How do you calculate the Theoretical yeild?
Given the following reaction 2 H2(g) + O2(g) –> 2 H2O(l) Calculate: a. the stoichiometric ratio of moles H2 to moles O2 b. the actual moles H2 to moles O2 when 1.50 mol H2 is mixed with 1.00 mol O2 c. the limiting reactant (H2 or O2) for the mixture in (b) d. the theoretical yield, in moles, of H2O for the mixture in (b) Solution a. The stoichiometric ratio is given by using the coefficients of the balanced equation. The coefficients are the numbers listed before each formula. This equation is already balanced. 2 mol H2 / mol O2 b. The actual ratio refers to the number of moles actually provided for the reaction. This may or may not be the same as the stoichiometric ratio. In this case, it is different: 1.50 mol H2 / 1.00 mol O2 = 1.50 mol H2 / mol O2 c. Note that the actual ratio of smaller than the required or stoichiometric ratio, which means there is insufficient H2 to react with all of the O2 that has been provided. The ‘insufficient’ component (H2) is the limiting reactant. Anot
