5. From the following heats of combustion,3CH,OH +-0,Oxe) →COe) + 2H,Ou2(g)2ΔΗ2(g)=-726.4kJrxnCigraphite) + O2c8)→ CO,ДН3-393.5kJ2(g)rxn1H2) +,O22) →H,OuΔΗ22(g)=-285.8kJrxnCalculate the enthalpy of formation of methanol, CH3OH, from its elements:1Cgraphite) + H2) +,O22) → CH,OH2

If we reverse any reaction sign will change of ∆H but magnitude remain same We multipy may equation…

5. From the following heats of combustion, 3 CH,OH + Oe → COue) +2H,Ou 2(8) AH° =-726.4kJ (1) 2(g) 2 rxn Cigraphite) + O2(8) →CO«g) AH° =-393.5kJ rxn 1 +÷0, +Oe) → H,Ou 2 H218) ΔΗ. =-285.8kJ rxn Calculate the enthalpy of formation of methanol, CH3OH, from its elements: Cgraphie) + H3) +÷2%e) →CH,OHa (graphite)

5. From the following heats of combustion, 3 CH,OH + Oe → COue) +2H,Ou 2(8) AH° =-726.4kJ (1) 2(g) 2 rxn Cigraphite) + O2(8) →CO«g) AH° =-393.5kJ rxn 1 +÷0, +Oe) → H,Ou 2 H218) ΔΗ. =-285.8kJ rxn Calculate the enthalpy of formation of methanol, CH3OH, from its elements: Cgraphie) + H3) +÷2%e) →CH,OHa (graphite)

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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3. Given the following equations and AH values, determine the heat of reaction at 298 K for the reaction C(s) + 2 H₂(g) → CH₁(B) C(s) + O₂(g) → CO₂(g) ΔΗ = -393.5 kJ H₂(g) + 1/2O₂(g) → H₂O(l) ΔΗ = -285.8 kJ ΔΗ = +890.3 kJ CO,(g) + 2 H,O(l) > CH%(g) + 2 Oz(g)
6. From the following heats of combustion, CH,OH + Oz) → CO2le) + 2H,0, AH°rxn = -726.4 kJ/mol C (graphite) + O2(g) → CO2 (g) H, (g) + Ozie) → H,O) AH°rxn = - 393.5 kJ/mol AH°rxn = -285.8 kJ/mol calculate the enthalpy of formation of methanol (CH;OH) from its elements: C(graphite) + 2H21) + O2l9) → CH;OH,
к Calculate AG rxn For the following reaction at 550k CH₂O(g) + 2H₂ → CH 4 (q) +H₂O (9) (9) Using AH° = - 94.9 KJ; AS³ = -224,2 J/K
Calculate the AH°rxn for the combustion of methane using the given AH°r. CH4 (g) + 202 (g) 2H20 (1) + CO2{g) AH°t, methane(g) = -74.60 kJ/mol AH°f, water(l) = -285.8 kJ/mol AH°t, carbon dioxide(g) = -393.5 kJ/mol 890.5 kJ/mol -890.5 kJ/mol -1.04 x 103 kJ/mol
2NO2(g) → N₂O4(g) 2NO(g) + O2(g) → 2NO2(g) Calculate the AH in kJ of 2NO(g) + O2(g) → N₂O4(g) AH₁ = -57.2kJ AH₂ -114.1kJ =
(e) Calculate the enthalpy change associated with this reaction. 2C(s) + H2(g) ---> C2H2(g) AH° = ??? kJ Given the following thermochemical equations: C2H2(g) + ½O2(g) ---> 2CO2(g) + H2O({) AH° = -1299.5 kJ C(s) + O2(g) ---> CO2(g) AH° = -393.5 kJ H2(g) + ½O2(g) ---> H2O(€) AH° = -285.8 kJ
Using the following equations, N,0(g)– 2NO2(g) AH° = +57.93 kJ 2NO(g) + O(g) 2NO,(g) AH° = -113.14 kJ %3D calculate the AH° for the following reaction: 2NO(g) + O2(g)– N,0,(g) AH° = kJ
The heat (enthalpy) of combustion of methanol is ΔHc = - 726kJ at T = 298K, at 1atm. (R = 8.31J/Kmol) CH3OH(l) + 3/2 O2(g) → CO2(g) + 2H2O(l) Find q, w and ΔU. a. q = - 726 000 J ; w = +1 238 J ; ΔU = - 727 338 J b. q = + 726 000 J ; w = -1 238 J ; ΔU = + 724 762 J c. q = + 726 000 J ; w = - 1 238 J ; ΔU = + 727 338 J d. q = - 726 000 J ; w = +1 238 J ; ΔU = - 724 762 J
V2
The standard enthalpies of combustion of formaldehyde, H2C=0(g), and formic acid, HCOOH(1), are -563 and -270 kJ/mol respectively. What is AH° for the following reaction? H2C=0(g) + ½ 02 --> HCOOH(1) O 563 kJ/mol O 833 kJ/mol O 293 kJ/mol O -833 kJ/mol
Calculate AHrxn for the reaction below. 2 NOCI(g) → N2(g) + 02(g) + Cl2(9) You are given the following set of reactions. 1/2 N2(g) + 1/2 02(g) → NO(g) AH = 90.30 k) NO(g) + 1/2 Cl2(g) → NOCI(g) AH = -38.6 kJ 4.0 kJ
Given the following information, AH° (A2B(g)) = -225 KJ/mol AH (BC(g)) = -160 KJ/mol %3D AH (AC(g)) = -85 KJ/mol AH (B(g)) = -75 KJ/mol Determine AH° for the reaction, A2B(g) + 2BC(g) 2AC(g) + 3B(g) -600 KJ/mol 150 KJ/mol 600 KJ/mol 450 KJ/mol