Chapter 11 LA #1 driving forces 1. Chapter 11 explores the ____________ behind chemical reactions and explains why reactions occur. 2. chemical reactions are often accompanied by ____________ in energy, ____________ in disorder or ____________. decrease increase both

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

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

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

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

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

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

16. CH4 + 2O2  CO2 + 2H2O Hcomb = -891 kJ 17. H2O(g)  H2O(l) H = - 40.6 kJ H2O(g)  H2O(l) endothermic or exothermic? - 8910 kJ + heat exothermic

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 = + 40.6 kJ H2O(l)  H2O(g) endothermic or exothermic? closer to low low + heat endothermic

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

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