Calculate the standard free energy change for the combustion of one mole of methane using the values for standard free energies of formation of the products and reactants. The sign of the standard free energy change allows chemists to predict if the reaction is spontaneous or not under standard conditions and whether it is product-favored or reactant-favored at equilibrium.
kJ/ mol-rxn
The equation for the reaction is: 2 CH4 + 3 O2 2 CO2 + 2 H2O
The standard gibbs free enrgy change = Sum of gibbs energy change of products - Sum of gibbs energy change of reactants = (2 * -623.1 + 2 * 228.61) - (2 * -74.850 = -1553.72 KJ/mol
Calculate the standard free energy change for the combustion of one mole of methane using the...
21A. Calculate the standard free energy change, AGºat 298 K for the reaction 2COXg) + 2NO(g) -2CO(g) + N:(g) The standard free energy of formation for CO is - 137 kJ, for NO it is 87.6 kJ/mol and for CO, it is -394 kJ/mol. B. Calculate the free energy change. AG. at 298 K. given that the partial pressure of CO is 5.0 atm, that of NO is 4.0 atm, that of CO, is 3.0 atm & that of N,...
Calculate the approximate enthalpy change, ?Hrxn, for the combustion of one mole of methane a shown in the balanced chemical equation: CH4+2O2?2H2O+CO2 Use the values you calculated in Parts A, B, C, and D, keeping in mind the stoichiometric coefficients. delta H CH4=1656 kJ/mol delta H O2=498 kJ/mol delta H H2O=-928 kJ/mol delta H CO2=-1598 kJ/mol
PLEASE EXPLAIN WHY EACH ANSWER IS TRUE OR FALSE 6. The standard free energy AG° of the reaction A +B C following statements true or false. D is +3 kJ/mol. Mark the The standard free energy of the reaction can be calculated from the free energies of formation of A, B, C, and D from the elements. The reaction is endothermic under standard state conditions. One way to get the reaction to proceed to the right is to increase the...
15. The standard Gibbs free energy change (AG%) for the Haber reaction at 298K is -2.83 kJ/mol N2(g) + 3H2(g) + 2NH3(g) If the reaction begins with 2.55 atm N2(g) 0.115 atm Hz(g) and 0.488 atm NH3(9) at 298K what is the free energy change (AG) for the reaction under these conditions AND will the reaction be spontaneous under these conditions? (10 points) 16. For the following reactions, predict whether they will tend to be spontaneous at either high or...
The standard enthalpy change for the combustion of 1 mole of propane is -2043.0 kJ. CzH3(g) + 5 O2(g) + 3 CO2(g) + 4H2O(g) Calculate 4, Hº for propane based on the following standard molar enthalpies of formation. molecule CO2(g) H2O(g) 4,Hº (kJ/mol-rxn) -393.5 -241.8
kJ/mole) The standard enthalpy of combustion of solid urea (NH2 (C-O) (C=O)NH2 ) is -632 kJ/mole under standard conditions. Its standard molar entropy is 104.60 J/K mol. Calculate the Gibbs energy of formation of urea at 298K.(ANS: -663 kJ/mol) 4.
Item 29 29 of 32 Review Constants Periodic Table Calculate the change in Gibbs free energy for each of the sets of AN A S , and T given in the following problems Predict whether or not the reaction in part A wil be spontaneous at the femperature indicated. (Assume that all reactants and products are in their standard states) spontaneous nonspontaneous Submit Part F Predict whether or not the reaction in part B will and products are in their...
Calculate the equilibrium constant K and the standard free energy change ΔrG˚ at room temperature for the following reaction, HF(aq) H+(aq) + F- (aq) At equilibrium, you measured the following concentrations of reactants and products: [HF]eq = 0.092 M, [H+] eq = 0.008M, [F- ] eq = 0.008 M Think about it: According to your calculation of ΔrG˚, is this reaction reactant favored or product favored? Do you come to the same conclusion when you look at the equilibrium...
4. (a) Calculate the Gibbs Free Energy of formation for urea at 25°C. Given: The standard enthalpy of formation is -333.17 kJ mol and the standard entropy of formation is 136.093 J K mol". (b) is the formation of urea a spontaneous process under these conditions? Explain. (7 pts) J mol
Calculate standard free energy change using AG values. Consider the reaction 2CO2(g) + 3H2(g) C2H2() + 4H2O(g) Use standard free energies of formation to calculate the standard free energy change for this reaction at 25°C. AG9rxn = kJ/mol