An unknown compound contains only carbon, hydrogen, and oxygen (cxhyoz). combustion of 3.50 g of this compound produced 5.13 g of carbon dioxide and 2.10 g of water.how many moles of hydrogen, h, were in the original sample?

The combustion reaction of the unknown compound can be written as follows:

Other part of the question is discussed below:

We know that 3.50 g of the compound produced 5.13 g of carbon dioxide and 2.10 g of water. This means that 1.63 g of oxygen were also produced in the reaction.

The mass of oxygen in the original sample is equal to the mass of oxygen produced in the reaction, so the original sample contained 1.63 g of oxygen.

The total mass of carbon and hydrogen in the original sample is equal to the mass of the sample minus the mass of oxygen, which is 3.50 g - 1.63 g = 1.87 g.

We can find the number of moles of hydrogen in the original sample by dividing the mass of hydrogen by the molar mass of hydrogen (1.008 g/mol). This gives us 1.87 g / 1.008 g/mol = 1.86 moles of hydrogen.

Therefore, the answer is 1.86

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Final answer:

By dividing the mass of water produced in combustion by the molar mass of Hydrogen in water, we find that the original compound contained 1.05 mol of Hydrogen.

Explanation:

To determine the mole amount of Hydrogen in the compound, you have to consider the reaction applied, and how it applies to the law of conservation of mass. Combustion of the compound produces carbon dioxide (CO2) and water (H2O). For water, one mol equals to the molar mass of H which is 1 g/mol, times the amount of H in water which is 2 to get 2 g/mol. Now knowing that 2.10 g of water were produced from combustion, we divide this by the molar mass of H-in-water to get the number of hydrogen moles in the original sample. So, the calculation will be 2.10 g/ 2 (g/mol) = 1.05 mol. So, the original compound contained 1.05 mol of hydrogen.

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