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If TiCl3 + Cl2 → TiCl4rnrn4.4573 moles of Cl2 are reacted with 0.62 moles of TiCl3, how many grams of TiCl4 will be produced if the reaction proceeds with a 89.64% yield?
Accepted Answer
Assuming pure reactants, 4.4573 moles of Cl2 is in excess of the 0.62 moles of TiCl3. Therefore, 0.62 moles of TiCl3 will react with 0.62 moles of Cl2. The balanced chemical reaction is:
TiCl3 + Cl2 → TiCl4
The mole ratio of TiCl4 to be formed is 1:1, so 0.62 moles of TiCl4 will be formed.
The molar mass of TiCl4 is 189.67 g/mol.
Therefore, the mass of TiCl4 produced will be:
0.62 moles TiCl4 × 189.67 g/mol TiCl4 = 117.51 g TiCl4
The reaction proceeds with an 89.64% yield. Therefore, the actual mass of TiCl4 produced will be:
117.51 g TiCl4 × 0.8964 = 105.41 g TiCl4
Therefore, 105.41 grams of TiCl4 will be produced.
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