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A compound that contains only carbon, hydrogen, and oxygen is composed of 48.64% C and 43.2% O by mass. What is the empirical formula of this compound?
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6. Chemical Reactions & Quantities
Empirical Formula
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Elemental analysis of a sample of an ionic compound showed 2.82 g of Na, 4.35 g of Cl, and 7.83 g of O. What is the empirical formula of the compound?
A
NaClO
B
NaClO2
C
NaClO3
D
NaClO4
Guida verificata passo dopo passo1
Step 1: Determine the number of moles of each element in the compound. Use the molar mass of each element: Na (22.99 g/mol), Cl (35.45 g/mol), and O (16.00 g/mol). Calculate the moles of Na, Cl, and O by dividing the given mass of each element by its molar mass.
Step 2: Calculate the moles of sodium (Na) by dividing 2.82 g by 22.99 g/mol.
Step 3: Calculate the moles of chlorine (Cl) by dividing 4.35 g by 35.45 g/mol.
Step 4: Calculate the moles of oxygen (O) by dividing 7.83 g by 16.00 g/mol.
Step 5: Determine the simplest whole number ratio of moles of each element by dividing each mole value by the smallest number of moles calculated in the previous steps. This will give you the empirical formula of the compound.
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