I need help solving this problem!! Please be detailed

Question

If 50.0g of H₂ and 100.0g of O₂ react, how many moles of H₂O can be produced in the reaction below?

2H₂(g) + O₂(g)= 2H₂O(g)

Answer 1

Any time you are given the quantities of BOTH reactants, you will be dealing with a limiting reactant problem. That is to say, you should find out which reactant is in limited supply and use that to determine how much product you can form.

In this problem we will calculate how many moles of H2O can be formed from 50.0 g of H2 and also from 100.0 g of O2. Whichever is the lower amount will be the limiting reactant and will provide the final answer.

2H₂(g) + O₂(g) ==> 2H₂O(g) we will now use dimensional analysis (unit factor method)...

For H₂: 50.0 g H₂ x 1 mol H₂/2.00 g x 2 mol H₂O/2 mol H₂ = 50.0 moles H₂O formed

For O₂: 100.0 g O₂ x 1 mol O₂/32 g x 2 mol H₂O/mol O₂ = 6.25 moles H₂O formed

So clearly, O₂ is limiting and 6.25 moles of H2O will be formed in the reaction