Hydrogen-filled balloon was ignited and 1.50 g of hydrogen reacted with 12.0 g of oxygen. how many grams of water vapor formed? (assume that water vapor is the only product.)

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.