The actual yield of magnesium nitrate formed from 130.8 g of magnesium and excess copper(II) nitrate is 245.2 g.
The balanced chemical equation is the equation in which the number of atoms on the reactant side is equal to the number of atoms on the product side in an equation.
The balanced chemical equation is as follows:
Mg + Cu(NO₃)₂ → Mg(NO₃)₂ + Cu
To calculate the actual yield use the expression
Actual yield = Efficiency × theoretical yield
Number of moles = [tex]\frac{\text{Given mass}}{\text{Molar mass}}[/tex]
= [tex]\frac{130.8}{24}[/tex]
= 5.45
Efficiency moles of Mg(NO₃)₂ = 0.304 × 5.45
= 1.6568 mol
Now put the value in above expression
Actual yield = Efficiency × theoretical yield
= 1.6568 × 148
= 245.2 g
Thus from the above conclusion we can say that The actual yield of magnesium nitrate formed from 130.8 g of magnesium and excess copper(II) nitrate is 245.2 g.
Learn more about the Balanced chemical equation here: https://brainly.com/question/26694427
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