Question

Find the number of moles of water that can be formed if you have 134 mol of hydrogen gas and 62 mol of oxygen gas

Answer 1

The number of moles of water that can be formed from 134 mol of hydrogen gas and 62 mol of oxygen gas is 124 moles because oxygen is the excess reactant, and it limits the production of water to twice its own amount.

Step-by-step explanation:

To find the number of moles of water that can be formed from 134 mol of hydrogen gas and 62 mol of oxygen gas, we look at the balanced chemical equation for the reaction:

2H₂(g) + O₂(g) → 2H₂O(g)

This reaction shows that two moles of hydrogen react with one mole of oxygen to produce two moles of water. This means that hydrogen is the limiting reactant since it will run out first. With this stoichiometry, half the number of moles of hydrogen will be required in moles of oxygen.

Since we have more moles of hydrogen available (134 mol) than twice the moles of oxygen (124 mol because 62 mol × 2 = 124 mol), oxygen is the excess reactant.

Therefore, we would use the full 62 moles of oxygen, which would require only 124 moles of hydrogen to react completely.

This results in 124 moles of water being produced.

Answer 2

164. You have excess hydrogen- you need double the number of moles hydrogen as oxygen because water has two hydrogens and only one oxygen while both hydrogen gas and oxygen gas are diatomic.

Because oxygen is diatomic, you spit it in half and basically double the number of moles, tack on your excess hydrogen, and you have 164 moles of water.

Edit: Lets look at it in one more way, taking into account what a mole is:

A mole is Avogadro's Constant number of particles- or about 6.02x10^23. So, we can multiply the number of moles you have to figure out how many particles of each we have. You can skip this step, because we will convert back to moles, but its illustrative of the concept.

6.02x10^23 x 174 moles H2 = 1.05 x 10^26 particles H2
6.02x10^23 x 82 moles O2 = 4.94 x 10^25 particles O2

I'm going to take one more step here- take them out of diatomic form. This will double the number of particles of each.

2.10 x 10^26 particles H+
9.88 x 10^25 particles O(2-)

Now, we know we need a 2:1 oxygen atom to hydrogen atom ration, so we devide and see oxygen is our limiting reagent. So, we have 9.88 x 10^25 single oxygen atoms, all of which will become water the hydr