Answer:
54 g is the theoretical yield
Explanation:
This is the reaction:
2H₂ + O₂ → 2H₂O
So 2 moles of hydrogen react with 1 mol of oxygen, to produce 2 mol of water.
If I have 3 moles of H₂ and 2 moles of O₂, the my limiting reactant is the hydrogen.
1 mol of O₂ react with 2 moles of H₂
S 2 mol of O₂ would react with 4 moles (I only have 3 moles)
Then, ratio is 2:2 the same as 1:1
As 2 mol of H₂ produce 2 moles of water, 3 moles of H₂ will produce 3 moles of H₂O.
This is the theoretical yield in moles. Let's convert them to mass (mol . molar mass)
3 mol . 18g/m = 54 g
Answer:
The theoretical yield of the reaction is 54.06 grams
Explanation:
Step 1: Data given
Moles of hydrogen gas = 3.0 moles
Moles of oxygen gas = 2.0 mol
Molar mass of H2O = 18.02 g/mol
Step 2: The balanced equation
2H2 + O2 → 2H2O
Step 3: Calculate the limiting reactant
For 2 moles H2 consumed, we need 1 mol O2 to produce 2 moles of H2O
Hydrogen gas is the limiting reactant. It will be completely consumed. (3.0 moles).
Oxygen gas is in excess. There will react 3.0/2 = 1.5 moles of O2.
There will remain 2.0 -1.5 = 0.5 moles
Step 4: Calculate the moles of H2O
For 2 moles of H2 we'll have 2 moles of H2O
For 3 moles H2 we'll have 3.0 moles of H2O
Step 5: Calculate theoretical yield of H2O
Mass H2O = moles H2O * molar mass H2O
Mass H2O = 3.0 moles * 18.02 g/mol
Mass H2O = 54.06 grams
The theoretical yield of the reaction is 54.06 grams
