Given the following data: 2Fe(s) + 3/2 O2(g) --> Fe2O3(s) AG°= -742.2 kJ/mol CO(g) + 1/2 O2(g) --> CO2(g) AG°= -257.2 kJ/mol Determine AG° for the reaction Fe2O3(s) + 3CO(g) --> 3CO2(g) + 2Fe(s) Question 23: Report the free energy change of reaction (delta G) in kJ to one decimal place delta G = KJ Check Reuse <> Embed H-P

Given the following data: 2Fe(s) + 3/2 O2(g) --> Fe2O3(s) AG°= -742.2 kJ/mol CO(g) + 1/2 O2(g) --> CO2(g) AG°= -257.2 kJ/mol Determine AG° for the reaction Fe2O3(s) + 3CO(g) --> 3CO2(g) + 2Fe(s) Question 23: Report the free energy change of reaction (delta G) in kJ to one decimal place delta G = KJ Check Reuse <> Embed H-P

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter5: Thermochemistry

Section: Chapter Questions

Problem 5.46QE

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Similar questions

The thermite reaction was once used to weld rails: 2Al(s)+Fe2O3(s)Al2O3(s)+2Fe(s)(a) Using heat of formation data, calculate H for this reaction. (b) Take the specific heats of Al2O3 and Fe to be 0.77 and 0.45 J/g C, respectively. Calculate the temperature to which the products of this reaction will be raised, starting at room temperature, by the heat given off in the reaction. (c) Will the reaction produce molten iron (mpFe=1535C,Hfus=270J/g)?
Given the following standard free energies at 25°C for the following reactions: N2O5(g)2NO(g)+32O2(g)G=59.2kJNO(g)+12O2(g)NO2(g)G=35.6kJ Calculate G° at 25°C for the following reaction: 2NO2(g)+12O2(g)N2O5(g)
Consider the reaction Fe2O3(s)+3H2(g)2Fe(s)+3H2O(g) a. Use Gf values in Appendix 4 to calculate G for this reaction. b. Is this reaction spontaneous under standard conditions at 298 K? c. The value of H for this reaction is 100. kJ. At what temperatures is this reaction spontaneous at standard conditions? Assume that H and S do not depend on temperature.
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.
The amount of manganese in steel is determined by changing it to permanganate ion. The steel is first dissolved in nitric acid, producing Mn2+ ions. These ions are then oxidized to the deeply colored MnO4 ions by periodate ion (IO4) in acid solution. a. Complete and balance an equation describing each of the above reactions. b. Calculate and G at 25C for each reaction.
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?
Actually, the carbon in CO2(g) is thermodynamically unstable with respect to the carbon in calcium carbonate(limestone). Verify this by determining the standardGibbs free energy change for the reaction of lime,CaO(s), with CO2(g) to make CaCO3(s).
Under standard conditions, what reaction occurs, if any, when each of the following operations is performed? a. Crystals of I2 are added to a solution of NaCl. b. Cl2 gas is bubbled into a solution of NaI. c. A silver wire is placed in a solution of CuCl2 d. An acidic solution of FeSO4 is exposed to air. For the reactions that occur, write a balanced equation and calculate ,G, and K at 25C.
Use the standard free energy of formation data in Appendix G to determine the free energy change for each of the following reactions, which are run under standard state conditions and 25 C. Identify each as either spontaneous or nonspontaneous at these conditions. (a) MnO2(s)Mn(s)+O2(g) (b) H2(g)+Br2(l)2HBr(g) (c) Cu(s)+S(g)CuS(s) (d) 2LiOH(s)+CO2(g)Li2CO3(s)+H2O(g) (e) CH4(g)+O2(g)C(s,graphite)+2H2O(g) (f) CS2(g)+3Cl2(g)CCl4(g)+S2Cl2(g)
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?
9.56 Using heats of formation tabulated in Appendix E, calculate the heats of reaction for the following. (a) C2H2(g)+52O2(g)2CO2(g)+H2O(l) (b) PCl3(g)+Cl2(g)PCl5(g) (c) C2H4(g)+H2O(g)C2H5OH(g) (d) Fe2O3(s)+2Al(s)Al2O3(s)+2Fe(l)
2. For the reaction 2 CO(g) + O2(g) → 2 CO2(g). ∆rH° = −566 kJ/mol-rxn. What is the enthalpy change for the oxidation of 42.0 g of CO(g)? −283 kJ −425 kJ −566 kJ −393.5 kJ