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Titanium is a transition metal used in many alloys because it is extremely strong and lightweight. titanium tetrachloride (ticl4) is extracted from titanium oxide using chlorine and coke (carbon). if you begin with 1.25 mol tio2, what mass of cl2 gas is needed

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Following reaction is involved in above question: 

TiO2    +          2Cl2            →          TiCl4      +        O2
(1 mole)           (2 mole)

In the above reaction, it can be seen that 1 mole of TiO2 reacts with 2 mole of Cl2 to form 1 mole of TiCl4.

∴ 1.25 mole of TiO2 will react with 2.5 mole of Cl2 to form 1 mole of TiCl4.

Now, 1 mole of Cl2 = 70 g 
∴ 2.5 mole of Cl2 = 70 X 2.5 = 175 g

Thus, for complete reaction of 1.25 mole of TiO2, 175 g of Cl2 will be required. 

Answer:

The correct answer is 175 grams of Chlorine is required.  

Explanation:

The reaction for the given case is:

TiO₂ (1 mole)  + 2Cl₂ (2 mole) → TiCl₄ + O₂

From the reaction, it can be observed that 1 mole of TiO₂ reacts with 2 mole of Cl₂ to produce 1 mole of TiCl₄.

Therefore, 1.25 mole of TiO₂ will react with 2.5 mole of Cl₂ to produce 1 mole of TiCl₄.

The molecular weight of 1 mole of Cl₂ is 70 g

Thus, 2.5 mole of Cl₂ = 70 × 2.5 = 175 g

Therefore, for complete reaction of 1.25 mole of TiO₂, 175 g of Cl₂ will be needed.

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