Answer:
87.6%
Step-by-step explanation:
Step 1:
The balanced equation for the reaction.
LiOH + HCl —> LiCl + H2O
Step 2:
Determination of the mass of LiOH that reacted and the mass of LiCl produced from the balanced equation.
This is illustrated below:
Molar mass of LiOH = 7 + 16 + 1 = 24g/mol
Mass of LiOH from the balanced equation = 1 x 24 = 24g
Molar Mass of LiCl = 7 + 35.5 = 42.5g/mol
Mass of LiCl from the balanced equation = 1 x 42.5 = 42.5g
Thus, from the balanced equation, 24g of LiOH reacted to produce 42.5g of LiCl.
Step 3:
Determination of the theoretical yield of LiCl.
This is illustrated below:
From the balanced equation above,
24g of LiOH reacted to produce 42.5g of LiCl.
Therefore, 20g of LiOH will react to produce = (20 x 42.5)/24 = 35.4g
Therefore, the theoretical yield of LiCl is 35.4g.
Step 4:
Determination of the percentage yield of LiCl. This is illustrated below:
Actual yield of LiCl = 31g
Theoretical yield of LiCl = 35.4g
Percentage yield of LiCl =.?
Percentage yield = Actual yield /Theoretical yield x 100
Percentage yield = 31/35.4 x 100
Percentage yield of LiCl = 87.6%