Question

Gaseous hydrogen and oxygen can be prepared in the laboratory from the decomposition of gaseous water.

The equation for the reaction is

2H2O(g)⟶2H2(g)+O2(g)

Calculate how many grams of O2(g) can be produced from 58.9 g H2O(g).

Answer 1

Mass of oxygen = 52.32 g

Step-by-step explanation:

Given data:

Mass of water = 58.9 g

Mass of oxygen produced = ?

Solution:

Chemical equation:

2H₂O → 2H₂ + O₂

Number of moles of water:

Number of moles = mass/ molar mass

Number of moles = 58.9 g/ 18 g/mol

Number of moles = 3.27 mol

Now we will compare the moles of water with oxygen from balance chemical equation.

H₂O : O₂

2 : 1

3.27 : 1/2×3.27 = 1.635 mol

Mass of oxygen produced:

Mass = number of moles × molar mass

Mass = 1.635 mol × 32 g/mol

Mass = 52.32 g