Calculate K at 298 K for the following reaction given the Gibbs free energy of formations...
calculate the Gibbs free-energy change for the following reaction at 298 k if the partial pressure of each is 0.10 atm and the Gf of NO and NOBr are 86.55 KJ/mol and 82.4 KJ/mol respectively.
Consider the reaction 2 NO2(g) N2O4(g) . (a) Using ΔGf N2O4(g) = 97.79 kJ/mol and ΔGf NO2(g) = 51.3 kJ/mol, calculate ΔG° at 298 K. ______ kJ (b) Calculate ΔG at 298 K if the partial pressures of NO2 and N2O4 are 0.45 atm and 1.55 atm, respectively. _____ kJ
Consider the reaction 2 NO2(g) →N2O4(g) .(a) Using ΔGfN2O4(g) = 97.79 kJ/mol and ΔGf NO2(g) = 51.3 kJ/mol, calculate ΔG° at 298 K.kJ(b) Calculate ΔG at 298 K if the partial pressures of NO2 and N2O4 are 0.25 atm and 1.30 atm, respectively.kJ
correct answer? The change in Gibbs free energy, AGⓇ for the following reaction at 298 K is 70.6 kJ/mol. 2NO,(9) — 2NO(g) + O2(9) What is Keq for this reaction? O 4.30 O 0.971 2.00 1.03 O 0.936
A reaction is at equilibrium at 298 K. At 310 K, the Gibbs free energy for the reaction is –12.6 kJ/mol. Assuming that both entropy and enthalpy are independent of temperature, what are the values of the entropy and enthalpy for this reaction?
1. What is the AGº of the reaction below, given the standard Gibbs free energy of formations provided. CH,(g) + 20kg) 5C0g) + 2H,0g) Substance AG (kJ/mol) CH4(g) 50.8 CO2(g) 394.4 H2O(g) -228.57 a. -50.8 kJ/mol b. -751 kJ/mol c. +113 kJ/mol d. -115 kJ/mol e. -807 kJ/mol
Calculate the standard Gibbs energy change for the following generic reaction at 298 K, using the standard enthalpies of formation and standard entropies from the table below A+B-C AHI KJ SI JKT Substance mor1 mor1 148.0 299.0 0 76.2 -269.9 105.3 Select one: O a. 8.001e4 kJ/mol O b.-337.5 kJ/mol O C.-265.1 kJ/mol O d. 382.9 kJ/mol o e.-3.460e4 kJ/mol
For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all species. For the reaction 2NO(g)+O2(g)↽−−⇀2NO2(g) the standard change in Gibbs free energy is Δ?°=−72.6 kJ/mol . What is ΔG for this reaction at 298 K when the partial pressures are ?NO=0.500 atm , ?O2=0.400 atm , and ?NO2=0.750 atm ?
29 5 points The change in Gibbs free energy, AGº for the following reaction at 298 K is 70.6 kJ/mol. 2NO,(9) — 2NO(g) + O2(g) What is Keq for this reaction? O 0.936 O 4.30 0 0.971 02.00 01.03 Previous
Will this reaction take place? Thank you Thermodynamics Gibbs Free energy Calculate Gibbs free energy for reaction of urea hydrolysis CO(NH2)2(aq) + H2O(0) = CO2(g) + NH3(e) From standard enthalpy and entropy data: AH° = 119 kJ AS9 = 354.8 J/K = 0.3578 kJ/K T = 25°C = 298°K AG = AH° – TYAS°