Final - Chem 124 Final Study Guide This is a summary of the...

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Chem 124 Final Study Guide This is a summary of the key concepts you should understand and be able to apply for the final exam. Applying the concepts means DOING calculations. Chapters 1 – 5: BASICS Conversion from one metric unit to another (g to mg, m to km, etc) Conversion from English to Metric given conversion factor Basic Chemical Nomenclature (what is formula for sodium chloride? Carbon dioxide?) Traits of different states of matter (solid, liquid, gas) Components of Matter (Compounds, elements, atoms, ions, electrons, protons, neutrons, isotopes) Translating & Balancing Chemical Equations – this includes being able to predict products for types of reactions listed on orange handout Using Chemical Equations to do Stoichiometry (given this reaction, X grams of reactant Y makes how many grams of product Z?) Recognizing simple reaction types (acid-base, precipitation, combustion, combination, decomposition, etc) Knowing & Using the Ideal Gas Law PV = nRT Chapter 6 – Thermochemistry Law of Conservation of Energy – Total energy of Universe is constant Forms of energy and their interconversion o Kinetic o Potential Definition of System & Surroundings Total Internal Energy of a System Δ E = q + w o Δ E a state function – what does that mean? o Heat out vs. heat in to a system o Work out vs. work in Pressure-volume work Energy Units o The Joule o The calorie 1 cal = 4.184 J o The Calorie 1 Cal = 1 kcal Enthalpy, Δ H o What is it? Where does it come from? o When does Δ H = Δ E? o Also a state function o Exothermic vs. Endothermic processes – sign of Δ H o Drawing and Using Energy Diagrams to illustrate Δ H See Figures 6.6, 6.8, 6.10
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o How do we measure or calculate it? Calorimetry o q = mc Δ T, in J or cal o -q lost = q gained o Specific heat capacity, c in J/g•K o Constant Pressure Calorimetry – “Coffee-cup” Calorimetry Hess’s Law o Manipulating reactions and corresponding changes in Δ H Enthalpies of Formation Δ H˚f o Know how to write chemical reactions that correspond to Δ H˚f Reactions forming one mole of a substance from its elements in their standard states-check tables in the back of book o Δ Hrxn = Σ n Δ H˚f products – Σ n Δ H˚f reactants Using Δ Hrxn in stoichiometry problems o Thermochemical equation is a complete balanced equation with corresponding Δ Hrxn included, in kJ o Gives you a way to convert between J moles and grams You should be able to use any of the ways to calculate q or Δ H in combination with one another. Chapter 12—Part of Sections 12.1 & 12.2 that relate to Thermochemistry Phase Changes—what are they? o
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Final - Chem 124 Final Study Guide This is a summary of the...

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