Mole to Mole Stoichiometry

Master mole to mole stoichiometry calculations with engaging chemistry practice!

1. Ammonia is one of the main nitrogen fertilizers. It is prepared by the reaction between molecular hydrogen and nitrogen 3 H2(g) + N2(g) → 2 NH3How many moles of NH3 are produced if 4.5 moles of N2 react? 2 moles 4.5 moles 9 moles 2.25 moles 2. Consider the last chemical reaction equation. How many moles of N2 and H2 are required to produce 3.8 moles of NH3? 2 moles of H2 and 1 mole of N2 5.7 moles of N2 and 1.9 moles of H2 5.7 moles of H2 and 1.9 moles of N2 5.7 moles of H2 and 5.7 moles of N2 3. Consider the last chemical reaction equation. How many grams of N2 are needed to produce 4.7 moles of NH3? 2.35 g 65.8 g 28 g 0.084 g 4. Balance the following chemical equation:(fill all blanks, even if it is "1") 2 Al(s) + 3 H2SO4(aq) → 1 Al2(SO4)3 (aq)+ 3 H2(g) 5. Phosphine is prepared by the reaction between molecular hydrogen and phosphorous 6 H2(g) + P4(s) → 4 PH3 How many moles of PH3 are produced if 1.5 moles of P4 react? and how many grams of PH3? 2.6 moles of PH3 0.375 moles of PH3 6 moles of PH3 4 moles ofPH3 Fill in the Blanks. Note: You may have to look ahead into the next few sections for some answers! Stoichiometry uses a balanced chemical equation to provide for molar relationships for all entities in a reaction.It is specifically the coefficients in the balanced chemical equation, that correspond to the molar ratios. By setting up a mole ratio, we can solve for unknown quantities of moles, when we are provided with a known quantity of moles of a different reactant or product.If we want to determine the mass of a compound that is found through stoichiometry, we must simply use molar mass values from the periodic table to convert from moles to mass. If we are asked to solve for the number of molecules that are produced through stoichiometry, we must multiply the quantity in moles (solved by means of the mole ratio) by Avogadro's Number to properly convert to molecules.The limiting reagent is the reactant that is used up first in a chemical reaction. When it is completely consumed in a reaction, the reaction will stop.The reactant that is left over when the reaction stops is called the excess reactant.We can determine the percentage yield of a chemical reaction, by dividing the actual yield by the theoretical yield, and multiplying by 100%.