The equation below shows the decomposition of lead nitrate. how many grams of oxygen are produced when 11.5 g no2 is formed? 2pb(no3) 2(s) --> 2pbo(s) + 4no2 (g) + o2(g

The mass of oxygen formed during the decomposition of lead nitrate is 2 grams.

The complete balanced equation will be:

From the reaction the decomposition of 2 moles of lead nitrate will give 4 moles of Nitric oxide and 1 mole of oxygen

The ratio of : Oxygen has been 2 : 1.

The moles of formed:

Moles =

Molecular weight of = 46 g/mol

Moles of =

Moles of = 0.25 moles.

The moles of = moles of Oxygen

Moles of oxygen =

Moles of oxygen = 0.06 mol.

The molecular weight of Oxygen = 32g/mol

Mass of 0.06 mol of Oxygen = 32 0.06

Mass of Oxygen = 2 grams.

The mass of oxygen formed during the decomposition of lead nitrate is 2 grams.

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