# How many moles of water are produced if 5.43 mol PbO2 are consumed? 10.9 mol.

Explanation:

To understand how to solve this problem, we must mention the reaction equation where water produced from PbO₂.

Pb + PbO₂ + 2H₂SO₄ → 2PbSO₄ + 2H₂O

Now, it is a stichiometric oriented problem, that 1 mole of PbO₂ produces 2 moles of H₂O.

Using cross multiplication:

1.0 mole of PbO₂ → 2.0 moles of H₂O

5.43 moles of PbO₂ → ??? moles of water

The moles of water produced = (5.43 x 2.0) = 10.86 moles ≅ 10.9 moles.

10.9

Explanation:

5.43 x = 10.86 which rounds to 10.9

just did it on edge 🙂

The correct answer is 10.86 moles.

It is a stoichiometry based problem,

One can solve this by just knowing the balanced chemical equation. The reaction where PbO2 is used and water is generated is:

Pb + PbO₂ + 2H₂SO₄ → 2PbSO₄ + 2H₂O

The mentioned reaction is witnessed in the lead storage battery.

Therefore, here as per the balanced equation one mole of PbO₂ is consumed providing two moles of water. So, for 5.43 moles of PbO₂, we will get,

2 × 5.43 moles of water = 10.86 moles.

this is a stoichiometry based problem

We can solve this by just knowing the balanced chemical equation.The reaction where PbO2 is used and water is produced is

Pb + PbO2 + 2H2SO4 > 2PbSO4 + 2H2O

This is reaction in lead storage battery

so here as per balanced equation one mole of PbO2 is consumed giving two moles of water

so if 5.43 moles of PbO2 we will get = 2 X 5.43 moles of water = 10.86 moles

It has to be understood that 2 moles of oxygen are there in each mole of PbO2. Then it has to be calculated for 2 moles of oxygen.

Amount of oxygen = 2 * 5.43 moles
= 10.86 moles
Now it is also a fact that each mole of H2O contains 1 mole of oxygen. Then it can be easily concluded that 10.86 moles of water will be produced. I hope the procedure is clear enough for you to understand.