Assuming an efficiency of 40 70 calculate the actual yield o

Assuming an efficiency of 40 70%, calculate the actual yield of magnesium nitrate formed fr magnesium and excess copper(ll) nitrate. 118.5 g of Number Tools ×101 bout us careers partes ay policy

Solution

One mole of magnesium will lreact with one mole of copper(II) nitrate to form one mole of magnesium nitrate

We have more copper(II) nitrate than you need for the reaction as given in question.

Molar mass of Mg = (118.5)*(1/24.3) = 4.87 moles of Mg

We need to find how many moles of magnesium nitrate would be required to produce

1 : 1 mole ratio in reaction

To get the actual yield, use the definition of the percent yield, which is

% yield = actual yield/theoretical yield

theoretical yield = 4.87 x 148.315 g = 722.294 g

Actual yield = 0.4070 * 722.294 = 293.97 g