Date: Hybrid Chemistry Regents Prep Ms. Hart/Mr. Kuhnau
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1 Name: Period: Date: Hybrid Chemistry Regents Prep Ms. Hart/Mr. Kuhnau UNIT 5: Kinetics and Equilibrium Lesson 1: Collision theory and potential energy diagrams By the end of today, you will have an answer to: What is required for a chemical reaction to take place? DO NOW: 1. A neutral atom contains 12 neutrons and 11 electrons. The number of protons in this atom is (1) 1 (3) 11 (2) 12 (4) The atomic mass of an element is the weighted average of (1) Number of protons in the isotopes of that element (2) Number of neutrons in the isotopes of that element (3) Atomic numbers of the naturally occurring isotopes of that element (4) Atomic masses of the naturally occurring isotopes of that element. 3. What is the electron configuration for an ion of calcium (Ca)? 4. What is the electron configuration for an atom of calcium in the excited state? 5. What is the chemical formula for calcium oxide? 6. Write a decay equation for Iron-53. Collision Theory (Video: In order for a chemical reaction to occur, the reactant need to collide with: ENERGY: PARTS OF THE POTENTIAL ENERGY DIAGRAM Potential Energy (Heat) Heat of reaction H = PEP-PER Reaction Coordinate 1
2 Exothermic versus Endothermic Reactions Endothermic Reaction Exothermic Reaction Energy is H Potential Energy diagram Example Chemical Reaction N2 (g) + 3H2(g) 2NH3(g) kJ H = 2C(s) + 2H2(g) kj C2H4(g) H = Practice: 1. Given the balanced equation representing a reaction: Which statement is true about energy in this reaction? (1) The reaction is exothermic because it releases heat. (2) The reaction is exothermic because it absorbs heat. (3) The reaction is endothermic because it releases heat. (4) The reaction is endothermic because it absorbs heat. 2. What is the H for the reaction in #1? Potential Energy Diagrams: Potential Energy Diagrams show us the potential energy changes during the course of a reaction as the products form from the reactants. They look like these below! 2
3 WHOLE GROUP PRACTICE: EXAMPLE 1: Understanding parts of the diagram 1. The diagram to the below represents the potential energy for the reaction: N 2 (g) + 3H 2 (g) 2NH 3 (g) a) What does (a) represent? b) What does (b) represent? c) What does (c) represent? d) What are the reactants in this equation? Place a 1 where you would find them on the potential energy diagram. e) What are the products in this equation? Place a 2 where you would find them on the potential energy diagram. EXAMPLE 2: CALCULATING HEAT OF REACTION USING THE DIAGRAM Base your answers to questions 1-4 on the potential energy diagram below. 1. What is the potential energy of the reactants? 2. What is the potential energy of the products? 3. What is the heat of the forward (left to right) reaction? HINT: Heat of reaction (ΔH)= Potential Energy of Products Potential Energy of Reactants 4. Is this reaction exothermic or endothermic? 3
4 EXAMPLE 3: MORE HEAT OF REACTION a) What is the heat of the FORWARD reaction? (Hint: heat of products-heat of reactants ) b) What is the heat of the BACKWARD reaction? (Hint: where are the products of the BACKWARD reaction found?) EXAMPLE 4: CONCEPTUAL UNDERSTANDING An increase in temperature increases the rate of a chemical reaction because the (1) Activation energy increases (2) Activation energy decreases (3) Number of molecular collisions increases (4) Number of molecular collisions decreases EXAMPLE 5: PUTTING IT ALL TOGETHER Given the reaction, A + B AB + 210kJ Is this reaction exothermic or endothermic? Draw a potential energy diagram for the reaction above, assuming there is an activation energy of 21 kj. What would the activation energy of the reverse reaction be? 4
5 Name: Period: Date: Hybrid Chemistry Regents Prep Ms. Hart/Mr. Kuhnau CW 5.1- Collision Theory and Potential Energy Diagram 10 points Directions: Answer all questions based on your knowledge of chemistry 1. In order for a chemical reaction to occur, there must always be (1) an effective collision between reacting particles (2) a bond that breaks in a reactant particle (3) reacting particles with a high charge (4) reacting particles with high kinetic energy 2. As the number of effective collisions between reacting particles increases, the rate of reaction (1) decreases (2) increases (3) remains the same (4) changes the orientation of the particles 3. Given the balanced equation: Which phrase best describes this reaction? (1) endothermic with H = kj (2) endothermic with H = kj (3) exothermic with H = kj (4) exothermic with H= kj 6. Which of the following potential energy diagrams represent: a) A endothermic reaction? b) An exothermic reaction? 4. Given the balanced equation representing a reaction: What occurs during this reaction? (1) A bond is broken as energy is absorbed. (2) A bond is broken as energy is released. (3) A bond is formed as energy is absorbed. (4) A bond is formed as energy is released. 5. Which statement correctly describes an endothermic chemical reaction? (1) The products have higher potential energy than the reactants, and the H is negative. (2) The products have higher potential energy than the reactants, and the H is positive. (3) The products have lower potential energy than the reactants, and the H is negative. (4) The products have lower potential energy than the reactants, and the H is positive. 7. Given the following reaction: S(s) + O 2 (g) SO 2 (g) + energy Is the reaction endothermic or exothermic? 8. In a chemical reaction, the difference between the potential energy of the products and the potential energy of the reactants is defined as (1) activation energy (2) ionization energy (3) heat of reaction (4) heat of vaporization 9. Exothermic reactions heat and endothermic reactions heat. 5
6 10. Match the following to the letters on the graph left: (1) Potential Energy of the products (2) Potential Energy of the reactants (3) Heat of Reaction (4) Potential Energy of the activated complex (5) Draw in and label what the activation energy would be. 11. Given the reaction at equilibrium: On the diagram below, complete the potential energy diagram from the forward reaction. Be sure your drawing shows the activation energy and the potential energy of the products. 12. Given the potential energy diagram for a chemical reaction: Which statement correctly describes the energy changes that occur in the forward reaction? (1) The activation energy is 10 kj and the reaction is endothermic (2) The activation energy is 10 kj and the reaction is exothermic (3) The activation energy is 50 kj and the reaction is endothermic (4) The activation energy is 50 kj and the reaction is exothermic 6
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