Question

2.56 g of hydrogen reacts completely with 20.3 g of oxygen to form X g of water. X =___g

Answer 1

Answer:

22.9g of H₂O are produced

Explanation:

The reaction of hydrogen with oxygen is:

2H₂(g) + O₂(g) → 2H₂O(g)

Where 2 moles of hydrogen react with 1 mole of oxygen to produce 2 moles of water

Moles of hydrogen are:

2.56g × (1mole / 2.01g) = 1.27moles H₂

Moles of oxygen are:

20.3g × (1mole / 32g) = 0.634moles O₂

These moles of oxygen react with:

0.634moles O₂ × (2mol H₂ / 1mol O₂) = 1.27mol H₂

-All hydrogen in reaction-

And produce:

0.634moles O₂ × (2mol H₂O / 1mol O₂) = 1.27mol H₂O

In grams:

1.27mol H₂O × (18.01g / 1mol) = 22.9g of H₂O are produced

Answer 2

Answer:

X = 22.9 g of water produced.

Explanation:

Reaction equation:

$H_{2} + \frac{1}{2}O_{2}$ → $H_{2}O$

1 mole of H2 - 2.016 g

?? mole of H2 - 2.56g = 1.27 moles in 2.56g of hydrogen

Since hydrogen is the limiting reactant, we'll use it to determine the mass of water produced.

Mole ratio of hydrogen to water is 1:1 (that is, 1 mole of hydrogen gives 1 mole of water. Consequently, 1.27 mole of H2 = 1.27 moles of H2O)

1 mole of water - 18.05 g

1.27 mole of H2O - X g

⇒ 1.27 × 18.05

X  = 22.9 g of water produced.