Chemistry 12.1

Interpreting Chemical Equations 12.1 Interpreting Chemical Equations A balanced chemical equation can be interpreted in terms of different quantities, including numbers of atoms, molecules, or moles; mass; and volume.

Interpreting Chemical Equations 12.1 Interpreting Chemical Equations Number of Atoms: Determine Number of atoms by multiplying coefficient by subscript, just like when balancing equations. The balanced chemical equation for the formation of ammonia can be interpreted in several ways. Predicting How many molecules of NH3 could be made from 5 molecules of N2 and 15 molecules of H2?

Interpreting Chemical Equations 12.1 Interpreting Chemical Equations Number of Molecules: Determine the number of molecules simply by looking at the coefficient. The balanced chemical equation for the formation of ammonia can be interpreted in several ways. Predicting How many molecules of NH3 could be made from 5 molecules of N2 and 15 molecules of H2?

Interpreting Chemical Equations 12.1 Interpreting Chemical Equations Moles: Moles are also determined by looking at the coefficient. The balanced chemical equation for the formation of ammonia can be interpreted in several ways. Predicting How many molecules of NH3 could be made from 5 molecules of N2 and 15 molecules of H2?

Interpreting Chemical Equations 12.1 Interpreting Chemical Equations Mass: Find the mass by multiplying the number of atoms by the mass on the Periodic Table. The balanced chemical equation for the formation of ammonia can be interpreted in several ways. Predicting How many molecules of NH3 could be made from 5 molecules of N2 and 15 molecules of H2?

Interpreting Chemical Equations 12.1 Interpreting Chemical Equations Volume: Multiply the # of moles (coefficient) by the standard at STP (22.4 L) The balanced chemical equation for the formation of ammonia can be interpreted in several ways. Predicting How many molecules of NH3 could be made from 5 molecules of N2 and 15 molecules of H2?

Mass Conservation in Chemical Reactions 12.1 Mass Conservation in Chemical Reactions Mass and atoms are conserved in every chemical reaction. Volume, moles, and molecules ARE NOT!

Mass Conservation in Chemical Reactions 12.1 Mass Conservation in Chemical Reactions How many moles of Sulfuric Acid are in the reaction? How many molecules of Iron (III) Sulfate are there?

Moles Sulfuric Acid: 3 Molecules Iron (III) Sulfate: 1 Answer: Moles Sulfuric Acid: 3 Molecules Iron (III) Sulfate: 1

Conceptual Problem 12.1

Conceptual Problem 12.1

Conceptual Problem 12.1

12.1 Section Quiz. 12.1.

12.1 Section Quiz. 1. A manufacturer of bicycles has 5350 wheels, 3023 frames, and 2655 handlebars. How many bicycles can be manufactured using these parts? 2675 bicycles 2655 bicycles 3023 bicycles 5350 bicycles

2. A reaction that produces iron metal from iron ore is shown below. 12.1 Section Quiz. 2. A reaction that produces iron metal from iron ore is shown below. Fe2O3•H2O(s) + 3CO(g)  2Fe(s) + 3CO2(g) + H2O(g) In this equation, the volume of gas at STP that reacts and the volume of gas at STP produced will be 3 L and 4 L. 67.2 L and 89.6 L. 67.2 L and 67.2 L 3 L and 3 L

12.1 Section Quiz. 3. What is conserved in the reaction shown below? H2(g) + Cl2(g)  2HCl(g) only mass only mass and number of moles only mass, number of moles, and number of molecules mass, number of moles, number of molecules, and volume

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