Answer:
13.39 g of H₂O
Solution:
The Balance Chemical Reaction is as follow,
2 H₂ + O₂ → 2 H₂O
Step 1: Find out the limiting reagent as;
According to Equation ,
4.032 g (2 mole) H₂ reacts with = 32 g (1 moles) of O₂
So,
1.5 g of H₂ will react with = X g of O₂
Solving for X,
X = (1.5 g × 32 g) ÷ 4.032 g
X = 11.90 g of O₂
It means for total oxidation of Hydrogen we require 11.90 g of O₂, but we are provided with 12 g of O₂. Therefore, H₂ is the limiting reagent and will control the yield.
Step 2: Calculate Amount of H₂O produced as;
According to Equation ,
4.032 g (2 mole) H₂ produces = 36 g (2 moles) of H₂O
So,
1.50 g of H₂ will produce = X g of H₂O
Solving for X,
X = (1.50 g × 36 g) ÷ 4.032 g
X = 13.39 g of H₂O
And this answer is correct.
