# Problem: Pure titanium metal is produced commercially from titanium (IV) chloride (TiCl4), which is produced via the reaction: TiO2(s) + 2C(s) + 2Cl2(g) → TiCl4(l) + 2CO(g) How much (moles) TiCl4 can be made from 2.0 mol TiO2(s), 5.0 mol C(s) and 3.0 mol Cl2(g)?a)  1.5 mol                b)  2.0 mol             c)  2.5 mol             d)  5.0 mol              e)  1.0 mol

###### FREE Expert Solution

We’re being asked to calculate the moles TiCl4 that will be formed in the reaction.

For this problem, we need to do the following steps:

Step 1: Write and balance a chemical equation for the given reaction.

Step 2: Determine the limiting reactant and calculate the mass of TiCl2 formed.

Step 1: Write and balance a chemical equation for the given reaction.

TiO(s) + 2 C(s) + 2 Cl2(g) ® TiCl(l) + 2 CO(g)

Reactants                 Products

Ti          1                         1

C          2                        2

Cl         4                        4

O         2                        2

Reaction is balanced

95% (434 ratings) ###### Problem Details

Pure titanium metal is produced commercially from titanium (IV) chloride (TiCl4), which is produced via the reaction:

TiO2(s) + 2C(s) + 2Cl2(g) → TiCl4(l) + 2CO(g) How much (moles) TiCl4 can be made from 2.0 mol TiO2(s), 5.0 mol C(s) and 3.0 mol Cl2(g)?

a)  1.5 mol

b)  2.0 mol

c)  2.5 mol

d)  5.0 mol

e)  1.0 mol