Question

If you are provided 4.00 kg of TiO2, 1.00 kg of C and 2.00 kg of Cl2, what mass of TiCl4 could be produced in the reaction shown below? (Hint: First identify the limiting reactant.) ___ TiO2(s) + ___ C(s) + ___ Cl2(g) → ___ TiCl4(g) + ___ CO(g) (not balanced: do this first)

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Answer 1

TiO₂(s) + 2 C(s) + 2 Cl₂(g) = TiCl₄(g) + 2 CO(g)

4 Kg of TiO2 = 4000 gm / 79.8658 = 50.08 Mole

1.00 kg of C = 1000 gm / 12.01 = 83.26 Mole

2.00 kg of Cl2 = 2000 gm / 70.90 = 28.2 Mole

here TiO₂ : C : Cl₂ is need 1 : 2 : 2 ratio.

Reactant present   50.08 Mole of TiO₂ :  83.26 Mole of C : 28.2 Mole of Cl₂

Cl2 only presents in minimum mole Hence it must be the limiting reagent.

28.2 Mole of Cl₂ will produce (28.2/2) 14.104 Mole of TiCl4 which is = 14.104 x 189.679 = 2675 gm of TiCl4 will be Produced (Molar mass of TiCl4 189.679)