Energy and Physical Changes Energy is transferred during both chemical and physical changes, most commonly in the form of heat

Energy Energy can be kinetic – associated with motion, such as thermal, mechanical, electric, sound Energy can be potential – associated with an object ’ s position, such as in chemical bonds, gravitational, electrostatic (size of charge and distance between charges) Energy is converted from one form to another GOAL: To be able to define energy and to recognize different types of energy

First Law of Thermodynamics The total energy of the universe is constant Energy is conserved -q=+q (heat lost by something equals heat gained by something else) GOAL: To understand that energy is not created or destroy, but transferred between different places and between different types of energy

Temperature and Heat are NOT the Same Thing! Temperature is a measure of the average kinetic energies of the particles in a substance Heat is energy that can be transferred between substances that are at different temperatures Heat will transfer between two objects in contact until thermal equilibrium occurs GOAL: To understand the different between heat and temperature, and to use the two terms correctly

Heat transfer The quantity of heat lost by a hotter object (-q) and the quantity of heat gained by a cooler object (+q) when they are in contact are numerically equal (but opposite direction) Exothermic (-q) heat is transferred from the system to the surroundings Endothermic (+q) heat is transferred from the surroundings to the system GOAL: To be able to recognize exothermic and endothermic in a variety of situations

Heat Transfer during a Temperature Change The quantity of heat transferred to or from an object when its temperature changes depends on: –Quantity of the material (m) –Size of the temperature change (T) –Identity of the material (c) Specific heat capacity – the quantity of heat required to raise the temperature of 1.00g of a substance by one kelvin (J/g. K) GOAL: To know the factors that determine temperature change when heat is applied or removed from an object

Consequences of Specific Heat Capacity Objects with a large c value take more energy to change temperature (compare seat belt buckle with bottle of water, or sand with water at the beach) If objects with different c values are allowed to reach thermal equilibrium, the object with the large c value contains more heat energy (aluminum foil vs baked potato) GOAL: To understand how specific heat capacity affects temperature change as heat is applied or removed from an object

Energy and Changes of State

During a State Change, Energy is used to change the position of particles (PE), BUT NOT the Speed (KE)! Heat of fusion – energy to convert a substance from solid to liquid (J/g) Heat of vaporization – energy to convert a substance from liquid to gas (J/g) NOTICE: The energy required for a change of state is determined by the type of substance and its quantity (mass), BUT NOT Temperature Change!!! GOAL: To be able to calculate the energy lost or gained in a state change

For a State Change: q = m (H fus ) or q = m (H vap ) EXAMPLE: The heat required to turn 10 degree water into 120 degree steam = (heat to raise temp of water to 100 degrees) + (heat to change state) + (heat to raise temp of steam to 120 degrees)

Observe: Cooling of Lauric Acid and Solid-Liquid Equilibrium (Freezing) Discussion –Use these terms: heat/energy, temperature, kinetic energy, potential energy, states, solid, liquid, state change, equilibrium White boards: Draw particle view of a solid Draw particle view of a liquid Draw particle view of the melting/freezing phase change

GOAL: To be able to label a heating/cooling curve with: states (solid, liquid, gas), state/phase changes (boiling/evaporating, condensing, solidifying, freezing), types of energy changes (kinetic or potential), how heat is calculated at each segment (heat of fusion or vaporization, q=mcT)

Energy Units Joule is the SI unit for thermal energy 1 J = 1 kg. m 2 /s 2 Kilojoules are also commonly used The calorie is an older unit for heat; 1 cal = J Dietary Calories are actually 1000 calories GOAL: To use the unit Joules to solve energy problems

q = m c  T Use to find Heat when Temperature is Changing! q is heat in joules m is mass in grams T = T final – T initial Water has a particularly high specific heat; metals have low specific heats GOAL: To be able to calculate heat lost or gained when a temperature change occurs

Assumptions Heat transfers until both substances are at the same temperature We assume no heat is transferred to warm the surroundings (though this is not accurate) The heat that is lost by one substance is equal and opposite in sign to the heat that is gained by the other substance GOAL: To understand these assumptions and apply them to solve Calorimetry problems (begins on slide 17)

Calorimetry Constant pressure calorimetry measures H Constant pressure calorimetry can be done with a coffee-cup calorimeter A reaction changes the temperature of the solution in the calorimeter; measuring the change in the solution allows calculation of the change in the reaction q rxn + q solution = 0 GOAL: To understand that heat lost by one substance equals heat gained by another substance within a closed system; and to be able to use this concept to solve constant pressure calorimetry problems

Thermodynamics – the study of heat and work  E = q + w  E is the change in kinetic and potential energies of the system Positive q is heat going into the system Negative q is heat leaving the system Positive w is work done on the system Negative w is work done by the system Work (of a gas): w = - P(  V) GOAL: To be able to assign signs to heat and work and solve for  E

State Functions A quantity that is the same no matter what path is chosen in going from initial to final Changes in internal energy and enthalpy for chemical or physical changes are state functions Neither heat nor work individually are state functions, but their sum is GOAL: To be able to define state function and recognize that  E and  H are state functions while q and w are not

Enthalpy Changes for Chemical Reactions Measures the change in heat content Enthalpy changes are specific to the identity and states of reactants and products and their amounts H is negative for exothermic reactions and positive for endothermic reactions Values of H are numerically equal but opposite in sign for chemical reactions that are the reverse of each other Enthalpy change depends on molar amounts of reactants and products

2 Methods to find  H rxn Hess’s Law (indirect method) If a reaction is the sum of two or more other reactions, H for the overall process is the sum of the H values of those reactions GOAL: To be able to solve for H rxn using both the indirect and direct methods

C(s) + O 2 (g)  CO 2 (g) H= kJ/mol CO(g) + 1/2O 2 (g)  CO 2 (g) H= kJ/mol _________________________________ C(s) + 1/2O 2 (g)  CO(g) H=?

C(s) + O 2 (g)  CO 2 (g) H= kJ/mol H 2 (g) + 1/2O 2 (g)  H 2 O(l) H= kJ/mol 2C 2 H 2 (g) + 5O 2 (g)  4CO 2 (g) + 2H 2 O(l ) H= kJ/mol __________________________________ 2C(s) + H 2 (g)  C 2 H 2 (g) H=?

Standard Enthalpies of Formation The standard molar enthalpy of formation (H f o ) is the enthalpy change for the formations of 1 mol of a compound directly from its component elements in their standard states The standard state of an element or a compound is the most stable form of the substance in the physical state that exists at standard atmosphere at a specified temperature

Standard Enthalpy of Formation The standard enthalpy of formation for an element in its standard state is zero Most enthalpies of formation values are negative, indicating an exothermic process The most stable compounds have the largest exothermic values

Enthalpies of Formation Enthalpy change for a reaction can be calculated from the enthalpies of formation of the products and reactants (direct method):  f o (products)] –  f o (reactants)] =  rxn o Reactions with negative values of  rxn o are generally product-favored, while positive  rxn o usually indicates a reactant-favored reaction

2H 2 S(g) + 3O 2 (g)  2H 2 O(l) + 2SO 2 (g) H=? SubstanceH f (kJ/mol) H 2 S (g) H 2 O (l) SO 2 (g)-296.1

Application of Enthalpy 2 Al(s) + Fe 2 O 3 (s)  Al 2 O 3 (s) + 2 Fe(l) 2 Al(s) + Fe 2 O 3 (s)  Al 2 O 3 (s) + 2 Fe(l) H rxn = kJ How much heat is released if 1 mole of Al is used? How much heat is released if 1 mole of Al is used? How much heat is released if 4.2 moles of Al is used? How much heat is released if 4.2 moles of Al is used? How much heat is released if 150. g of Al is used? How much heat is released if 150. g of Al is used?