Consider a hypothetical chemical reaction: A+B C+D (In this equation A, B, C and D stand for some unknown chemical formulas.) Here is an energy diagram for the reaction: energy (kJ/mol) 400 300- 200. 100- A+B reaction coordinate Use the energy diagram to answer these questions. What is the heat of reaction? C+D Is the reaction exothermic or endothermic? Can you determine the activation energy? Can you determine the activation energy of the reverse reaction? C+D A+B k kJ/mol O Exothermic O Endothermic ONeither O Yes, it's kJ/mol O No. O Yes, it's kJ/mol O No. X S

Consider a hypothetical chemical reaction: A+B C+D (In this equation A, B, C and D stand for some unknown chemical formulas.) Here is an energy diagram for the reaction: energy (kJ/mol) 400 300- 200. 100- A+B reaction coordinate Use the energy diagram to answer these questions. What is the heat of reaction? C+D Is the reaction exothermic or endothermic? Can you determine the activation energy? Can you determine the activation energy of the reverse reaction? C+D A+B k kJ/mol O Exothermic O Endothermic ONeither O Yes, it's kJ/mol O No. O Yes, it's kJ/mol O No. X S

General, Organic, and Biological Chemistry

7th Edition

ISBN:9781285853918

Author:H. Stephen Stoker

Publisher:H. Stephen Stoker

Chapter9: Chemical Reactions

Section: Chapter Questions

Problem 9.43EP

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Consider the following potential energy diagrams for two different reactions. Which plot represents an exothermic reaction? In plot a, do the reactants on average have stronger or weaker bonds than the products? In plot b, reactants must gain potential energy to convert to products. How does this occur?
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A 29.1-mL sample of 1.05 M KOH is mixed with 20.9 mL of 1.07 M HBr in a coffee-cup calorimeter (see Section 6.6 of your text for a description of a coffee-cup calorimeter). The enthalpy of the reaction, written with the lowest whole-number coefficients, is 55.8 kJ. Both solutions are at 21.8C prior to mixing and reacting. What is the final temperature of the reaction mixture? When solving this problem, assume that no heat is lost from the calorimeter to the surroundings, the density of all solutions is 1.00 g/mL, and volumes are additive.
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