Taking into account the above reaction of magnesium hydroxide with hydrochloric acid to produce magnesium chloride. Show the calculation for the determination of theoretical yield of MgCl2 from 15.0g of magnesium hydroxide and 10.0 g of HCl.
Balanced
Mg(OH)2(s) + 2 HCl (aq) ➙ MgCl2(aq) + 2 H2O(l)
- No. Of moles of Mg(OH)2 In 16.1 g :-
No. Of moles = mass (g) /molar mass(g)
= 16.1 g / 58.32 g/mol
= 0.276 moles of Mg(OH)2 is used.
- No. Of moles of HCl In 11.0 g :-
No. Of moles = mass (g) /molar mass(g)
= 11.0 g / 36.458 g/mol
= 0.302 moles of HCl is used for reaction.
According the balance chemical reaction :-
1 mol of magnesium hydroxide require 2 moles of HCl for complete neutralization
0.276 moles of Mg(OH)2 require 0.276 x 2 = 0.552 moles of HCl for complete neutralization, but it is present in less amount. (0.302 moles)
Therefore,
HCl is the limiting reagent
Now,
Since HCl is limiting reagent moles of MgCl2 form is depend upon HCl
2 moles of HCl produces 1 mole of MgCl2
0.302 moles of HCl produces ? mole of MgCl2
? moles of MgCl2 =( 0.302 x 1 )/ 2
= 0.151 moles Of MgCl2 will produced.
- Mass of 0.151 mole of MgCl2
= No. Of moles x molar mass
= 0.151 mol x 95.211 g/mol
= 14.376861 g of MgCl2 will be produced
- HCl is the limiting reagent
- 14.38 g of MgCl2 will be produced
Taking into account the above reaction of magnesium hydroxide with hydrochloric acid to produce magnesium chloride. Show the calculation for the determination of theoretical yield of MgCl2 from 15.0g of magnesium hydroxide and 10.0 g of HCl.
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