A 1.50-g mixture of the solid salts Na2SO4(molar mass 142.04 g/mol) and Pb(NO3)2(molar mass 331.20 g/mol) forms an aqueous solution with the precipitation of PbSO4 molar mass 303.26 g mol The precipitate was filtered and dried, and its mass was determined to be 0.392 g.The limiting reactant was determined to be Na2SO4. a. Write the molecular form of the equation for the reaction
Pb(NO3)2(aq) + Na2SO4(aq) ==> PbSO4(s) + 2NaNO3(aq)
The molecular form of the equation for the reaction can be represented as:
2 Na2SO4 + Pb(NO3)2 -> 2 NaNO3 + PbSO4
To write the molecular form of the equation for the reaction, we first need to determine the balanced chemical equation based on the given information.
We know that the reaction involves the mixture of Na2SO4 and Pb(NO3)2, resulting in the formation of PbSO4 as a precipitate.
The molecular form of the reaction can be written as:
2 Na2SO4 (aq) + Pb(NO3)2 (aq) → PbSO4 (s) + 2 NaNO3 (aq)
This equation shows that two moles of Na2SO4 react with one mole of Pb(NO3)2 to form one mole of PbSO4 and two moles of NaNO3.