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skylarladson2549
17.10.2020 •
Chemistry
A compound containing only carbon, hydrogen, and oxygen is analyzed using combustion analysis. When 50.1 g of the compound is burned, 91.8 g of carbon dioxide and 25.1 g of water are collected. In order to determine the moles of carbon in the compound, first determine the moles of carbon dioxide that were produced from the combustion.
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Ответ:
Explanation:
Hello,
In this case, since the carbon of the initial compound is present in the carbon dioxide product, we can compute the mass and moles of carbon in the compound:
Next, the mass and moles of hydrogen in the compound, is contained in the yielded amount of water, thus, we compute the mass and moles of hydrogen in the compound:
In such a way, the mass of oxygen comes from the mass of the compound minus the mass of carbon and oxygen:
And the moles:
Then, we compute the subscripts by diving the moles of C, H and O by the moles of oxygen as the smallest moles:
After that, we write:
Which must be shown in whole number only, thereby we multiply the subscripts by 2, so the empirical formula turns out:
Best regards.
Ответ:
1.16L can be made
Explanation:
Molarity = Mol / Volume
Volume = Mol / Molarity
Let's determine the moles of salt, with that mass:
130 g FeCl₂ . 1mol / 126.75 g = 1.02 moles of FeCl₂
Volume = 1.02 mol / 0.88 mol/L → 1.16L