Question

1. Alexander does the following reaction with 43.5 grams of 02. If he makes 213.4 grams of K20, what was his percent yield?

4 K3P + 3 02 -> 6 K20 + 1 P4

Answer 1

To find the percent yield, you need to first calculate the theoretical yield of the reaction, which is the maximum amount of product that could be produced from the given amount of reactants. In this case, you can use the balanced equation to calculate the number of moles of K2O produced from the moles of O2 used.

First, convert the mass of O2 to moles by dividing by the molar mass of O2 (32 g/mol): 43.5 g / 32 g/mol = 1.3625 mol O2

Then, use the balanced equation to find the moles of K2O produced: 1.3625 mol O2 * (6 mol K2O / 3 mol O2) = 2.725 mol K2O

Then, convert the moles of K2O to grams by multiplying by the molar mass of K2O (94 g/mol): 2.725 mol K2O * 94 g/mol = 255.99 g

The percent yield is then calculated as: (Actual yield / Theoretical yield) * 100 = (213.4 / 255.99) * 100 = 83.3%

So the percent yield of the reaction is 83.3%.

Step-by-step explanation: