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THERMOCHEMISTRY

THERMOCHEMISTRY

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THERMOCHEMISTRY

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  1. THERMOCHEMISTRY HEAT CAPACITY, SPECIFIC HEAT, ENDOTHERMIC/EXOTHERMIC, ENTHALPY, STANDARD ENTHALPIES, CALORIMETERY

  2. INTROTOTHERMOCHEMISTRY • Chemical rxns involve changes in energy • Breaking bonds___________________ • Forming bonds___________________ • The study of the changes in energy in chem rxns is called _________________. • The energy involved in chemistry is real and generally a measurable value • Energy units are numerous, but we will concentrate on the ______ (SI base unit) and the ______ (little c, big C is the food Calorie or a kilocalorie) • 1 calorie = ______________

  3. There are three methods used to transfer heat energy • ___________ – transfer of heat through direct contact • ___________ – transfer of heat through a medium like air or water • _____________ – transfer of heat by electromagnetic radiation

  4. WHAT IS HEAT? • Hot & cold, are automatically associated with the words heat and temperature • Heat & temperature are NOT synonyms • The temperature of a substance is directly related _____________________ ____________, specifically its: • The ___________ Energy defines the temperature • Particles vibrating fast = ______ • Particles vibrating slow = ______

  5. A Hot Spoon An Ice Cold Spoon energy transfer • _________ energy is transferred from one particle to the next (a.k.a. conduction) • Sometimes this energy can be transferred from one object to another and influence physical properties • The more energy an object has the more energy is transferred

  6. 2 Hot Spoons • Thermal energy is the total energy of all the particles that make up a substance • Kinetic energy from_________________ • Potential energy from_______________(within or between the particles) • Thermal energy is dependent upon the amount or mass of material present (KE =_________) • Thermal energy is also related to the _________ __________

  7. Different type of materials • May have the same temp, same mass, but different ________________ • Affected by the potential energy stored in chemical bonds or the ________________ __________________ • So it is possible to be at same temp (same KE) ________________________ _______________ • The different abilities to hold onto or release energy is referred to as the substance’s _____________

  8. ________ energy can be transferred from object to object through direct contact • __________________,transferring energy from molecule to molecule

  9. HEAT RESERVOIR HEAT CAPACITY • The measure of how well a material absorbs or releases heat energy is its heat capacity • It can be thought of as a reservoir to hold heat, how much it holds before it overflows is its __________________ • Heat capacity is a physical property unique to a particular material • Water takes_______of energy to raise temp 1 °C • Steel takesonly_________of energy to raise temp 1 °C

  10. SPECIFIC HEAT CAPACITY • The amount of energy it takes to raise the temp of a standard amount of an object ____ is that object’s specific heat capacity (__) • The standard amount =_________ • Specific heats can be listed on data tables • Smaller the specific heat  the _______ _______ it takes the substance to feel hot • Larger the specific heat  the _________ ________ it takes to heat a substance up (______________________________)

  11. Specific heats and heat capacities work for gains in heat and in losses in heat • Smaller the specific heat the_________ it takes the substance to cool off • Larger the specific heat the_________ it takes the substance to cool off • Specific heat capacity values are used to calculate changes in energy for chemical rxns • It’s important for chemists to know how much energy is ___________________ in chemical rxns

  12. CHANGE IN HEAT ENERGY (__________) • The energy used or produced in a chem rxn is called the ___________________ • Burning a 15 gram piece of paper produces a particular amount of heat energy or a particular amount of enthalpy • Enthalpy is a value that also contains a component of direction (_____________ ____________) • Heat gained is the ______ direction; ie exo- • Heat lost is the _______ direction; ie endo-

  13. HEAT HEAT HEAT HEAT

  14. Chemical rxns can be classified as either: • ____________ a reaction in which heat energy is generated (a___________) • _____________ reaction in which heat energy is absorbed (a___________) • Exothermic rxns typically feel _______ as the rxn proceeds • Give off heat energy, sometimes quite alot • Endothermic rxns typically feel _____ the longer the rxn proceeds • Absorb heat energy, sometimes enough to get very cold

  15. Exothermic rxn • To a cold camper, the important product here is the heat energy

  16. In an exothermic process the amount of energy given off is more than the initial energy invested. So the products are less in energy than the reactants.

  17. Endothermic rxn • Similar system as what is found in cold packs

  18. Activation Energy Energy Lost ENDOTHERMIC RXN In an endothermic process more energy is required to cause the rxn to proceed than obtained in return. So the products are less in energy than the reactants.

  19. CHANGE IN ENTHALPY • Most common measurement of the energy or enthalpy in a reaction is actually a ____________________ (____) • DHrxn = ∑Hproducts - ∑Hreactants • The enthalpy absorbed or gained (changed) in a rxn is dependent on the _______________ of material reacting • We can stoichiometrically calculate how much energy a rxn uses or produces • DH values can be provided with a rxn equn and have magnitude & direction of transfer (+ or -)

  20. USING H IN CALCULATIONS • Chemical reaction equations are very powerful tools. • Given a rxn equation with an energy value, We can calculate the amount of energy produced or used for any given amount of reactants. (For Example) How much heat will be absorbed for 1.0g of H2O2 to decompose in a bombardier beetle to produce a defensive spray of steam

  21. Molar mass Analyze: we know that if we had 2 mols of H2O2 decomposing we would use 190kJ of heat, but how much would it be if only 1.0 g of H2O2 Therefore: we have to convert our given 1.0 g of H2O2 to moles of H2O2 1mol H2O2 1.0g H2O2 = ______ mol __g H2O2

  22. Rxn equation Therefore: with 2 moles of H2O2 it requires the use of 190 kJ of energy, but we don’t have 2 moles we only have .02941 mols of H2O2, so how much energy would the bug require? ___kJ .02941 mol = ___kJ _molH2O2

  23. Example #2 How much heat will be released when 4.77 g of ethanol (C2H5OH) react with excess O2 according to the following equation: C2H5OH+3O2 2CO2+3H2O H = -1366.7kJ analyze: we know that if we had 1 mol of ethanol(assuming coefficient of 1 in rxn equation) burning we would produce 1366.7kJ of heat, but how much would it be if only we only had 4.77 g of ethanol?

  24. C2H5OH+3O22CO2+3H2O H = -1366.7kJ 1mol C2H5OH _______kJ 4.77g C2H5OH 1mol C2H5OH __g C2H5OH = ____ kJ

  25. Classroom Practice 1 Ethanol, C2H5OH, is quite flammable and when 1 mole of it burns it has a reported H of -1366.8 kJ. How much energy is given off in the combustion of enough ethanol to produce 12.0 L of Carbon dioxide @ 755 mmHg and 25.0°C? 1 C2H5OH+ 3 O2 2 CO2+ 3 H2O H= -1366.8 kJ

  26. FINAL TEMP – INITIAL TEMP SPECIFIC HEAT MASS • We can also track energy changes due to temp changes, using _______________: H = • If the temp difference is positive • The rxn is ___________ because the final temp is greater than the initial temp • So the enthalpy ends up __________ • if the temp change is negative • the enthalpy ends up___________ • the rxn absorbed heat into the system, soit’s________________

  27. if you drink 4 glasses of ice water at 0°C, how much heat energy is transferred as this water is brought to body temp? each glass contains 250 g of water & body temp is 37°C. • mass of 4 glasses of water: • _________________________________ • change in water temp: • _________________________________ • specific heat of water: • _______________________________

  28. Example 2: 500 g of a liquid is heated from 25°C to 100°C. The liquid absorbs 156,900 J of energy. What is the specific heat of the liquid and identify it. DH = mCDT

  29. Classroom Practice 2 An orange contains 445 kJ of energy. What volume of water could this same amount of energy raise from a temp of 25.0°C to the boiling point? Water at 0.00°C was poured into 30.0g of water in a cup at 45.0°C. The final temp of the water mixture was 19.5°C. What was the mass of the 0.00°C water?

  30. Enthalpy is dependent on the________of the rxn • It’s important to have a_____________of conditions, which allows us to compare the affect of temps, pressures, etc. On different substances • Chemist’s have defined a standard set of conditions • Stand. Temp =___________________ • Stand. Press =___________________ • Enthalpy produced in a rxn under standard conditions is the ____________________

  31. Standard enthalpies can be found on tables measured as standard__________ ____________, enthalpies of combustion, _________________, enthalpies of fusion, and enthalpies of vaporization • Enthalpy of formation (Hf) is the amount of energy involved in the formation of a compound from its component elements. • Enthalpy of combustion (Hcomb) is the amount of energy produced in a combustion rxn. • Enthalpy of solution (Hdiss) is the amount of energy involved in the dissolving of a compound

  32. Enthalpy of fusion (Hfus) is the amount of energy necessary to melt a substance. • Enthalpy of vaporization (Hvap) is the amount of energy necessary to convert a substance from a liquid to a gas. • All of these energies are measured very carefully in a laboratory setting under specific conditions • _________________________________ • These measured energies are reported in tables to be used in calculations all over the world.

  33. Calorimetry is the process of measuring heat energy • Measured using a device called a ________________ • Uses the heat absorbed by H2O to meas-ure the heat _______ by a rxn or an object • The amount of ________________ by the water is ___________ the amount of heat ____________ by the rxn Hsys is the system or what is taking place in the main chamber (rxn etc.) And Hsur is the surroundings which is generally water. HSYS=-HSUR

  34. A COFFEE CUP CALORIMETER USED FOR A REACTION IN WATER, OR JUST A TRANSFER OF HEAT. A BOMB CALORIMETER USED WHEN TRYING TO FIND THE AMOUNT OF HEAT PRODUCED BY BURNING SOMETHING.

  35. CALORIMETRY • With calorimetry we use the sign of what happens to the water • When the water loses heat into the system it obtains a _____________ (-Hsurr) • ___________ (+Hsys) • When the water gains heat from the system it obtains a _____________ (+Hsurr) • _________ (-Hsys)

  36. - D H -D H rxn + D H water ______ _____ _____ _____ water HEAT HEAT + D H HEAT HEAT rxn = = WATER = SURROUNDINGS WATER = SURROUNDINGS + SIGN MEANS HEAT WAS ABSORBED BY THE RXN - SIGN MEANS HEAT WAS RELEASED BY WATER SYSTEM SYSTEM - SIGN MEANS HEAT WAS RELEASED BY THE RXN + SIGN MEANS HEAT WAS ABSORBED BY WATER EXOTHERMIC ENDOTHERMIC

  37. CALORIMETRY • You calculate the amount of heat absor-bed by the water (using H= mCT) • Which leads to the amount of heat given off by the rxn • you know the mass of the water (___ _______________) • you know the specific heat for water (__________________) • and you can measure the change in the temp of water (__________________)

  38. A chunk of Al that weighs 72.0g is heated to 100°C is dropped in a calorimeter containing 120ml of water at 16.6°C. the H2O’s temp rises to 27°C. HAl= • mass of Al = ____ • Tinitial of Al = _____ • Tfinal of Al = _____ • CAl = _________ (from table) HAl

  39. We can do the same calc with the water info = HH2O • Mass of H2O= _____ • Tinitial of H2O= _____ • Tfinal of H2O = _____ • CH2O= __________ (from table) HH2O Equal but opposite, means that the Al decreased in temp, it released its stored heat into the H2O, causing the temp of the H2O to increase.

  40. When a 4.25 g sample of solid NH4NO3 dissolves in 60.0 g of water in a calori-meter, the temperature drops from 21.0°C to 16.9°C. Calculate the energy involved in the dissolving of the NH4NO3. DHwater = (mwater)(Cwater)(DTwater)

  41. Classroom Practice 3 A coffee-cup calorimeter with a mass of 4.8 g is filled with water to mass of 250 g. The water temperature was 24.2C before 3.2 g of NaOH pellets was added to the water. After the NaOH pellets had dissolv-ed the temp of the water registered 85.8C. How much heat did the H2O absorb, and how much heat did the NaOH produce? 41.0g of glass at 95°C is placed in 175 g of Water at 19.5°C in a calorimeter. The temps are allowed to equalize. What is the final temp of the glass/water mixture? (Water = 4.18J/g°C; Glass = 8.78J/g°C)