Question 6: Given the following data: 2Fe(s) + 3/2 O2(g) --> Fe2O3(s) AH°=-822.2 kJ/mol CO(g) + 1/2 O2(g) --> CO2(g) AH°= -383.3 kJ/mol Determine AH° for the reaction Fe2O3(s) + 3CO(g) --> 3CO2(g) + 2Fe(s) Report the heat of reaction (delta H) in kJ to one decimal place delta H = KJ Check Reuse <> Embed H-P

Question 6: Given the following data: 2Fe(s) + 3/2 O2(g) --> Fe2O3(s) AH°=-822.2 kJ/mol CO(g) + 1/2 O2(g) --> CO2(g) AH°= -383.3 kJ/mol Determine AH° for the reaction Fe2O3(s) + 3CO(g) --> 3CO2(g) + 2Fe(s) Report the heat of reaction (delta H) in kJ to one decimal place delta H = KJ Check Reuse <> Embed H-P

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter17: Electrochemistry And Its Applications

Section: Chapter Questions

Problem 36QRT: Hydrazine, N2H4, can be used as the reducing agent in a fuel cell. N2H4(aq) + O2(aq) N2(g) + 2 H2O...

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Using values of fH and S, calculate rG for each of the following reactions at 25 C. (a) 2 Pb(s) + O2(g) 2 PbO(s) (b) NH3(g) + HNO3(aq) NH4NO3(aq) Which of these reactions is (are) predicted to be product-favored at equilibrium? Are the reactions enthalpy- or entropy-driven?
Hydrazine, N2H4, can be used as the reducing agent in a fuel cell. N2H4(aq) + O2(aq) N2(g) + 2 H2O () (a) If rG for the reaction is 598 kJ, calculate the valueof E expected for the reaction. (b) Suppose the equation is written with all coefficients doubled. Determine rG and E for this new reaction.
Using values of fH and S, calculate rG for each of the following reactions at 25 C. (a) 2 Na(s) + 2 H2O() 2 NaOH(aq) + H2(g) (b) 6 C(graphite) + 3 H2(g) C6H6() Which of these reactions is (are) predicted to be product-favored at equilibrium? Are the reactions enthalpy- or entropy-driven?
2C(s, graphite) + 3H2(g) → C2H6(g) AHrxn =? Given: (1) C(s, graphite) + 02 (8) → CO2(8) AH1 = -393. 5 kJ (2) H2 (8) + O2 (8) → H;O(1) AH2 = – -285. 8 kJ (3) 2C,H6 (8) + 702 (8) → 4CO2 (8) + 6H20(1) AH3 = -3119. 6 kJ
[4] rxn 2. Given the following information, calculate AH for the reaction. 2C3Hs(g) +1002(g) → 6CO2(g) + 8H₂O(1) | AH¦ (C³H8(g)) = -103.9 kJ/mol; AH; (CO2(g)) = -393.5 kJ/mol, AH; (H₂O(1) = -285.5 kJ/mol
Calculate AH for the process: N2(g) + 202(g) → 2NO2(g) from the following information: N28) +O2(g) → 2NO(g) AH = 180.5 kJ NO(g) + 02(8) → NO2(g) AH = -57.06 kJ
Please answer both
Calculate the enthalpy change for the reaction2 H2O2(l)---->2 H2O(l) + O2(g)using enthalpies of formation:ΔHf°[H2O2(l)] = -187.8 kJ/mol ΔHf°[H2O(l)] = -285.8 kJ/mol (a) -88.0 kJ(b) -196.0 kJ(c) +88.0 kJ(d) +196.0 kJ(e) more information needed
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Calculate the quantity of heat released when 5.00 g of H2O2(1) decomposes at constant pressure. 2 H2O2(1) --> 2 H2O(1) + 02(g) AH = -196 kJ -144 kJ O -14.4 kJ O -1.41 kJ
3
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