Balanced chemical equation for reaction of aluminium hydroxide and sulfuric acid is as follows:
(a) From the balanced chemical reaction, 2 mole of gives 1 mole of thus, 1 mole of gives 0.5 moles of and 0.410 moles of gives 0.205 moles of .
Molar mass of is 342.1509 g/mol thus, mass of will be:
m=n×M=0.205 mol×342.1509 g/mol=70.14 g
Similarly, 3 moles of gives 1 mole of thus, 1 mole of gives 0.33 moles of and 0.410 moles of gives 0.136 moles of .
Thus, mass of will be:
m=n×M=0.136 mol×342.1509 g/mol=46.76g
Since, mass of obtained from is less than that from , is the limiting reactant.
(b) Number of moles of is 0.410 mol, from the balanced chemical reaction 3 moles of gives 1 mole of thus, 1 mole of gives 0.33 moles of and 0.410 moles of gives 0.136 moles of .
Therefore, number of moles of formed is 0.136 mol.
(c) After the completion of reaction, all of the limiting reactant gets converted into product thus, 0.410 mole of reacts completely to give 0.136 mol of .
From the balanced chemical reaction, 1 mole of formed from 2 moles of , thus, 0.136 mol of formed from 0.136×2=0.272 mol.
Thus, 0.272 moles of is used and remaining moles will be (0.410-0.272) mol=0.138 mol.
Therefore, 0.138 mol of excess reactant remains after the completion of reaction.