Calculate the mass of oxygen that will be released during the decomposition of 3.6 g of water under

Calculate the mass of oxygen that will be released during the decomposition of 3.6 g of water under the influence of a constant electric current.

1.The decomposition of water under the action of an electric current occurs according to the equation:

2H2O = 2H2 + O2;

2.n (H2O) = m (H2O): M (H2O);

M (H2O) = 1 * 2 + 16 = 18 g / mol;

n (H2O) = 3.6: 18 = 0.2 mol;

3.in accordance with the coefficients in the equation, oxygen forms half as much as water decomposes:

n (O2) = n (H2O): 2 = 0.2: 2 = 0.1 mol;

4.Calculate the mass of the oxygen obtained:

m (O2) = n (O2) * M (O2) = 0.1 * 32 = 3.2 g.

Answer: 3.2 g.