Answer: The theoretical yield and percent yield for this experiment are 40 g and 82% respectively.
Explanation:
[tex]2KClO_3\rightarrow 2KCl+3O_2[/tex]
According to avogadro's law, 1 mole of every substance weighs equal to the molecular mass and contains avogadro's number [tex](6.023\times 10^{23})[/tex] of particles.
To calculate the moles:
[tex]\text{Moles of potassium chloride}=\frac{\text{Mass of potassium chloride}}{\text{Molar mass of potassium chloride}}=\frac{33g}{74.5g/mole}=0.44moles[/tex]
[tex]\text{Moles of potassium chlorate}=\frac{\text{Mass of potassium chlorate}}{\text{Molar mass of potassium chlorate}}=\frac{66g}{122.5g/mole}=0.54moles[/tex]
According to stochiometry:
2 moles of [tex]KClO_3[/tex] produce = 2 moles of [tex]KCl[/tex]
0.54 moles of [tex]KClO_3[/tex] should produce = [tex]\frac{2}{2}\times 0.54=0.54moles[/tex] of [tex]KCl[/tex]
Thus theoretical yield is [tex]moles\times {\text {Molar mass}}=0.54mol\times 74.5g/mol=40g[/tex]
But Experimental yield is 33 g.
[tex]{\text {percentage yield}}=\frac{\text {Experimental yield}}{\text {Theoretical yield}}\times 100\%[/tex]
[tex]{\text {percentage yield}}=\frac{33g}{40g}\times 100\%=82\%[/tex]
The theoretical yield and percent yield for this experiment are 40 g and 82% respectively.
