1. Chapter 11 LA #1 driving forces
1. Chapter 11 explores the ____________ behind chemical reactions and explains why reactions occur chemical reactions are often accompanied by ____________ in energy, ____________ in disorder or ____________.
decrease
increase
both

2. 3. Temperature
represents the ____________ of thermal energy
_______________ on the quantity of matter
a measure of the
___________________ of the particles in a sample of matter
intensity
does not depend
average kinetic energy

3. 4. The particles in a body at a high temperature have a _______ (higher or lower) average kinetic energy than the particles in a body at a low temperature.
5. Which has a higher temperature ---- a cup of boiling water or a pot of boiling water?
higher
same temperature

4. quantity depends more 2 liters of water 6. Heat
indicates the ___________ of thermal energy
__________ on the quantity of matter
7. for the same type of matter, a larger mass has ________ (more or less) thermal energy than a smaller mass at the same temperature
8. Which has more thermal energy ----
2 liters of water or 1 liter of water at the same temperature?
quantity
depends
more
2 liters of water

5. 9. Thermodynamics deals with ____________________ of all kinds.
10. Thermodynamic properties
_________________
energy transformations
enthalpy
entropy
Gibb’s energy

6. 11. Enthalpy - the heat energy that is "inside" an object or substance
______________, _________________, or ____ - the amount of heat energy absorbed or released during a chemical reaction
12. heat of formation - heat energy absorbed or released during the _________ of one mole of a compound from its elements at 298 K and 1 atm pressure
heat of reaction
enthalpy change ΔH
synthesis

7. 13. heat of solution - heat energy absorbed
13. heat of solution - heat energy absorbed or released when a substance _________ in a solvent
14. heat of combustion - heat energy released when a substance reacts with ____________ to form _______________ and ______
15. the _______ the quantity of the substance undergoing a chemical or physical change, the _____ heat will be transferred
dissolves
oxygen gas
carbon dioxide
water
greater
more

8. 16. CH4 + 2O2  CO2 + 2H2O Hcomb = -891 kJ
17. H2O(g)  H2O(l) H = kJ
H2O(g)  H2O(l)
endothermic or exothermic? kJ
+ heat
exothermic

9. 18. in liquid H2O, water molecules are much ________ (closer to or further away from) each other than water vapor;
_____ energy state; ____ enthalpy state
19. H2O(l)  H2O(g) H = kJ
H2O(l)  H2O(g)
endothermic or exothermic?
closer to
low
low
+ heat
endothermic

10. 20. in gaseous H2O, water molecules are
20. in gaseous H2O, water molecules are widely separated; _____ energy state; _____ enthalpy state
21. a reaction that liberates energy (exothermic; _________ in energy) is _____ (more or less likely to occur) than one that does not.
high
high
decrease
more

11. more
22. the ______ energy released by an exothermic reaction, the ________ the decrease in enthalpy, and the _____ likely it is that the reaction will be spontaneous.
23. spontaneous change - a change that will occur because of the ___________________ once it is initiated.
greater
more
nature of the system