thermochemistry powerpoint #2. enthalpy the chemical and physical changes that occur around us...
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Thermochemistry
Powerpoint #2
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Enthalpy
• The chemical and physical changes that occur around us essentially occur at constant atmospheric pressure.
• Most commonly, the only kind of work produced by chemical and physical changes open to the atmosphere is the mechanical work associated with change in the volume of the system.
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Pressure – Volume Work
• The work involved in the expansion or compression of gases if called P-V work.
• When pressure is constant, as in our example, the sign and magnitude of the pressure-volume work is given by
• w = -P DV
• The negative sign is necessary to conform with the sign conventions given earlier.
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W = - PΔV
• When the volume expands, ΔV is a positive quantity and w is a negative quantity.
• Energy leaves the system as work, indicating that work is done by the system on the surroundings.
• When the volume contracts, ΔV is a negative quantity and w is a positive quantity.
• Energy enters the system as work, indicating that work is done on the system by the surroundings
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Enthalpy, denoted H
• From a Greek word meaning “to warm”
• Accounts for heat flow in processes occurring at constant pressure when no forms of work are performed other than P-V work.
• H = E + PV (its definition)
• Is a state function because internal energy, pressure, and volume are all state functions.
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Enthalpy
• When a change occurs at constant pressure, the change in enthalpy is given by the following relationship:
• ΔH = DE + PDV
• the heat at constant pressure qp can be calculated from
• ΔE = qp+ w = qp- PΔV
• qp= ΔE + P ΔV = ΔH
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• The change in enthalpy equals the heat gained or lost at constant pressure.
• Because qp is something we can either measure or readily calculate and because so many physical and chemical changes occur at constant pressure, enthalpy is a more useful function than internal energy.
• For most reactions the difference in ΔH and ΔE are so small because P ΔV is small.
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Enthalpies of Reaction
• Because ΔH = ΔH final – ΔH initial, the enthalpy change for a chemical reaction given by the enthalpy of the products minus the enthalpy of the reactants.
• ΔH = ΔHproducts – ΔHreactants
• Enthalpy of reaction–the enthalpy change that accompanies a reaction
• Sometimes called –Heat of reaction
• ΔHrxn
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Guidelines when using thermochemical equations:
• 1. Enthalpy is an extensive property –ΔH is directly proportional to the amount of reactant consumed in the process.
• 2. The enthalpy change for a reaction is equal in magnitude, but opposite in sign, to the ΔH for the reverse reaction.
• 3. The enthalpy change for a reaction depends on the state of the reactants and products. Important to note the states in your equations.
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Calorimetery
• Measurement of heat flow.
• Use a calorimeter.
• The temperature change experienced by an object when it absorbs a certain amount of heat.
• It is a unique value for all substances.
• Heat Capacity – the amount of heat required to raise its temperature by 1 K.
• • The greater the heat capacity, the greater the heat required to
produce a given increase in temperature.
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• The heat capacity of one mole of a substance.
• C – has units of J/gxK or J/gx◦C
• Specific heat capacity (specific heat) –the heat capacity of one gram of a substance
• q• C = ------ or q = C x m x ΔT• m x ΔT
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Bomb Calorimetry
• Constant volume calorimeter is called a bomb calorimeter.
• Material is put in a container with pure oxygen. Wires are used to start the combustion. The container is put into a container of water.
• The heat capacity of the calorimeter is known and tested.
• Since ΔV = 0, PΔV = 0, ΔE = q
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Bomb Calorimeter
• thermometer
• stirrer
• full of water
• ignition wire
• Steel bomb
• sample
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Properties
• Intensive properties not related to the amount of substance.
• density, specific heat, temperature.
• Extensive property - does depend on the amount of stuff.
• Heat capacity, mass, heat from a reaction.
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Hess’s Law
• Enthalpy is a state function.
• It is independent of the path.
• We can add equations to come up with the desired final product, and add the ΔH
• Two rules
• If the reaction is reversed the sign of ΔH is changed
• If the reaction is multiplied or divided, so is ΔH
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Remember…
• H is a state function, so for a particular set of reactants and products, ΔH is the same whether the reaction takes place in one step or in a series of steps.
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Enthalpies of Formation
• The enthalpy change associated with the formation of a compound from its constituent elements.
• Labeled ΔHf
• The enthalpy change for a reaction at standard conditions (25ºC, 1 atm , 1 M solutions). These are standard state conditions.
• Symbol ΔHfº
• When using Hess’s Law, work by adding the equations up to make it look like the answer.
• The other parts will cancel out.
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Standard Enthalpies of Formation
• Hess’s Law is much more useful if you know lots of reactions.
• Made a table of standard heats of formation. The amount of heat needed to for 1 mole of a compound from its elements in their standard states.
• Standard states are 1 atm, 1M and 25ºC
• For an element it is 0