How many grams of oxygen are required to produce 56.0 g water vapor?

A worked example. Just follow the steps.

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To determine the number of grams of oxygen required to produce 56.0 g of water vapor, you need to consider the chemical formula for water and the molar mass of oxygen.

The chemical formula for water is H2O, which means that each molecule of water consists of two hydrogen atoms and one oxygen atom.

The molar mass of oxygen (O) is approximately 16.00 g/mol.

To calculate the grams of oxygen required, you can use the following steps:

Step 1: Determine the number of moles of water vapor by dividing the given mass of water vapor (56.0 g) by its molar mass. The molar mass of water (H2O) is approximately 18.02 g/mol, which is calculated by adding the molar masses of hydrogen (1.01 g/mol) and oxygen (16.00 g/mol).

Moles of water vapor = Mass of water vapor / Molar mass of water

Moles of water vapor = 56.0 g / 18.02 g/mol

Moles of water vapor ≈ 3.11 mol

Step 2: Since each water molecule contains one oxygen atom, the number of moles of oxygen atoms is equal to the number of moles of water vapor.

Moles of oxygen = Moles of water vapor ≈ 3.11 mol

Step 3: To calculate the mass of oxygen required, multiply the number of moles of oxygen by its molar mass.

Mass of oxygen = Moles of oxygen * Molar mass of oxygen

Mass of oxygen ≈ 3.11 mol * 16.00 g/mol

Mass of oxygen ≈ 49.76 g

Therefore, approximately 49.76 grams of oxygen are required to produce 56.0 grams of water vapor.