AQA Chemistry empirical formula
This question is about citric acid, a hydrated tricarboxylic acid. Its formula can be represented as H3Y..𝑥H2O
0 8 . 1 A 1.50 g sample of H3Y..𝑥H2O contains 0.913 g of oxygen by mass.
The sample burns completely in air to form 1.89 g of CO2 and 0.643 g of H2O Show that the empirical formula of citric acid is C3H5O4
Why do you times the number of moles of H2O by 2 to get the moles of H atoms which is 0.0357x2=0.0714 ? Why wouldn't you divide as H2O has 2 H atoms?
0 8 . 1 A 1.50 g sample of H3Y..𝑥H2O contains 0.913 g of oxygen by mass.
The sample burns completely in air to form 1.89 g of CO2 and 0.643 g of H2O Show that the empirical formula of citric acid is C3H5O4
Why do you times the number of moles of H2O by 2 to get the moles of H atoms which is 0.0357x2=0.0714 ? Why wouldn't you divide as H2O has 2 H atoms?
Original post by anon25x
This question is about citric acid, a hydrated tricarboxylic acid. Its formula can be represented as H3Y..𝑥H2O
0 8 . 1 A 1.50 g sample of H3Y..𝑥H2O contains 0.913 g of oxygen by mass.
The sample burns completely in air to form 1.89 g of CO2 and 0.643 g of H2O Show that the empirical formula of citric acid is C3H5O4
Why do you times the number of moles of H2O by 2 to get the moles of H atoms which is 0.0357x2=0.0714 ? Why wouldn't you divide as H2O has 2 H atoms?
0 8 . 1 A 1.50 g sample of H3Y..𝑥H2O contains 0.913 g of oxygen by mass.
The sample burns completely in air to form 1.89 g of CO2 and 0.643 g of H2O Show that the empirical formula of citric acid is C3H5O4
Why do you times the number of moles of H2O by 2 to get the moles of H atoms which is 0.0357x2=0.0714 ? Why wouldn't you divide as H2O has 2 H atoms?
If you have 1 mol of water molecules then you have 2 moles of hydrogen atoms.
You determine the moles of water and then multiply by 2 to get the moles of hydrogen atoms.
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