Question

Calculate the mass of unreacted oxygen gas. If 100g of oxygen gas is passed to burn 10g of hydrogen gas to water. Also determine the amount of water produced

Answer 1

If this is a numerical problem, then the answer is that 10g or 5 moles of Hydrogen react with 2.5 moles of Oxygen to form 5 moles of water, or 5×18=90g of water. Here is the required reaction:

H2(5mol.)+12O2(2.5mol.)→H2O(5mol.)

In reality, if 10g of hydrogen is burned with excess Oxygen, instead of water, Hydrogen Peroxide would be formed.

And stoichiometrically, with 10g of Hydrogen, that is 5 moles of Hydrogen, 5 moles of H2O2 would be formed. That is 5×34=170g of H2O2

Here is the required reaction:

H2(5mol.)+O2(5mol.)→H2O2(5mol.)