Respuesta :
Answer: The percent yield of aluminium phosphate in the reaction is 78.78 %
Explanation:
To calculate the number of moles, we use the equation:
[tex]\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}[/tex] .....(1)
- For sodium phosphate:
Given mass of sodium phosphate = 33.4 g
Molar mass of sodium phosphate = 164 g/mol
Putting values in equation 1, we get:
[tex]\text{Moles of sodium phosphate}=\frac{33.4g}{164g/mol}=0.204mol[/tex]
The chemical equation for the reaction of sodium phosphate and aluminium chloride is:
[tex]Na_3PO_4+AlCl_3\rightarrow 3NaCl+AlPO_4[/tex]
By Stoichiometry of the reaction:
1 mole of sodium phosphate produces 1 mole of aluminium phosphate
So, 0.204 moles of sodium phosphate will produce = [tex]\frac{1}{1}\times 0.204=0.204[/tex] moles of aluminium phosphate
- Now, calculating the mass of aluminium phosphate from equation 1, we get:
Molar mass of aluminium phosphate = 122 g/mol
Moles of aluminium phosphate = 0.204 moles
Putting values in equation 1, we get:
[tex]0.204mol=\frac{\text{Mass of aluminium phosphate}}{122g/mol}\\\\\text{Mass of aluminium phosphate}=(0.204mol\times 122g/mol)=24.88g[/tex]
- To calculate the percentage yield of aluminium phosphate, we use the equation:
[tex]\%\text{ yield}=\frac{\text{Experimental yield}}{\text{Theoretical yield}}\times 100[/tex]
Experimental yield of aluminium phosphate = 19.6 g
Theoretical yield of aluminium phosphate = 24.88 g
Putting values in above equation, we get:
[tex]\%\text{ yield of aluminium phosphate}=\frac{19.6g}{24.88g}\times 100\\\\\% \text{yield of aluminium phosphate}=78.78\%[/tex]
Hence, the percent yield of aluminium phosphate in the reaction is 78.78 %
