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A compound containing only carbon, hydrogen, and oxygen is analyzed using combustion analysis. When 50.1 g of the compound is burned, 89.3 g of carbon dioxide and 36.6 g of water are collected.

Given that there are 21.6 g of oxygen in the original compound, determine the number of moles of oxygen in the original compound.

Sagot :

Answer:

1.35mol

Explanation:

To determine the number of moles of oxygen in the original compound, we can follow these steps:

Calculate the moles of carbon and hydrogen in the compound.

Calculate the moles of oxygen that are part of the compound.

Step 1: Calculate the Moles of Carbon and Hydrogen

From CO₂:

Given:

Mass of CO₂ produced = 89.3 g

Molar mass of CO₂ (C: 12.01 g/mol, O₂: 2 * 16.00 g/mol = 32.00 g/mol) = 44.01 g/mol

Moles of CO₂=Mass of CO₂/Molar mass of CO₂= 89.3g/44.01 g/mol=2.029mol

Since each mole of CO₂ contains 1 mole of carbon, the moles of carbon in the original compound are:

Moles of C=2.029mol

From H₂O:

Given:

Mass of H₂O produced = 36.6 g

Molar mass of H₂O (H: 2 * 1.01 g/mol = 2.02 g/mol, O: 16.00 g/mol) = 18.02 g/mol

Moles of H₂O=Mass of H₂O/Molar mass of H₂O=36.6g/18.02g/mol=2.03

mol

Since each mole of H₂O contains 2 moles of hydrogen, the moles of hydrogen in the original compound are:

Moles of H =2×2.03mol=4.06mol

Step 2: Calculate the Mass of Carbon and Hydrogen in the Compound

Mass of Carbon:

Mass of C=Moles of C×Molar mass of C=2.029mol×12.01g/mol=24.36g

Mass of Hydrogen:

Mass of H=Moles of H×Molar mass of H=4.06mol×1.01g/mol=4.10g

Step 3: Calculate the Mass of Oxygen in the Compound

Given:

Total mass of the compound = 50.1 g

Mass of oxygen in the compound = 21.6 g (given)

Step 4: Calculate the Moles of Oxygen in the Compound

Moles of O=Mass of O/Molar mass of O=21.6g/16.00g/mol=1.35 mol

So, the number of moles of oxygen in the original compound is 1.35mol

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