Question

Consider the unbalanced reaction Ti(s) + Cl₂(g) --> TiCl4(s)

When 10.3 g of Ti react with 12.7 g of Cl₂, 16.2 g of TiCl4 are obtained. The
theoretical yield of TiCl4 is (number and unit)
A/
A/
A
, the limiting reactant is (name or symbol)
and the percent yield is (number)
%. (Remember to use correct sig figs)

Answer 1

Step-by-step explanation:

First, we need to determine the limiting reactant and the theoretical yield of TiCl4.

To do this, we need to calculate the amount of TiCl4 that should be produced based on the amount of each reactant, assuming that each reacts completely. We can start by calculating the amount of Ti and Cl2 in moles:

• moles of Ti = 10.3 g / 47.867 g/mol = 0.215 moles
• moles of Cl2 = 12.7 g / 70.906 g/mol = 0.179 moles

Next, we need to determine which reactant is limiting. To do this, we can calculate the amount of TiCl4 that would be produced if each reactant were completely consumed:

If Ti is limiting: 0.215 moles Ti × (1 mole TiCl4 / 1 mole Ti) × (189.68 g TiCl4 / 1 mole TiCl4) = 40.8 g TiCl4

If Cl2 is limiting: 0.179 moles Cl2 × (1 mole TiCl4 / 1 mole Cl2) × (189.68 g TiCl4 / 1 mole TiCl4) = 34.0 g TiCl4

Since the actual yield of TiCl4 is 16.2 g, which is less than the theoretical yield calculated when Cl2 is limiting, we can conclude that Cl2 is the limiting reactant.

Therefore, the theoretical yield of TiCl4 is 34.0 g.

We can calculate the percent yield by dividing the actual yield by the theoretical yield and multiplying by 100%:

percent yield = (actual yield / theoretical yield) × 100%

percent yield = (16.2 g / 34.0 g) × 100% = 47.6%

Therefore, the theoretical yield of TiCl4 is 34.0 g, the limiting reactant is Cl2, and the percent yield is 47.6%.