1. Chemistry 17.4

2. Calculating Heats of Reaction
17.4
Emeralds are composed of the elements chromium, aluminum, silicon, oxygen, and beryllium. What if you wanted to determine the heat of reaction without actually breaking the gems down to their component elements? You will see how you can calculate heats of reaction from known thermochemical equations and enthalpy data.

3. 17.4
Hess’s Law
Hess’s Law
What are two ways that you can determine the heat of reaction when it cannot be directly measured?

4. Hess’s law allows you to determine the heat of reaction indirectly.
17.4
Hess’s Law
Hess’s law allows you to determine the heat of reaction indirectly.
Hess’s law of heat summation states that if you add two or more thermochemical equations to give a final equation, then you can also add the heats of reaction to give the final heat of reaction.

5. 17.4
Hess’s Law
Hess’s law is used to determine the enthalpy change for the formation of CO(g) from its elements. Interpreting Diagrams How does the diagram represent endothermic and exothermic reactions differently?

6. 17.4
Hess’s Law
Hess’s law is used to determine the enthalpy change for the conversion of diamond to graphite. Interpreting Diagrams Which of the reactions shown is an example of decomposition?

7. Standard Heats of Formation
17.4
Standard Heats of Formation
Standard Heats of Formation
For a reaction that occurs at standard conditions, you can calculate the heat of reaction by using standard heats of formation.

8. Standard Heats of Formation
17.4
Standard Heats of Formation
The standard heat of formation (∆Hf0) of a compound is the change in enthalpy that accompanies the formation of one mole of a compound from its elements with all substances in their standard states at 25°C.

9. Standard Heats of Formation
17.4
Standard Heats of Formation

10. Standard Heats of Formation
17.4
Standard Heats of Formation
The Standard Heat of Formation of Water
This enthalpy diagram shows the standard heat of formation of water. Classifying Is this reaction endothermic or exothermic?

11. 17.7

12. 17.7

13. 17.7

14. 17.7

15. for Sample Problem 17.7
Problem Solving Solve Problem 32 with the help of an interactive guided tutorial.

16. Standard Heats of Formation
17.4
Standard Heats of Formation
Standard heats of formation are used to calculate the enthalpy change for the reaction of carbon monoxide and oxygen. Interpreting Diagrams How does this diagram also demonstrate Hess’s law?

17. 17.4 Section Quiz.
17.4.

18. 17.4 Section Quiz.
1. According to Hess’s law, it is possible to calculate an unknown heat of reaction by using
heats of fusion for each of the compounds in the reaction.
two other reactions with known heats of reaction.
specific heat capacities for each compound in the reaction.
density for each compound in the reaction.

19. 17.4 Section Quiz.
2. The heat of formation of Cl2(g) at 25°C is
the same as that of H2O at 25°C.
larger than that of Fe(s) at 25°C.
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zero.

20. 17.4 Section Quiz.
3. Calculate  H0 for NH3(g) + HCl(g)  NH4Cl(s) Standard heats of formation: NH3(g) = 45.9 kJ/mol, HCl(g) = 92.3 kJ/mol, NH4Cl(s) = 314.4 kJ/mol
176.2 kJ
360.8 kJ
176.2 kJ
268 kJ .

21. Solve the Concept Map with the help of an interactive guided tutorial.

22. END OF SHOW