What is the maximum mass of TiCl4 that can be obtained from 79.0 g TiO2, 37.9 g Cl2 and excess carbon? Please show all your steps.
3 TiO2(s) + 6 Cl2 + 4 C(s) --> 3 TiCl4(g) + 2 CO2(g) + 2 CO(g)
Molar Masses:TiO2-79.88, Cl2-70.90, TiCl4-189.68
See your post above.
To calculate the maximum mass of TiCl4 that can be obtained, we need to use the concept of limiting reactants. The limiting reactant is the one that is completely consumed and determines the maximum amount of product that can be formed.
Step 1: Calculate the moles of each reactant
Moles of TiO2 = mass / molar mass = 79.0 g / 79.88 g/mol = 0.988 mol
Moles of Cl2 = mass / molar mass = 37.9 g / 70.90 g/mol = 0.534 mol
Step 2: Determine the stoichiometric ratio
Based on the balanced chemical equation, the stoichiometric ratio between TiO2 and TiCl4 is 3:3, and between Cl2 and TiCl4 is 6:3. This means that 3 moles of TiO2 are required to produce 3 moles of TiCl4, and 6 moles of Cl2 are required to produce 3 moles of TiCl4.
Step 3: Find the limiting reactant
To determine the limiting reactant, compare the moles of each reactant to their stoichiometric ratio. The reactant that produces fewer moles of TiCl4 is the limiting reactant.
The moles of TiCl4 that can be formed from TiO2 = 0.988 mol × (3 mol TiCl4 / 3 mol TiO2) = 0.988 mol
The moles of TiCl4 that can be formed from Cl2 = 0.534 mol × (3 mol TiCl4 / 6 mol Cl2) = 0.267 mol
Since the moles of TiCl4 that can be formed from Cl2 (0.267 mol) are lower than the moles of TiCl4 that can be formed from TiO2 (0.988 mol), Cl2 is the limiting reactant.
Step 4: Calculate the mass of TiCl4 formed
The molar mass of TiCl4 is 189.68 g/mol.
Mass of TiCl4 formed = moles of TiCl4 formed × molar mass
= 0.267 mol × 189.68 g/mol
= 50.787 g
Therefore, the maximum mass of TiCl4 that can be obtained is 50.787 g.