Respuesta :
Answer: Thus 8.41 g was the mass of the original sample
Explanation:
To calculate the moles :
[tex]\text{Moles of solute}=\frac{\text{given mass}}{\text{Molar Mass}}[/tex]
[tex]\text{Moles of} O_2=\frac{3.29g}{32g/mol}=0.103moles[/tex]
[tex]2KClO_3\rightarrow 2KCl+3O_2[/tex]
According to stoichiometry :
As 3 moles of [tex]O_2[/tex] are produced by = 2 moles of [tex]KClO_3[/tex]
Thus 0.103 moles of [tex]O_2[/tex] are produced by =[tex]\frac{2}{3}\times 0.103=0.0687moles[/tex] of [tex]KClO_3[/tex]
Mass of [tex]KClO_3=moles\times {\text {Molar mass}}=0.0687moles\times 122.5g/mol=8.41g[/tex]
Thus 8.41 g was the mass of the original sample.
8.41 grams is the mass of original sample of KClO₃.
How we calculate mass from moles?
Mass of any substance will be calculated from the moles as:
n = W/M, where
W = given or required mass
M = molar mass
Given chemical reaction is:
2KClO₃ → 2KCl + 3O₂
Given mass of O₂ = 3.29g
Moles of O₂ = 3.29g/16g/mole = 0.103 moles
From the stoichiometry of reaction, it is claer that:
3 moles of O₂ = produced by 2 moles of KClO₃
0.103 moles of O₂ = produced by 2/3×0.103 = 0.0687 moles of KClO₃
Now mass of KClO₃ = 0.0687 × 122.5g/mol = 8.41g
Hence, 8.41g is the mass of KClO₃.
To know more about moles, visit the below link:
https://brainly.com/question/13860160
