Question

Decomposition of hydrogen peroxide gives water and oxygen. How much of hydrogen peroxide is required to produce 48 g of oxygen?

Answer 1

Explanation:The molecular weight of hydrogen peroxide is 34 g/mol, and the molecular weight of oxygen is 32 g/mol.

Therefore, 48 g of oxygen is equal to 1.5 moles of oxygen.

To produce 1.5 moles of oxygen we must use 1.5 moles of hydrogen peroxide, which is equal to 51 g of hydrogen peroxide.

Answer 2

Step-by-step explanation:

To begin with, hydrogen peroxide breakdown must be done at a stoichiometric ratio.

2H2O2 -> 2H2O + O2

(Mass divided by molar mass Equals moles) - (48 / 16 = 3) 48g of oxygen is equivalent to about 3 moles of oxygen atoms.

Given that the reaction above produces a 1:1 ratio of hydrogen peroxide to oxygen atoms, 3 moles of hydrogen peroxide are required to create 3 moles of oxygen atoms (1.5 moles of diatomic oxygen).

The values of hydrogen and oxygen are thus added to determine the required quantity of hydrogen peroxide. 2 * 1.008 + 2 * 16 = 34.016g.

Hydrogen peroxide in 3 moles is equal to 3 * 34.016g.

In order to generate 48g of oxygen, 102.048g of hydrogen peroxide is required.

The volume of hydrogen peroxide is calculated by dividing the mass by the density.

So, 102.048g divided by 1.45g equals 70.3779310345mL.