Question

The theoretical yield of a reaction is the amount of product obtained if the limiting reactant is completely converted to product. Consider the reaction: CH4(g) + CCl4(g) → 2 CH2Cl2(g) If 15.81 g CH4 is mixed with 19.52 g CCl4, calculate the theoretical yield (g) of CH2Cl2 produced by the reaction.

Answer 1

Consider the reaction:

CH4(g) + CCl4(g) → 2 CH2Cl2(g)

If 15.81 g =CH4 is mixed with

19.52 g= CCl4,

Moles of CH4 = 15.81 g/ 16.04 g/mol

= 0.986 moles.

Moles of CCl4 = 19.52 g / 153.82 g/mol

= 0.127 molesCCl4

CCl4 is limiting agent due to following reasons:

1. It completely reacted in the reaction.
2. It determines the amount of the product in mole.

Now calculate the moles of CH2Cl2:

0.127 molesCCl4 * 1.0 molesCCl4/ 2 moles of CH2Cl2

= 0.0635 mol CH2Cl2

Now calculate the mass of 0.0635 mol CH2Cl2

Molar mass = 84.93 g/mol

84.93 g/mol*0.0635 mol

= 5.39 g

Or = 5.4 g

The theoretical yield of a reaction is 5.4 g