PPT-Reactants, Products, and Leftovers

Activity 1 Introduction to Chemical reactions by Trish Loeblein httpphetcoloradoedu Learning Goals Students will be able to Relate the realworld example of making sandwiches to chemical reactions. Chemical Reactions. Investigation One. Chemical compounds are formed when two or more elements combine.. H. ₂ + O .  H₂O (water). Na + . Cl.  . NaCl. ( Sodium Chloride – Salt). Chemical Compounds. . 10/29/15. What do you think it means when we say 2 chemicals can react?. Objective . Tonight’s Homework. To learn how to count atoms before and after a reaction. p 228: 1-7. Notes on Reactants and Products. Chapter 17. Pages 511-524. Phase Diagrams. -a graph of pressure vs. temp that shows the conditions under which the phases of a substance exist. Triple point – . indicates the T and P conditions at which the solid, liquid, and vapor of the substance coexist at eq. Predicting products. Based on the reactants alone, you should be able to . Predict the products. Write them correctly. Balance the final equation. There are some general guidelines to follow for each type of reaction. . Parts of a chemical equation:. Reactants. : a substance present at the beginning of a chemical reaction. (Left side). Products. : a substance that is produced during a chemical reaction (Right Side). Activity 2:. . Limiting Reactants in Chemical . reactions. by Trish Loeblein . . http://phet.colorado.edu. (assuming complete reactions). Learning Goals: . Students . will be able to: . Predict the amounts of products and leftovers after reaction using the concept of limiting reactant. Reaction Kinetics. &. Chemical Equilibrium. Reaction Mechanisms. Reaction Mechanism:. the step-by-step sequence of reactions by which the overall chemical change occurs.. Intermediates:. species that appear in some steps but not in the net equation.. Equilibrium. When a reaction is at a state of equilibrium, the rate of the forward reaction __________ the rate of the reverse reaction.. is equal to. is slower than. is faster than. is the reverse of. by Trish Loeblein . . http://phet.colorado.edu. (assuming complete reactions). Reactants, Products, and Leftovers . Activity 1. :. Introduction to Chemical reactions. by Trish Loeblein . . http://phet.colorado.edu. Reaction. Reaction. Rates. Rates. Rates. Kinetics. Will the reaction occur?. How fast?. What are the steps . of the reaction?. Kinetics asks …. Kinetics. Even if Δ. G. indicates that . it is a favorable reaction, it still may not occur (it may not be spontaneous).. Barbara Mowery. York College. At equilibrium, the rate of the forward reaction is _______ the rate of the reverse reaction.. equal to. slower than. faster than. d. the reverse of. At equilibrium, the rate of the forward reaction is _______ the rate of the reverse reaction.. Reaction Energies. In our earlier discussions of calorimetry, we used . physical. sources of heat (hot metal slug). It is also possible to use . chemical. sources of heat (like hot packs and cold packs).. Chemical reactions. A . chemical reaction . is when one or more substances change into different substances. . Example . iron + sulfur .  iron (ii) sulfide + energy. Go to textbook Page 225. Read page 225 and write definitions for the following into your notes.. Methane, CH. 4. , burns in air.. Chlorine gas reacts with sodium bromide.. Energy and Reactions. Context clues in given scenarios or observations in experimentation convey energy transfer in reactions. .