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Aqueous Reactions and Thermochemistry: Understanding Electrolytes, Reactions, and Enthalpy

This guide covers key concepts in aqueous reactions and thermochemistry, focusing on electrolytes, solubility, precipitation, acid-base interactions, and oxidation-reduction processes. It includes predictions of precipitates, balanced equations for various reactions, calculations of molarity, and discussions on thermodynamic principles like the first law, endothermic vs. exothermic reactions, and Hess's law. It serves as a comprehensive tool for mastering the behavior of compounds in solutions and the energy changes involved in chemical processes.

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Aqueous Reactions and Thermochemistry: Understanding Electrolytes, Reactions, and Enthalpy

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  1. Unit 2 Chapters 4, and 5

  2. Aqueous Reactions • Solution: • Electrolyte: • Nonelectrolyte:

  3. Dissolving compounds and molecules

  4. The diagram below represents an aqueous solution of one of the following compounds: MgCl2, KCl, or K2SO4. Which solution does the drawing best represent?

  5. Solubility of Ionic Compounds

  6. Precipitation Reactions • Double Replacement Reaction: • Ionic Equation: • Net Ionic Equation:

  7. Predict the identity of the precipitate that forms when solutions of BaCl2 and K2SO4 are mixed. Write the balanced chemical equation for the reaction.

  8. Acid-Base Reactions • Acid: • Base: • Strong acid or base vs weak acid or base:

  9. Neutralization Reactions

  10. Write a balanced molecular equation for the reaction between aqueous solutions of acetic acid and barium hydroxide. Write the net ionic equation for this reaction.

  11. Oxidation-Reduction Reactions • Oxidation-Reduction: • Oxidation: • Reduction:

  12. Oxidation Numbers

  13. Determine the oxidation number of sulfur in each of the following: a.) SCl2 b.) Na2SO3 c.) SO42-

  14. Oxidation of Metals • By acid: • By soluble salt:

  15. Write the balanced molecular and net ionic equation of aluminum with hydrobromic acid.

  16. Activity Series

  17. Solution Concentration • Molarity:

  18. Calculate the molarity of a solution made by dissolving 23.4 g of sodium sulfate in enough water to form 125 mL of solution.

  19. Concentration of Electrolytes

  20. What are the molar concentrations of each of the ions present in a 0.025 M aqueous solution of calcium nitrate?

  21. Converting molarity, moles, and volume

  22. How many grams of Na2SO4 are required to make 0.350 L of 0.500 M Na2SO4?

  23. Dilution

  24. How many milliliters of 3.0 M H2SO4 are needed to make 450 mL of 0.10 M H2SO4?

  25. Titrations • Titration:

  26. How many grams of Ca(OH)2 are needed to neutralize 25.0 mL of 0.100 M HNO3?

  27. Chapter 5 Thermochemistry

  28. Thermochemistry • Thermodynamics: • Thermochemistry:

  29. Types of Energy

  30. Units of Energy

  31. System and Surroundings • System: • Surroundings:

  32. Transferring Energy

  33. First Law of Thermodynamics

  34. Internal Energy

  35. Heat, Work, and ΔE

  36. Endothermic vs. Exothermic • Endothermic: • Exothermic:

  37. State Functions

  38. Enthalpy • Enthalpy • Heat transfer from system to surroundings • Heat transfer from surroundings to system

  39. Enthalpies of Reaction CH4(g) + 2 O2(g)  CO2(g) + 2 H2O(l) ΔH = -890 kJ

  40. How much heat is released when 4.50 g of methane gas is burned in a constant pressure system?

  41. Hess’s Law

  42. The enthalpy of reaction for the combustion of C(s) to CO2(g) is -393.5 kJ/mol, and the enthalpy for the combustion of CO to CO2 is -283.0 kJ/mol: C(s) + O2(g)  CO2(g) ΔH = -393.5 kJ CO(g) + ½ O2(g)  CO2(g) ΔH = -283.0 kJ Use this information to calculate the enthalpy for the combustion of C(s) to CO(g)

  43. Enthalpies of Formation • Standard Enthalpy of Formation • Formation Reactions

  44. Using Enthalpies of Formation • Hess’s Law • Equation:

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