'6 kj' diaporamas de présentation

Thermochemistry: Chemical Energy

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Thermochemistry

Thermochemistry. Chapter 6. Kinetic Energy. energy of motion thermal energy is kinetic 1/2 mv 2. Heat. energy transferred between two objects as a result of the temperature difference between them. Temperature. A measure of kinetic energy. 1st Law of Thermodynamics.

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Enthalpy (H)

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Thermochemistry: Chemical Energy

Chapter 8. Thermochemistry: Chemical Energy. Energy is the capacity to do work Thermal energy is the energy associated with the random motion of atoms and molecules Chemical energy is the energy stored within the bonds of chemical substances

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Thermochemistry: Chemical Energy

Chapter 8. Thermochemistry: Chemical Energy. Energy is the capacity to do work Thermal energy is the energy associated with the random motion of atoms and molecules Chemical energy is the energy stored within the bonds of chemical substances

632 views • 46 slides

Thermo/Gas/Quantum Review

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Thermochemistry

Thermochemistry. kinetics. Equilibrium. Endothermic vs. Exothermic Rxns. Heat = enthalpy, ? H. Joules, or KJ. break bond (reactants). requires energy (endothermic). form bond (products). releases energy (exothermic). Avg. bond Enthalpy:.

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Thermodynamics

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Thermochemistry

Thermochemistry. Energy-capacity to do work or to produce heat Law of Conservation of Energy 1 st law of thermodynamics Energy can be neither created nor destroyed Energy of universe is constant Potential energy in chemistry, this is usually the energy stored in reactants and products

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Thermochemistry Unit Section 16.2

Thermochemistry Unit Section 16.2. Practice Problem #15:. a . H 2 O (g). H 2(s) + 1/2O 2(g) ? H 2 O (g) + 241.8 KJ. b . CaCl 2(s). Ca (s) + Cl 2(g) ? CaCl 2(s) + 795.4 KJ. c. CH 4(g). C (s) + 2H 2(g) ? CH 4(g) + 74.6 KJ. d . C 6 H 6(l). 6C (s) + 3H 2(g) + 49 KJ ? C 6 H 6(l).

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Ch. 15: Energy and Chemical Change

Ch. 15: Energy and Chemical Change. Sec. 15.3: Thermochemical Equations. Objectives. Write thermochemical equation for chemical reactions and other processes. Describe how energy is lost or gained during changes of state. Calculate the heat absorbed or released in a chemical reaction. Review.

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17-1 Thermochemistry

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Chapter 17

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System strives for minimum Free Energy

System strives for minimum Free Energy. The standard free-energy of reaction ( D G 0 ) is the free-energy change for a reaction when it occurs under standard-state conditions. rxn. a A + b B c C + d D. -. [. +. ]. [. +. ]. =. -. m D G 0 (reactants). S. S. =. f.

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Thermochemistry

Thermochemistry. Chapter 6!. By James Lauer and David Miron. 6.1 The Nature of Energy. Key Terms First law of thermodynamics - The energy of the universe is constant Energy - the capacity to do work or to produce heat

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Ch. 6: Energy and Thermochemistry

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Standard Heats of Reaction

Standard Heats of Reaction. The value of D H for a reaction depends on the temperature and pressure so scientists have agreed upon a set of reference conditions for the comparison of enthalpy data. These conditions are 25 o C and 100. kPa. (SATP).

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Car A 21.6 kJ

Car A 21.6 kJ. Go back to figure 1.6 P= -1250 W from B to A P=1200 W from A to B P=55760 W from A to B P=-16500 W from B to A. Pmax =937.5 mW W=1.875 mJ. W(1)=50 J, W(6)=0 J, W(10)=50 J. 2A 0.5A 40V 25W, 80W and 20W 125W. 20 A 1080 W. 96 mA 48 mA 600 mA -72.96 W. H.W.

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Phase Changes

Phase Changes. How much energy does it take?. Changes in Phase. It takes energy to go from solid to liquid and liquid to gas. The change from one phase to another takes a little extra push of energy in order to get to that next phase. Energy Diagram for Phase Changes. Changes in Phase.

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MASS-ENERGY STOICHIOMETRY

MASS-ENERGY STOICHIOMETRY. A chemical equation which contains the energy change associated with the reaction is called a thermochemical equation. If a thermochemical equation contains either the energy gain or loss or the mass of one reactant or product, it is

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