Compute for the mass percent composition of elements in water (H2O).
In our previous lesson, we already identify the mass of both hydrogen and oxygen for 1 mole of water: H2 = 2.02 g/mol and O = 16.00 g/mol. While the molar mass of water is 18.02 g/mol.
With this, let us use the formula for % mass that we have above.
% mass = ( total mass of element / molar mass ) X 100
% of Hydrogen in water = ( 2.02 g/mol / 18.02 g/mol ) X 100 = ______ % (answer rounded-off to 2-decimal places)
% of Oxygen in water = (16.00 g/mol / 18.02 g/mol ) X 100 = ______ % (answer rounded-off to 2-decimal places)
In our previous lesson, we already identify the mass of both hydrogen and oxygen for 1 mole of water: H2 = 2.02 g/mol and O = 16.00 g/mol. While the molar mass of water is 18.02 g/mol.
With this, let us use the formula for % mass that we have above.
% mass = ( total mass of element / molar mass ) X 100
% of Hydrogen in water = ( 2.02 g/mol / 18.02 g/mol ) X 100 = ______ % (answer rounded-off to 2-decimal places)
% of Oxygen in water = (16.00 g/mol / 18.02 g/mol ) X 100 = ______ % (answer rounded-off to 2-decimal places)
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Explanation:
Now, mass of an element in a given mass of compound = (atomic mass of the element × number of atoms of the element in one molecule of the compound) × given mass of compound / molar mass of the compound. Hope, this helps.