Question

1. If you had 1.73 moles of hydrogen (H2) and 0.89 moles of oxygen (O2), which would be the limiting reactant? How many moles of water can you produce from your supply of hydrogen and oxygen?

My answers:
H2 is the limiting reactant because it produces the least amount of product.

From my supply of H2, I can produce 1.73 mol H2O, and from my supply of O2, I can produce 1.78 mol H2O.

2. If you had 17.3 g of hydrogen and 89.1 g if oxygen, which is the limiting reactant, and how many grams of water could you produce?

My answers:
O2 is the limiting reactant.
10.0 g H2O could be produced.

Answer 1

For problem #2 the mass of oxygen is 8.91g, not 89.1 g.

Answer 2

1. You are right with your numbers BUT you make a huge error with your statement. Yes, you can produce 1.73 mols H2O from the hydrogen BUT you CAN'T produce 1.78 mols H2O from your supply of O2. No matter how you slice it, you can produce ONLY as much as the limiting reagent will allow so you can produce 1.73 mols H2O, period no matter how much more oxygen you had.

2. I think you made a decimal error in 2. I believe that is 100 g H2O and not 10.0. Check it out to make sure.

Answer 3

So disregard my answer to 2.

Answer 4

If you had 1.85 moles of hydrogen (H2) and 0.86 moles of Oxygen(O2) which would be the limiting reactant? How many moles of water can you produce from your supply of hydrogen and Oxygen?