Presentation is loading. Please wait.

Presentation is loading. Please wait.

Stoichiometry Chapter 12.

Similar presentations


Presentation on theme: "Stoichiometry Chapter 12."— Presentation transcript:

1 Stoichiometry Chapter 12

2 A balanced chemical equation provides the same kind of quantitative information that a recipe does.
Everyday Equations

3 Using balanced chemical equations
Chemists use balanced chemical equations to calculate how much reactant is needed or product is formed in a reaction. Stoichiometry: the calculation of quantities in chemical reactions Using balanced chemical equations

4 Mass and atoms are conserved in every chemical reaction.
Conservation of Mass

5 A mole ratio is a conversion factor derived from the coefficients of a balanced chemical equation interpreted in terms of moles. N2(g) + 3H2(g)  2NH3(g) 1 mole N2 2 mole NH3 3 mole H2 3 mole H2 1 mole N2 2 mole NH3 Mole Ratio

6 In a chemical reaction, an insufficient quantity of any of the reactants will limit the amount of product that forms. Limiting reagent: reagent that determines the amount of product that can be formed by the reaction. The reaction occurs only until the limiting reagent is used up. Excess reagent: the reactant that is not completely used up in a reaction. Limiting Reagents

7 Theoretical yield: max amount of product that COULD be formed from given amounts of reactants
Actual yield: amount of product ACTUALLY formed in lab Percent yield: ratio of actual yield to theoretical yield, as percent. Measure of efficiency of reaction during procedure. Percent Yield


Download ppt "Stoichiometry Chapter 12."

Similar presentations


Ads by Google