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Answer:

[tex]oxygen \: at \: 94.1\% \: hydrogen \: at \: 5.9\% \\ at \: 100gram \: oxygen \: \\ \: 94.1\% = .941 \times 100g \\ = 94.1 \times \frac{1mol}{16g} = 5.88g \\ hydrogen \: \\ 5.9\% = .059 \times 100 = 5.9 \times \frac{1mol}{1.002g} = 5.88g \\ here \: oxygen = hydrogen \: so \: ratio \\ = 1 \: \: \: 1 \: \\ emperical \: formula \: = oh\\ thank \: you[/tex]

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Composition:

5.9% Hydrogen and 94.1% Oxygen (by mass)

in a 100 gram sample:

5.9 gram Hydrogen

94.1 gram Oxygen

Finding the number of moles:

Moles of Hydrogen:

moles = given mass/ molar mass

moles = 5.9 / 1          [molar mass of Hydrogen = 1g/mol]

moles of hydrogen = 5.9 moles

Moles of Oxygen:

number of moles = given mass / molar mass

number of moles  = 94.1 / 16          [molar mass of Oxygen = 16g/mol]

moles of Oxygen = 5.88 ≈ 5.9 moles

Empirical Formula:

Moles of Hydrogen : Moles of Oxygen

5.9 : 5.9

Moles of Hydrogen : Moles of Oxygen = 1:1

Empirical Formula = OH

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