Heat of Reactions.

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Presentation transcript:

Heat of Reactions

The Nature of Energy Energy - the ability to do work or produce heat. Potential energy Energy of position Kinetic energy Energy of motion E = ½ mv2

The Nature of Energy Law of conservation of energy- Energy can be converted from one form to another but can neither be created or destroyed.

The Nature of Energy State function Property of the system that changes independent of path Is this a state function?

Temperature and Heat Temperature - a measure of the random motions of the components of a substance. Hot water Cold water (90. oC) (10. oC)

Temperature and Heat Heat - flow of energy between two objects due to a temperature difference between the objects. Heat is the way in which thermal energy is transferred from a hot object to a colder object. Hot water Cold water (90. oC) (10. oC) Water Water (50. oC) (50. oC)

Exothermic and Endothermic Processes System – part of the universe on which we focus attention Surroundings – everything else in the universe Burning a match

Exothermic and Endothermic Processes Exothermic – energy flows out of the system Endothermic – energy flows into the system

DH = Change in enthalpy (heat) -DH = exothermic Rx +DH = endothermic Rx

Thermodynamics Thermodynamics – study of energy First law of thermodynamics Energy of the universe is constant

Measuring Energy Changes The common energy units for heat are the calorie and the joule. Calorie – the amount of energy (heat) required to raise the temperature of one gram of water 1oC. Joule – 1 calorie = 4.184 joules

Thermochemistry (Enthalpy) Enthalpy (Heat), H – energy function At constant pressure H is equal to the energy that flows as heat. H = heat

Calorimetry Enthalpy, H is measured using a calorimeter.

Hess’s Law For a particular reaction, the change in enthalpy is the same whether the reaction takes place in one step or a series of steps. Example: N2(g) + 2O2(g)  2NO2(g) H = 68 kJ

ΔHf = (S DH products) – (S DH reactants) Standard enthalpy of formation (ΔHf ) – The change of enthalpy that accompanies the formation of 1 mole of a substance in its standard state from its constituent elements in their standard states ΔHf = (S DH products) – (S DH reactants)