Unit 2
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Transcript of Unit 2
Unit 2Chapters 4, and 5
Solution:
Electrolyte:
Nonelectrolyte:
Aqueous Reactions
Dissolving compounds and molecules
The diagram below represents an aqueous solution of one of the following compounds: MgCl2, KCl, or K2SO4. Which solution does the drawing best represent?
Solubility of Ionic Compounds
Double Replacement Reaction:
Ionic Equation:
Net Ionic Equation:
Precipitation Reactions
Predict the identity of the precipitate that forms when solutions of BaCl2 and K2SO4 are mixed. Write the balanced chemical equation for the reaction.
Acid:
Base:
Strong acid or base vs weak acid or base:
Acid-Base Reactions
Neutralization Reactions
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.
Oxidation-Reduction:
Oxidation:
Reduction:
Oxidation-Reduction Reactions
Oxidation Numbers
Determine the oxidation number of sulfur in each of the following:
a.) SCl2
b.) Na2SO3
c.) SO42-
By acid:
By soluble salt:
Oxidation of Metals
Write the balanced molecular and net ionic equation of aluminum with hydrobromic acid.
Activity Series
Molarity:
Solution Concentration
Calculate the molarity of a solution made by dissolving 23.4 g of sodium sulfate in enough water to form 125 mL of solution.
Concentration of Electrolytes
What are the molar concentrations of each of the ions present in a 0.025 M aqueous solution of calcium nitrate?
Converting molarity, moles, and volume
How many grams of Na2SO4 are required to make 0.350 L of 0.500 M Na2SO4?
Dilution
How many milliliters of 3.0 M H2SO4 are needed to make 450 mL of 0.10 M H2SO4?
Titration:
Titrations
How many grams of Ca(OH)2 are needed to neutralize 25.0 mL of 0.100 M HNO3?
Chapter 5Thermochemistry
Thermodynamics:
Thermochemistry:
Thermochemistry
Types of Energy
Units of Energy
System:
Surroundings:
System and Surroundings
Transferring Energy
First Law of Thermodynamics
Internal Energy
Heat, Work, and ΔE
Endothermic:
Exothermic:
Endothermic vs. Exothermic
State Functions
Enthalpy
Heat transfer from system to surroundings
Heat transfer from surroundings to system
Enthalpy
CH4(g) + 2 O2(g) CO2(g) + 2 H2O(l)
ΔH = -890 kJ
Enthalpies of Reaction
How much heat is released when 4.50 g of methane gas is burned in a constant pressure system?
Hess’s Law
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)
Standard Enthalpy of Formation
Formation Reactions
Enthalpies of Formation
Hess’s Law
Equation:
Using Enthalpies of Formation