Question

For the reaction shown, compute the theoretical yield of the product in moles for each of the following initial amounts of reactants.


Ti (s) + 2 Cl2 (g) ? TiCl4 (s)


2 mol Ti; 2 mol Cl2 -------------- moles


5 mol Ti; 9 mol Cl2 -------------- moles


0.483 mol Ti; 0.911 mol Cl2 ---- moles


12.4 mol Ti; 15.8 mol Cl2 ------- moles

.

Answer 1

For each of these problems, we will have to find out the limiting reagent from each of the reactants.

1.

2 moles of Ti x 1 mole of TiCl4/1 mole of Ti = 2 moles of TiCl4

2 moles of Cl2 x 1 mole of TiCl4/2 moles of Cl2 = 1 mole of TiCl4

LR is Cl2 because it produces fewer moles of TiCl4. Therefore, theoretical yield is 1 mole.

2.

5 moles of Ti x 1 mole of TiCl4/1 mole of Ti = 5 moles of TiCl4

9 moles of Cl2 x 1 mole of TiCl4/2 moles of Cl2 = 4.5 moles of TiCl4

LR is Cl2 because it produces fewer moles of TiCl4. Therefore, theoretical yield is 4.5 moles.

3.

0.483 moles of Ti x 1 mole of TiCl4/1 mole of Ti = 0.483 moles of TiCl4

0.911 moles of Cl2 x 1 mole of TiCl4/2 moles of Cl2 = 0.456 moles of TiCl4

LR is Cl2 because it produces fewer moles of TiCl4. Therefore, theoretical yield is 0.456 moles.

4.

12.4 moles of Ti x 1 mole of TiCl4/1 mole of Ti = 12.4 moles of TiCl4

15.8 moles of Cl2 x 1 mole of TiCl4/2 moles of Cl2 = 7.9 moles of TiCl4

LR is Cl2 because it produces fewer moles of TiCl4. Therefore, theoretical yield is 7.9 moles.

Hope this helps! :-)