Question

car batteries use solid lead and lead (iv) oxide in sulfuric acid to produce an electric current. pb + pbo2 + 2 h2so4 → 2 pbso4 + 2 h2o. calculate the moles of lead (ii) sulfate that would be produced if 5 moles of solid lead react with an excess of lead (iv) oxide and sulfuric acid. enter the value in the box. moles

Explanation:

Step1: Identify the mole - ratio from the balanced equation

The balanced chemical equation is $Pb + PbO_2+2H_2SO_4
ightarrow 2PbSO_4 + 2H_2O$. The mole - ratio of $Pb$ to $PbSO_4$ is $1:2$.

Step2: Calculate the moles of $PbSO_4$

If 5 moles of $Pb$ react, and the mole - ratio of $Pb$ to $PbSO_4$ is $1:2$, then the moles of $PbSO_4$ produced is $n = 2\times5$ moles.

Answer:

10 moles