6.72 Many portable gas heaters and grills use propane, CHg(g), as fuel. Using standard enthalpies of formation, calculate the quantity of heat produced when 10.0 g of propane is com- pletely combusted in air under standard conditions. 6.73/Using values from Appendix C, calculate the standard en- 6.8 ae thalpy change for each of the following reactions: (a) 2 SO2(8) + O2(8) → 2 SO3(g) (b) Mg(OH)2(s) – (c) N2O4(8) + 4 H2(8) (d) SiCl4(1) + 2 H20(1) → SiO2(s) + 4 HC1(8) MgO(s) + H2O(1) Bor N2(8) + 4 H20((g) 6 6.74 Using values from Appendix C, calculate the value of AH° for each of the following reactions: (a) CaO(s) + 2 HC1(g) CaCl2(s) + H2O(8) → 2 Fe2O3(s) (b) 4 FeO(s) + O2(8) (c) 2 CuO(s) + NO(g) Cu20(s) + NO2(g) g) + 2 H20(1)

6.72 Many portable gas heaters and grills use propane, CHg(g), as fuel. Using standard enthalpies of formation, calculate the quantity of heat produced when 10.0 g of propane is com- pletely combusted in air under standard conditions. 6.73/Using values from Appendix C, calculate the standard en- 6.8 ae thalpy change for each of the following reactions: (a) 2 SO2(8) + O2(8) → 2 SO3(g) (b) Mg(OH)2(s) – (c) N2O4(8) + 4 H2(8) (d) SiCl4(1) + 2 H20(1) → SiO2(s) + 4 HC1(8) MgO(s) + H2O(1) Bor N2(8) + 4 H20((g) 6 6.74 Using values from Appendix C, calculate the value of AH° for each of the following reactions: (a) CaO(s) + 2 HC1(g) CaCl2(s) + H2O(8) → 2 Fe2O3(s) (b) 4 FeO(s) + O2(8) (c) 2 CuO(s) + NO(g) Cu20(s) + NO2(g) g) + 2 H20(1)

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Incorrect. What is the heat of formation of elements in their standard states? Did you use the correct equation of products minus reactants? The amino acid glycine, C2H5NO2, is one of the compounds used by the body to make proteins. The equation for its combustion is 4C2H5NO2(s) + 902(g) → 8CO2(g) +10H20(1) +2N2(g) For each mole of glycine that burns, 973.49 kJ of heat is liberated. Use this information, plus values of AHº for the products of combustion, to calculate AH° for glycine. AH = kJ/mol eTextbook and Media Hint Solution 935 pm A 27°C Haze O G 10 ENG Type here to search 15/03/2022 1080 acer Insert Delete F11 F12 Prt Sc Pause Br F8 F9 F10 F7 NumLk F5 F3 Esc Coca) Backsp * 8 8 # 2$ % & 9 @ € 7 1 2 3 !!
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5(a)
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