Question

Consider the balanced equation for the following reaction:

3Ca(ClO3)2(aq) + 2Li3PO4(aq) → Ca3(PO4)2(s) + 6LiClO3(aq)
Determine the theoretical yield of LiClO3(aq) in grams if the percent yield of LiClO3(aq) is 81.0% and 9.45 moles of LiClO3(aq) forms.

Answer 1

Answer: The theoretical yield of the lithium chlorate is 1054.67 grams

Step-by-step explanation:

To calculate the mass for given number of moles, we use the equation:

`\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}`

Actual moles of lithium chlorate = 9.45 moles

Molar mass of lithium chlorate = 90.4 g/mol

Putting values in above equation, we get:

`9.45mol=\frac{\text{Actual yield of lithium chlorate}}{90.4g/mol}\\\\\text{Actual yield of lithium chlorate}=(9.45mol* 90.4g/mol)=854.28g`

To calculate the theoretical yield of lithium chlorate, we use the equation:

`\%\text{ yield}=\frac{\text{Actual yield}}{\text{Theoretical yield}}* 100`

Actual yield of lithium chlorate = 854.28 g

Percentage yield of lithium chlorate = 81.0 %

Putting values in above equation, we get:

`81=\frac{854.28g}{\text{Theoretical yield of lithium chlorate}}* 100\\\\\text{Theoretical yield of lithium chlorate}=(854.28* 100)/(81)=1054.67g`

Hence, the theoretical yield of the lithium chlorate is 1054.67 grams