Question

In a reaction, 358 g of $TiC{l}_4$ is reacted with 96 g of Mg. Calculate the % yield of $Ti$ if 32 g of $Ti$ is obtained from the reaction. (Molar mass of $Ti$ = 48 g/mol, Mg = 24 g/mol)

• A. 35.46%
• B. 66.86%
• C. 85.76%
• D. 48.34%

Answer 1

The correct option is A 35.46%

$TiC{l}_4+2Mg\to 2MgC{l}_2+Ti$
Moles of $TiC{l}_4=\frac{358}{190}=1.88$; moles of Mg $=\frac{96}{24}=4$
Calculation of limiting reagent:
2 moles of Mg reacts with 1 mole of $TiC{l}_4$
4 moles will react $=\frac{1}{2}\times 4=2$ moles of $TiC{l}_4$
Hence $TiC{l}_4$ is the limiting reagent.
1 mole of $TiC{l}_4$ produces 1 mole of Ti
1.88 mole will produce 1.88 mole of Ti
Mass of 1.88 mole of $Ti=1.88\times 48=90.24$ g
% yield $=\frac{\text{actual yield}}{\text{theoretical yield}}\times 100=\frac{32}{90.24}\times 100=35.46$