Answer:
The answer is 87.5%
Explanation:
Step 1:
The balanced equation for the reaction. This is given below:
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 = 6.9 + 16 + 1.01 = 23.91g/mol
Mass of LiOH from the balanced equation = 1 x 23.91 = 23.91g
Molar Mass of mass of LiCl = 6.9 + 35.45 = 42.35g/mol
Mass of LiCl from the balanced equation = 1 x 42.35 = 42.35g
Summary:
From the balanced equation above,
23.91g of LiOH reacted to produce 42.35g of LiCl.
Step 3:
Determination of the theoretical yield of LiCl.
The theoretical yield of LiCl can be obtained as follow:
From the balanced equation above,
23.91g of LiOH reacted to produce 42.35g of LiCl.
Therefore, 20g of LiOH will react to produce = (20 x 42.35)/23.91 = 35.42g of LiCl.
Therefore, the theoretical yield of LiCl is 35.42g
Step 4:
Determination of the percentage yield of LiCl.
Actual yield of LiCl = 31g
Theoretical yield of LiCl = 35.42g
Percentage yield =?
Percentage yield = Actual yield /Theoretical yield x100
Percentage yield = 31/35.42 x 100
Percentage yield = 87.5%
