Keep in mind that in our Thermochemistry unit, we already covered Enthalpy as the heat of reaction, and spent time using heat of formation values to calculate the over all change in enthalpy. Entropy and Free Energy can be calculated in a similar way from given values of Thermochemical data in a table or chart.

Watch these short videos and see if you can figure out how the basics of what each of the three terms means, and then see how each of the provided equations is used with given data to solve for the values for change in each. Pay close attention to the spontaneity of the reactions and how values for these can tell us if a reaction will be spontaneous or not.

Simple explanation of the relationship between Enthalpy, Entropy, and Free Energy:

Understanding Entropy (2 min version)

An excellent 5 minute video explaining Free Energy and Entropy:

Sample problem using Hess' Law, Entropy, and Gibbs Free Energy equations:

Please make sure you watch these videos, then tackle the problems pertaining to this topic in your Big Idea #6 packet before Thursday. We'll take 30 minutes or so after school (before practice starts... you can be a few minutes late) to go over these.

See you Thursday!

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ab_review_key.pdf |

review_thermochemistry_key.doc |

heat_of_formation_review_key.pdf |

chemreview_module_17_18_gases.pdf |

1. Were your points good? Explain.

2. Calculate your percent error for your leftover product.

3. What could cause the weight of your leftover product to be larger than theoretically possible? Smaller?

4. How much product should be produced from the reaction if 5.00 grams of your initial solid were used?

Notes: Sodium Carbonate mixed with vinegar. Weight before and after gives mass of CO2 lost. Final product was heated, dried, and leftover sodium acetate is weighed and analyzed.

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chapter2ism.pdf |

chapter1ism.pdf |

review_thermochemistry_key.doc |

a.

b.

c.

d.

e.

f.

1. V2 =

2. T2 =

3. Volume will increase by 4x due to temp, but decrease by 3x due to pressure, so total change is

4. P2 =

5. V2 =

6. V =

7. P =

8. m = 3.8 g

9. mol = 78.125 mol; P =

10. If 1.00 g Br2 gas, then mol = 0.00626 mol = 0.171 L; D =

11. If 1.00 g Ar, then mol = 0.025 mol = 0.606 L; D =

12. If 100 g of Freon, then 16.3 L = 0.727 mol; Molar Mass =

13. Empirical formula = NO2; Molar Mass = 92.02 g/mol; Molecular Formula is

14. Partial Pressure of Ar = 0.469 atm

15. Pressure of H2 = 0.877 atm; mol H2 = 0.283; m =

16. If 1.00 g of air; D =

17. CO2 = 0.45 mol; Volume CO2 =

18. O2 = 0.274 mol; Volume O2 =

19. H2 = 0.0997 mol; Volume H2 =

20. 1.00 L N2 = 1000 mL = 807 g N2 = 28.8 mol; Volume N2 gas =

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ph_curve_data.xls |

Above is the pH Curve file to download and open in Excel. We will be entering your pH d

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