Lecture 23 - Thermochemistry II

Thursday, April 11, 2024

1:30 PM

Please complete course evaluations https://boisestate.bluera.com/boisestate/ +1% if >70% respond Please complete this questionnaire to reflect on ﷟HYPERLINK "https://boisestatecanvas.instructure.com/courses/28699/quizzes/249663"Chemistry Attitudes and Experiences (End of Semester) Class notes (1-22): https://bricejurban.github.io/CHEM111/ Assignments this week: ﷟HYPERLINK "https://boisestatecanvas.instructure.com/courses/28699/assignments/1017881"HW 12 Thermochemistry due next Wednesday Complete Practice Exam. To be posted tonight or tomorrow Read Chapter 14 Reminders: Midterm 4 is next Thursday My CIC (EDUC 107) Hours: Friday 11AM - 1PM Office Hours (SCNC 314 or Zoom): ﷟HYPERLINK "https://calendly.com/bricejurban/office-hours"By appointment Today (4/11) Standard Molar Enthalpies of Formation Average Molar Bond Enthalpies Calorimetry Next Tuesday (4/16) Heating Curves Intermolecular Forces Phase Diagrams Crystals (?) The End of CHEM 111 Content? Molar Enthalpies of Formation The molar enthalpy of formation ΔH°f of a substance is the reaction that forms one mole of that compound from its standard elements. 2 C(s) + H2(g) → C2H2(g) Mg(s) + C(s) + 3/2 O2(g) → MgCO3(s) 5 C(s) + 11/2 H2(g) + ½N2(g) + O2(g) → C5H11NO2(g) ΔH°f = +227.4 kJ ΔH°f = –1095.8 kJ ΔH°f = –455.1 kJ etc. Actually carrying out these reactions from the elements is usually impossible, or nearly so, so these values must be determined by careful experimentation usually involving multiple reactions and then making use of Hess's Law. For example, if we want to find the molar enthalpy of formation ΔH°f of acetylene gas (C2H2), we can get a pure sample of acetylene and measure the heat of combustion (or look this value up in a table): C2H2(g) + 5/2O2(g) → 2CO2(g) + H2O(l) ΔH°rxn = –1300 kJ This then gives us two simpler molecules which we can easily find in the tabulated molar enthalpies of formation ΔH°f Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings
This then gives us two simpler molecules which we can easily find in the tabulated molar enthalpies of formation ΔH°f C(s) + O2(g) → CO2(g) ΔH°f = –393.5 kJ H2(g) + ½O2(g) → H2O(l) ΔH°rxn = –285.8 kJ *Note that heats of combustions give water as a liquid, not as a gas. Method 1: Use Hess's Law Method 2: Use Molar Enthalpies of Formation ΔH°rxn = nΔH°f [products] - nΔH°f [reactants] I passed out an ﷟HYPERLINK "https://boisestatecanvas.instructure.com/courses/28699/modules/items/3050437"reference table that should have most of the values needed to calculate the following. However here are some other references that might be of interest: Calculate the value of ΔH°rxn using ΔH°f values then determine whether each reaction is endothermic or exothermic. Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings
then determine whether each reaction is endothermic or exothermic. H2(g) + F2(g) → 2HF(g) 3H2(g) + N2(g) → 2 NH3(g) 2CO(g) + O2(g) → 2CO2(g) 2 NO(g) + O2(g) → 2NO2(g) pro-nzlI9kta.jpeg pro-L0ekgxgw.jpeg Bond Enthalpies Untitled picture.png Machine generated alternative text: Energy absorbed o o o Ato ms Energy as heat released o Step 2 bond formation tep 1 bond breaking Reactants Products Untitled picture.png Machine generated alternative text: energy required to break all the AHO bonds in the reactant molecules energy evolved as heat upon the formation of all the bonds in the product molecules Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings
Untitled picture.png Machine generated alternative text: energy required to break all the AHO bonds in the reactant molecules energy evolved as heat upon the formation of all the bonds in the product molecules Untitled picture.png Untitled picture.png Machine generated alternative text: B Ond O-H 0-0 NT-H c-o c-o NEN c-c CI-CI Br-Br C-F c-CI H-CI C-Br H-Br C-N Molar bond enthalpy, Hw/kJ.m01-l 464 142 351 502 730 347 615 811 414 439 331 276 293 615 Bond CEN H-S Molar bond enthalpy, Hw/kJ .mol-l 890 390 159 418 945 155 243 192 435 565 431 368 364 The enthalpy change for the equation ClF3(g) → Cl(g) + 3 F(g) is 523 kJ·mol–1. Calculate the average molar bond enthalpy of a chlorine-fluorine bond in a ClF3 molecule. Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings
Use the molar bond enthalpy data to estimate the value of ΔH°rxn for the equation: CCl4(g) + 2 F2(g) → CF4(g) + 2 Cl2(g) Calculate the average molar bond enthalpy of a carbon–hydrogen bond in a CH4 molecule. Given that ΔH°f[H(g)] = 218.0 kJ·mol−1 ΔH°f[C(g)] = 716.7 kJ·mol−1 ΔH°f[CH4(g)] = −74.6 kJ·mol−1 Why is there a slight difference between this value and the molar bond enthalpy of a carbon–hydrogen bond listed in Table 14.5 Ammonia reacts with oxygen to form nitrogen dioxide and steam, as follows: 4NH3(g) + 7O2(g) ---> 4NO2(g) + 6H2O(g) ΔH°rxn = –1135 kJ Determine the bond energy of the N−O bond of NO2 Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink 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Determine the bond energy of the N−O bond of NO2 pro-gm70r8hp.jpeg Determine the enthalpy for the following reaction: C(s) + CO2(g) ---> 2CO(g) The enthalpy of sublimation of graphite, C(s) is 719 kJ/mol Determine the enthalpy of combustion of propane (C3H8) using bond enthalpies. Then compare it with the combustion value listed in the reference above. 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The Measurement of Heat Transfer (Calorimetry) Calorimetry is the measure of heat is transferred due to: _________________________________________________________ A substances resistance to temperature changes is known as the ____________________ When heat capacity has the units ____________ it is referred to as _____________ When heat capacity has the units ____________ it is referred to as _____________. Untitled picture.png Machine generated alternative text: copper block specific heat of copper aluminum block specific heat Of aluminum water specific heat Of water Specific Heat Capacity - warms up and cools down quickly as takes much less energy to change its temparature Specific Heat Capacity - warms up and cools down slowly as it takes up much more energy to change its temperature Substance Phase Specific heat capacity, cP J⋅g−1⋅K−1 Molar heat capacity, CP,m J⋅mol−1⋅K−1 Air (typical room conditions) gas 1.012 29.19 Argon gas 0.5203 20.7862 Carbon dioxide CO2 gas 0.839 36.94 Helium gas 5.1932 20.7862 Hydrogen gas 14.30 28.82 Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings 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Untitled picture.png Machine generated alternative text: copper block specific heat of copper aluminum block specific heat Of aluminum water specific heat Of water Specific Heat Capacity - warms up and cools down quickly as takes much less energy to change its temparature Specific Heat Capacity - warms up and cools down slowly as it takes up much more energy to change its temperature Hydrogen gas 14.30 28.82 Hydrogen sulfide H2S gas 1.015 34.60 Methane CH4 at 2 °C gas 2.191 35.69 Nitrogen gas 1.040 29.12 Neon gas 1.0301 20.7862 Oxygen gas 0.918 29.38 Water at 100 °C (steam) gas 2.03 36.5 Ammonia NH3 liquid 4.700 80.08 Ethanol C2H5OH liquid 2.44 112 Water at 25 °C liquid 4.1816 75.34 Aluminium solid 0.897 24.2 Copper solid 0.385 24.47 Glass solid 0.84 Gold solid 0.129 25.42 Iron solid 0.449 25.09 Lead solid 0.129 26.4 Paraffin wax C25H52 solid 2.5 (avg) 900 Silver solid 0.233 24.9 Steel solid 0.466 Uranium solid 0.116 27.7 Water at −10 °C (ice) solid 2.05 38.09 A calorimeter is used to measure the heat of chemical reactions, physical changes and heat capacity Constant pressure calorimeters measure the change in heat of a reaction occurring in solution. The heat transfer at constant pressure qp is known as the enthalpy change ΔH. Constant volume (bomb) calorimeters resists change in volume and are used to measures the change in heat of combustion reactions. The heat transfer at constant volume qv is known as the internal energy change ΔU. A calorimeter can also measure the specific heat capacity (c) of a substance at constant pressure cP or at constant volume cV. For instance a hot metal (M) transfers heat (q) to the cool water bath (W) until both are at equilibrium. The change in temperature can be measured to find c. CNX_Chem_05_02_Calorim.jpg Untitled picture.png Machine generated alternative text: Motorized stirrer Ignition wires Heat Thermometer Insulated container Sealed bomb 02(g) Sample cup Water Untitled picture.png Machine generated alternative text: System Surroundings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings
CNX_Chem_05_02_Calorim.jpg Untitled picture.png Machine generated alternative text: Motorized stirrer Ignition wires Heat Thermometer Insulated container Sealed bomb 02(g) Sample cup Water Untitled picture.png Machine generated alternative text: System Surroundings If Beaker A contains 50.0 g of water (cp = 4.18 J/g·°C) and Beaker B contains 50.0 g of acetone (cP = 2.15 J/g·°C), both at the same temperature. If both beakers are heated with the same amount of energy, which liquid will have the higher final temperature? The equation for heat transfer is: How much energy is released when 20.0 g of water is cooled from 50°C to 30°C? (cP, water = 4.18 J/g·°C) Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings
When a 50.0 g block of copper was heated with 1046 J of energy, the temperature increased from 10.0°C to 64.3°C. What is the specific heat of copper? What is the final temperature when a 90.0 g of aluminum at 20°C releases 500 J of energy? (cP,Al = 0.897 J/g·°C) A 31.1 g wafer of pure gold (cP, Au = 0.129 J/g·°C) initially at 69.3 °C is submerged into 64.2 g of water (cP, water = 4.18 J/g·°C) at 27.8 °C in an insulated container. What is the final temperature of both substances? 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Heat transfer during Phase Transitions (Heating and Cooling Curves) (Next Tuesday) During the process of melting energy is needed to change a substance from ___________ to ____________ At constant pressure this is known as the __________ of _________ (ΔHfus) and is typically given in kJ/mol The opposite process is known as ______________________ and the energy change is equivalent to __________ A related process that requires much more energy is the enthalpy of vaporization (__________ to ________) (ΔHvap) The opposite process is known as ______________________ and the energy change is equivalent to __________ These are latent heat processes meaning the phase change occur at constant temperature Substance Molar Heat of fusion (kJ/mol) Melting point (°C) Molar Heat of vaporization (kJ/mol) Boiling point (°C) Ammonia (NH3) 5.6572 −77.74 23.32 −33.34 Carbon dioxide (CO2) 8.10 −78 25.3 -78.46 Hydrogen 0.12 −259 0.917 −253 Lead 4.8 327.5 180 1750 Methane (CH4) 0.95 −182.6 8.20 −161.6 Nitrogen 0.720 −210 5.60 −196 Oxygen 0.445 −219 6.82 −183 Water 6.02 0 40.80 100 How much energy is required to melt 20.0 g of lead at -259 °C? Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings Ink Drawings
How much heat is released by the condensation of 2.88 mols of oxygen at -183 °C? When studying the energy required to transition between phases, it is useful to plot the temperature versus energy. When energy is absorbed by the system this is known as a ____________________ and when it is released by the system it is a _____________________ Untitled picture.png Machine generated alternative text: heat (J)
Find the energy required for 20.0 g of ice at -10 °C to change to steam at 130 °C.

 

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