Answer:
17.57kg of [tex]TiCl_{4}[/tex] and its percentage yield is 81.0%
Explanation:
Through the reaction you can get the theoretical amount of [tex]TiCl_{4}[/tex] that must be produced.
[tex]7.39kgTiO_{2}x\frac{1kmolTiO_{2} }{79.867kgTiO_{2}}x \frac{1kmolTiCl_{4}}{1kmolTiO_{2}}x\frac{189.867kgTiCl_{4} }{1kmolTiCl_{4}}=17.57kgTiCl_{4}[/tex]
If the amount obtained is less than the theoretical amount, it means that the initial sample was not 100% pure. Now the actual amount obtained is compared with the theoretical amount using a percentage
[tex]yield=\frac{actual amount}{theoretical amount}x100= \frac{14.24kg}{17.57kg}x100[/tex]=81.0%
The theoretical yield and percentage yield of TiCl₄ are:
1. The theoretical yield of TiCl₄ is 17.55 Kg
2. The percentage yield of TiCl₄ is 81.14%
The balanced equation for the reaction is given below:
TiO₂ + 2C + 2CI₂ −> TiCI₄ + 2CO
Molar mass of TiO₂ = 48 + (16×2) = 80 g/mol
Mass of TiO₂ from the balanced equation = 1 × 80 = 80 g
Divide by 1000 to express in Kg
80 / 1000 = 0.08 kg
Molar mass of TiCI₄ = 48 + (35.5×4) = 190 g/mol
Mass of TiCI₄ from the balanced equation = 1 × 190 = 190 g
Divide by 1000 to express in Kg
190 / 1000 = 0.19 Kg
From the balanced equation above,
0.08 kg of TiO₂ reacted to produce 0.19 Kg of TiCI₄
1. Determination of the theoretical yield of TiCI₄
From the balanced equation above,
0.08 kg of TiO₂ reacted to produce 0.19 Kg of TiCI₄.
Therefore,
7.39 kg of TiO₂ will react to produce = [tex]\frac{7.39 * 0.19}{0.08}\\\\[/tex] = 17.55 Kg of TiCI₄.
Thus, the theoretical yield of TiCI₄ is 17.55 Kg
2. Determination of the percentage yield of TiCI₄
Actual yield = 14.24 kg
Theoretical yield = 17.55 Kg
[tex]Percentage yield = \frac{Actual}{Theoretical} * 100\\\\= \frac{14.24}{17.55} * 100\\\\[/tex]
Therefore, the percentage yield of TiCI₄ is 81.14%
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