Question

Cuantas moléculas de oxigeno se producen por la descomposición de 28.5 g de H2O2 (masa molecular = 34.0g/mol) de acuerdo a la ecuación

2H2O2(l) → 2H2O(l)+O2(g)

Answer 1

The question is as follows: How many oxygen molecules are produced by the decomposition of 28.5 g of H2O2 (molecular mass = 34.0g / mol) according to the equation

2H2O2 (l) → 2H2O (l) + O2 (g)

Answer: There are
`2.52 * 10^(23)` molecules are produced by the decomposition of 28.5 g of
`H_(2)O_(2)` according to the equation
`2H_(2)O(l) \rightarrow 2H_(2)O(l) + O_(2)(g)`.

Step-by-step explanation:

Given: Mass of
`H_(2)O_(2)` = 28.5 g

As moles is the mass of a substance divided by its molar mass. Hence, moles of
`H_(2)O_(2)` is calculated as follow.

`Moles = (mass)/(molarmass)\\= (28.5 g)/(34.0 g/mol)\\= 0.838 mol`

According to the given equation, 2 moles of
`H_(2)O_(2)` gives 1 mole of
`O_(2)`. So, moles of
`O_(2)` produced by 0.838 moles of
`H_(2)O_(2)` will be calculated as follows.

`Moles of O_(2) = (0.838 mol)/(2)\\= 0.419 mol`

This means that moles of
`O_(2)` produced is 0.419 mol.

As per the mole concept, 1 mole of every substance has
`6.022 * 10^(23)` molecules.

So, molecules of
`O_(2)` present in 0.419 mole are as follows.

`0.419 * 6.022 * 10^(23)\\= 2.52 * 10^(23)`

Thus, we can conclude that there are
`2.52 * 10^(23)` molecules are produced by the decomposition of 28.5 g of
`H_(2)O_(2)` according to the equation
`2H_(2)O(l) \rightarrow 2H_(2)O(l) + O_(2)(g)`.