Determine the percent yield for the reaction between 6.92 g K and 4.28 g of O2 if 7.36 g of K2O is produced?

Question

Best answer to whoever can solve AND explain this throughoughly.

Answer 1

This is a limiting reactant / stoichiometry question

First write the balanced equation

4K + O2 == 2K2O

Convert the grams for each reactant to moles, using their respective molecular mass.

Now you have to calculate the stoich. twice, once for each reactant. Don't forget to use the corect molar ratio each time. See how much K2O can be made from each item. The smallest one is the limiting reactant. The reaction stops when one of the reactants is used up.

Now take the 7.36 grams actually produced and divide this by the amount that should have been produced from above. That gives you the percent yield