Principles of General Chemistry
3rd Edition
ISBN: 9780073402697
Author: SILBERBERG, Martin S.
Publisher: McGraw-Hill College
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Chapter 6, Problem 6.11P
Why can we measure only changes in enthalpy, not absolute enthalpy values?
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Chapter 6 Solutions
Principles of General Chemistry
Ch. 6 - Prob. 6.1PCh. 6 - An adiabatic process is one that involves no heat...Ch. 6 - Name a common device used to accomplish each...Ch. 6 - Prob. 6.4PCh. 6 - A system receives 425 J of heat from and delivers...Ch. 6 - A system releases 255 cal of heat to the...Ch. 6 - Prob. 6.7PCh. 6 - Prob. 6.8PCh. 6 - The nutritional calorie (Calorie) is equivalent to...Ch. 6 - Classify the following processes as exothermic or...
Ch. 6 - Why can we measure only changes in enthalpy, not...Ch. 6 - Draw an enthalpy diagram for a general exothermic...Ch. 6 - Prob. 6.13PCh. 6 - Prob. 6.14PCh. 6 - Prob. 6.15PCh. 6 - Write a balanced equaĂ¼on and draw an approximate...Ch. 6 - Write a balanced equation and draw an approximate...Ch. 6 - The circles represent a phase change at constant...Ch. 6 - The scenes below represent a physical change...Ch. 6 - What data do you need to determine the specific...Ch. 6 - Is the specific heat capacity of a substance an...Ch. 6 - Find q when 22.0 g of water is heated from 25.0C...Ch. 6 - Prob. 6.23PCh. 6 - A 295-g aluminum engine part at an initial...Ch. 6 - A 27.7-g sample of the radiator coolant ethylene...Ch. 6 - Two iron bolts of equal mass-one at 100.C, the...Ch. 6 - Prob. 6.27PCh. 6 - When 155 mL of water at 26C is mixed with 75 mL of...Ch. 6 - Prob. 6.29PCh. 6 - Prob. 6.30PCh. 6 - Prob. 6.31PCh. 6 - When 25.0 mL of 0.500MH2SO4 is added to 25.0 mL of...Ch. 6 - Would you expect O2(g)20(g) to have a positive or...Ch. 6 - Is H positive or negative when 1 mol of water...Ch. 6 - Prob. 6.35PCh. 6 - Consider the following balanced thermochemical...Ch. 6 - When 1 mol of NO(g) forms from Its elements, 90.29...Ch. 6 - Prob. 6.38PCh. 6 - Liquid hydrogen peroxide, an oxidizing agent in...Ch. 6 - Prob. 6.40PCh. 6 - Most ethylene (C2H4), the starting material for...Ch. 6 - Prob. 6.42PCh. 6 - Prob. 6.43PCh. 6 - Calculate H for Ca(s)+12O2(g)+CO2(g)CaCO3(s) Given...Ch. 6 - Calculate H for 2NOCl(g)N2(g)+O2(g)+Cl2(g) given...Ch. 6 - Write the balanced overall equation (equation 3)...Ch. 6 - Write the balanced overall equation (equation 3)...Ch. 6 - Diamond and graphite are two crystalline forms of...Ch. 6 - Prob. 6.49PCh. 6 - Prob. 6.50PCh. 6 - Use Table 6.3 or Appendix B to write a balanced...Ch. 6 - Prob. 6.52PCh. 6 - Calculate Hrxno for each of the following:...Ch. 6 - Calculate Hrxno for each of the following:...Ch. 6 - Copper(I) oxide can be oxidized to copperr (II)...Ch. 6 - Prob. 6.56PCh. 6 - Nitroglycerine, C3H5(NO3)3(l), a powerful...Ch. 6 - The common lead-acid car battery produces a large...Ch. 6 - Stearic acid (C18H36O2) is a fatty acid, a...Ch. 6 - A ballonist begins a trip in a helium-filled...Ch. 6 - Prob. 6.61PCh. 6 - Prob. 6.62PCh. 6 - Prob. 6.63PCh. 6 - Prob. 6.64PCh. 6 - Four 50.-g sample of different liquids are placed...Ch. 6 - When simple sugars, called monosaccharides, link...Ch. 6 - Reaction of gaseous CIF with F2 yields liquid...Ch. 6 - Prob. 6.68PCh. 6 - When organic matter decomposes under oxygen-free...Ch. 6 - The heat of atomization (Hatomo) is the heat...Ch. 6 - Prob. 6.71PCh. 6 - Prob. 6.72PCh. 6 - An aqueous wastes stream with a maximum...Ch. 6 - Kerosene, a common space-heater fuel, is a mixture...Ch. 6 - Prob. 6.75PCh. 6 - Phosphorus pentachloride is used in the industrial...Ch. 6 - Prob. 6.77PCh. 6 - Silicon tetrachloride is produced annually on the...Ch. 6 - Prob. 6.79PCh. 6 - You want to determine Ho for the reaction...Ch. 6 - Prob. 6.81PCh. 6 - Prob. 6.82PCh. 6 - Liquid methanol (CH3OH) can be used as an...Ch. 6 - How much heat is released when 25.0 g of methane...
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- n Section 10.7, two characteristics of enthalpy changes for reactions are listed. What are these characteristics? Explain why these characteristics are true.arrow_forward9.41 Under what conditions does the enthalpy change equal the heat of a process?arrow_forwardWhich of the enthalpies of combustion in Table 5.2 the table are also standard enthalpies of formation?arrow_forward
- Compounds with carboncarbon double bonds, such as ethylene, C2H4, add hydrogen in a reaction called hydrogenation. C2H4(g)+H2(g)C2H6(g) Calculate the enthalpy change for this reaction, using the following combustion data: C2H4(g)+3O2(g)2CO2(g)+2H2O(l);H=1411kJC2H6(g)+72O2(g)2CO2(g)+3H2O(l);H=1560kJH2(g)+12O2(g)H2O(l);H=286kJarrow_forwardWhen 2.50 g of methane burns in oxygen, 125 kJ of heat is produced. What is the enthalpy of combustion per mole of methane under these conditions?arrow_forwardDifferentiate between the enthalpy of formation of H2O(l)andH2O(g) . Why is it necessary to specify thephysical state of water in the following thermochemicalequation CH4(g)+2O2(g)CO2(g)+2H2O(lorg)H=?arrow_forward
- Draw a diagram like Figure 2.11 that illustrates the change in enthalpy for the chemical reaction C s 2H2 g CH4 g Which is exothermic by 74.8 kJ/mol.arrow_forwardA 0.470-g sample of magnesium reacts with 200 g dilute HCl in a coffee-cup calorimeter to form MgCl2(aq) and H2(g). The temperature increases by 10.9 C as the magnesium reacts. Assume that the mixture has the same specific heat as water and a mass of 200 g. (a) Calculate the enthalpy change for the reaction. Is the process exothermic or endothermic? (b) Write the chemical equation and evaluate H.arrow_forwardUse Hesss law to calculate the enthalpy change for the formation of CS2() from C(s) and S(s) [C(s) + 2 S(s) CS2()] from the following enthalpy values. C(s)+O2(g)CO2(g)rH1=393.5kJ/mol-rxnS(s)+O2(g)SO2(g)rH2=296.8kJ/mol-rxnCS2(l)+3O2(g)CO2(g)+2SO2(g)rH3=1103.9kJ/mol-rxnarrow_forward
- Explain why absolute enthalpies and energies cannot be measured, and only changes can be determined.arrow_forwardA compound is 82.7% carbon and 17.3% hydrogen, and has a molar mass of approximately 60 g/mol. When 1.000 g of this compound burns in excess oxygen, the enthalpy change is 49.53 kJ. (a) What is the empirical formula of this compound? (b) What is the molecular formula of this compound? (c) What is the standard enthalpy of formation of this compound? (d) Two compounds that have this molecular formula appear in Appendix G. Which one was used in this exercise?arrow_forwardIs the following reaction the appropriate one to use in determining the enthalpy of formation of methane, CH4(g)? Why or why not? C(g)+4H(g)CH4(g)arrow_forward
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