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Chapter 5 Thermochemistry John D. Bookstaver St. Charles Community College Cottleville, MO Chemistry, The Central Science , 11th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten

Energy ,[object Object],[object Object],[object Object]

Potential Energy ,[object Object]

Kinetic Energy ,[object Object],1 2 KE =  mv 2

Units of Energy ,[object Object],[object Object],[object Object],1 J = 1  kg m 2 s 2

Definitions: System and Surroundings ,[object Object],[object Object]

Definitions: Work ,[object Object],[object Object],[object Object]

Heat ,[object Object],[object Object]

Conversion of Energy ,[object Object],[object Object]

First Law of Thermodynamics ,[object Object],[object Object]

Internal Energy ,[object Object]

Internal Energy ,[object Object],[object Object]

Changes in Internal Energy ,[object Object],[object Object],[object Object]

Changes in Internal Energy ,[object Object],[object Object]

 E , q , w , and Their Signs

Exchange of Heat between System and Surroundings ,[object Object]

Exchange of Heat between System and Surroundings ,[object Object],[object Object]

State Functions ,[object Object]

State Functions ,[object Object],[object Object]

State Functions ,[object Object],[object Object],[object Object]

Work ,[object Object],[object Object]

Enthalpy ,[object Object],[object Object],H = E + PV

Enthalpy ,[object Object],[object Object],[object Object],[object Object]

Enthalpy ,[object Object],[object Object],[object Object],[object Object],[object Object]

Endothermicity and Exothermicity ,[object Object]

Endothermicity and Exothermicity ,[object Object],[object Object]

Enthalpy of Reaction ,[object Object],[object Object]

Enthalpy of Reaction ,[object Object]

The Truth about Enthalpy ,[object Object],[object Object],[object Object]

Heat Capacity and Specific Heat ,[object Object]

Heat Capacity and Specific Heat ,[object Object],Specific heat = heat transferred mass  temperature change s = q m   T

Constant Pressure Calorimetry ,[object Object]

Constant Pressure Calorimetry ,[object Object],[object Object]

Bomb Calorimetry ,[object Object],[object Object]

Hess’s Law ,[object Object],[object Object]

Enthalpies of Formation ,[object Object]

Standard Enthalpies of Formation ,[object Object]

Calculation of  H ,[object Object],[object Object],C 3 H 8 ( g ) + 5 O 2 ( g )  3 CO 2 ( g ) + 4 H 2 O ( l ) C 3 H 8 ( g )  3 C ( graphite ) + 4 H 2 ( g ) 3 C ( graphite ) + 3 O 2 ( g )  3 CO 2 ( g ) 4 H 2 ( g ) + 2 O 2 ( g )  4 H 2 O ( l )

Calculation of  H ,[object Object],C 3 H 8 ( g ) + 5 O 2 ( g )  3 CO 2 ( g ) + 4 H 2 O ( l ) C 3 H 8 ( g )  3 C ( graphite ) + 4 H 2 ( g ) 3 C ( graphite ) + 3 O 2 ( g )  3 CO 2 ( g ) 4 H 2 ( g ) + 2 O 2 ( g )  4 H 2 O ( l ) C 3 H 8 ( g ) + 5 O 2 ( g )  3 CO 2 ( g ) + 4 H 2 O ( l )

Calculation of  H ,[object Object],[object Object],[object Object]

[object Object],[object Object],[object Object],Calculation of  H C 3 H 8 ( g ) + 5 O 2 ( g )  3 CO 2 ( g ) + 4 H 2 O ( l )

Energy in Foods ,[object Object]

Energy in Fuels ,[object Object]

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