Stoikiometri Guide

2H₂ + O₂ → 2H₂O

In chemistry, you must always identify the limiting reactant before you can calculate how much product you will actually get. Even when you do the math perfectly, real experiments rarely produce the theoretical amount of product. Some product may stick to the glassware, evaporate, or react in a side reaction. The amount you calculate is the theoretical yield (the perfect result). The amount you actually measure in the lab is the actual yield . stoikiometri

Consider the famous reaction of hydrogen and oxygen to form water: 2H₂ + O₂ → 2H₂O In chemistry, you

The other reactants are called excess reactants . The amount you calculate is the theoretical yield

Look at the coefficients: For every 2 moles of H₂O produced, you need 2 moles of H₂. The ratio of H₂ to H₂O is 2:2, which simplifies to 1:1. Moles of H₂ needed = 2.00 moles H₂O × (2 mol H₂ / 2 mol H₂O) = 2.00 moles H₂.