How do I distinguish between the limiting reactant and excess reactant in a chemical equation?
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To distinguish between the limiting reactant and excess reactant in a chemical equation, you need to compare the amount of each reactant you have with the stoichiometry of the balanced chemical equation.
Here's a step-by-step guide to determine the limiting reactant and excess reactant:
1. Start by writing the balanced chemical equation for the reaction.
2. Convert the known quantities of each reactant to moles. You can do this by dividing the given mass (in grams) by the molar mass of each respective reactant.
3. Next, use the mole ratio from the balanced equation to determine the number of moles of the other reactant that would be required for complete reaction.
4. Compare the calculated number of moles for each reactant to the number of moles needed based on the balanced equation. The reactant with the smaller number of moles is the limiting reactant, as it will be completely consumed in the reaction.
5. The reactant with the larger number of moles is the excess reactant. It is called "excess" because there is more of it than is needed to react completely.
So, by following these steps and comparing the calculated moles of each reactant to the stoichiometry of the balanced equation, you can determine the limiting reactant and excess reactant in a chemical equation.