4) (a) Use the standard entropy values (AS") in the Appendix to solve for ?5° of...
5) N2(g) + O2(g) 2 NO(g) ΔΗ' 180.7 kJ ; AS°-24.7 J/K 25°C (a)Calculate the standard free-energy change for the reaction at 25 C. (b) Calculate AG at 500 C using the value calculated from part a. 6) (Hess' Law) AG +1102 kJ/mole What is the change in free energy when 18 moles of chlorine gas are rea to make phosphorus trichloride cted with phosphorus
question 17.57
entropy change for H2(g) + CuO(s) → H2O(0) + Cu(s) 17.56 Use the data in Appendix G to calculate the standard entropy change for 2Al(s) + Fe2O3(s) → Al2O3(s) + 2Fe(s) OBJECTIVE Define Gibbs free energy and relate the sign of a Gibbs free-energy change to the direction of spontane- ous reaction. 17.57 Calculate AGº for the following reactions and state whether each reaction is spontaneous under standard con- ditions at 298 K. (a) Fe2O3(s) + 2Al(s) →...
Use the standard molar entropies in Appendix B to calculate the standard entropy of reaction for the oxidation of graphite to carbon monooxide: 2C(s)+O2(g)→2CO(g)
Please help with #4&5. Will rate high is answers are
correct. Thank you!
4. Using the given standard molar entropies, calculate the standard entropy change, AS, for the following reaction at 298 K: 2 H2(g) + O2(g) → 2 H20(1) O2(g) 205.0 (H2O(1) 79.91 H2(g) Sº (J/K) 130.58 a) 326.3J/K b) 88.5 J/K c) 306.34 J/K d) -306.34 J/K e) -386.25 J/K 5. Calculate the standard free-energy change for the formation of NO(g) from N2(g) and O2(g) at 298 K:...
17. Using values for the standard enthalpies of formation (AH:9) and standard molar entropy (439) on the Appendix, calculate the following thermodynamic values for the complete combustion of ethanol: (10 points) C2H5OH(g) + 302(g) → 2CO2(g) + 3H2O(g) a) The standard enthalpy change (AHº) b) The standard entropy change (AS) c) Use values from a) and b) above to calculate AGO at 298K d) Is this reaction spontaneous at 298K under standard conditions?
1. Calculate AH° and AG', using data in Appendix C. Determine whether each reaction is endothermic or exothermic, and spontaneous or nonspontaneous. a) 2PbO(s) + N2(g) → 2Pb(s) + 2NO(g) b) CS2(1) + 2H20(1) - CO2(g) + 2H,S(9)
Absolute Entropy Sº, in moll K1 3. Use the following table and rxn to answer the questions. Standard Heat of Substance Formation, AH, in kJ moli C(s) 0.00 CO2(g) -393.5 H2(g) H2O(1) -285.85 O2(g) 0.00 C3H2COOH(1) 0.00 5.69 213.6 130.6 69.96 205.0 226.3 The enthalpy change for the combustion of butyric acid at 25°C, AH"comb, is-2,183.5 kilojoules per mole. C3H7COOH(1) + 5O2(g) = 4CO2(g) + 4H20(1) a) From the data above, calculate the standard heat of formation, AH,, for butyric...
Consider the reaction 2H2(g)+ O2(g)>2H20(g) Using standard thermodynamic data at 298K, calculate the entropy change for the surroundings when 1.77 moles of H2(g) react at standard conditions J/K surroundings
Consider the reaction 2H2(g)+ O2(g)>2H20(g) Using standard thermodynamic data at 298K, calculate the entropy change for the surroundings when 1.77 moles of H2(g) react at standard conditions J/K surroundings
Calculate standard free energy change using AHA and S values. Consider the reaction 2HS(g) + 302(g) >2H20(1) + 2502(9) Calculate the standard free energy change for this reaction at 25°C from AHºrn and Serx A Gºrx = kJ/mol
2. (11.1) Use values of AH and AG in Appendix H to evaluate the standard molar reaction enthalpy and the thermodynamic equilibrium constant at 298.15K for the oxidation of nitrogen to form aqueous nitric acid: 3N2(g) + O2(g) + įH2O(l) → H+ (aq) + NO3- (aq)