Question

Using the Hoffman apparatus for electrolysis, a chemist decomposes 2.3 moles of water into its gaseous elements. How many grams of hydrogen gas should get (theoretical yield)? The chemist collected 2.0 moles hydrogen gas. What is his percent yield?

Answer 1

Answer:

2.318032g

Explanation:

-The electrolysis equation of water is written as below:

$2H_2O_{(l)}->2H_2_{(g)}+O_2_{(g)}$

-The mole ratio of Water to the hydrogen formed is 1:1, therefore 2.3 moles of hydrogen gas is produced.

-Hydrogen's molar mass is 1.00784 grams:

$Mass=moles\times molar \ mass\\\\\=2.3\times 1.00784\\\\=2.318032\ g$

Hence, 2.318032 grams of hydrogen is produced.