Hydrogen peroxide is composed of two elements: hydrogen and oxygen. In an experiment, 1.250 g of hydrogen peroxide is fully decomposeed. If 0.074g of hydrogen are obtained, what about Oxygen?

To find the amount of oxygen obtained, we first need to calculate the molar mass of hydrogen peroxide (H2O2).

Molar mass of H = 1.008 g/mol
Molar mass of O = 16.00 g/mol

Molar mass of H2O2 = 2(1.008) + 2(16.00) = 34.016 g/mol

Next, we need to calculate the moles of hydrogen obtained:

0.074 g / 1.008 g/mol = 0.0734 mol

Since the ratio of hydrogen to oxygen in hydrogen peroxide is 2:2, we know that for every 2 moles of hydrogen obtained, 1 mole of oxygen is obtained.

Therefore, the moles of oxygen obtained is half of the moles of hydrogen obtained:

0.0734 mol / 2 = 0.0367 mol

Finally, we can calculate the mass of oxygen obtained:

0.0367 mol x 16.00 g/mol = 0.5872 g

Therefore, 0.5872 g of oxygen are obtained in the experiment.

Step 1: Calculate the mass of oxygen in hydrogen peroxide

Mass of hydrogen peroxide = Mass of hydrogen + Mass of oxygen

Mass of oxygen = Mass of hydrogen peroxide - Mass of hydrogen

Mass of oxygen = 1.250 g - 0.074 g = 1.176 g

Step 2: Calculate the percentage of oxygen in hydrogen peroxide

Percentage of oxygen = (Mass of oxygen / Mass of hydrogen peroxide) x 100%

Percentage of oxygen = (1.176 g / 1.250 g) x 100% = 94.1%

Conclusion:

The original hydrogen peroxide sample contains 1.176 g of oxygen, which corresponds to 94.1% of the total mass.