regards!