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Calculate the standard free energy change for a reaction at 298K where the Keq is 1.4 x 10-5
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- construct a balanced reaction for the formation of Fe2O3(s) from its elements in their standard states at 298 K. For a stoichiometric coefficients of 1,Calculate AG for the following reaction at 25 °C: rxn 4CO₂(g) + 2H₂O(1) → 2C₂H₂(g) + 5O₂ (g) Round your answer to 5 significant digits. Note: Reference the Thermodynamic properties of pure substances table for additional information. kJ mol ☐ x10 XUse the data provided in the table to calculate the change in Gibbs Free-Energy at 25 degrees Celsius for the reaction given. Ag+ (aq) Cl- (aq) AgCl (s) S0 (J K-1 mole-1) 72.68 56.4 96.2 Delta H Kj/mol 105.58 -167.2 -127.07 Group of answer choices -75.2 kJ +55.7 kJ +32.5 kJ -75.2 kJ -55.7 kJ
- Using enthalpies of formation, calculate AH° for the following reaction at 25°C. Also calculate AS" for this reaction from standard entropies at 25°C. Use these values to calculate AG for the reaction at this temperature. Species AH; (kJ/mol) S" (J/mol·K) COCL, (9) -220.1 283.9 H20(1) -285.8 69.95 CO2 (9) -393.5 213.7 HCI(9) -92.31 186.8 COCI, (9) + H20(1) + CO, (9) + 2HCI(9) ΔΗ' kJ AS J/K AG° = kJFor the reaction NH,NO3(aq) –→N½0(g) + 2 H2O(1) AG° = -181.7 kJ and AH° = -149.6 kJ at 321 K and 1 atm. This reaction is (reactant, product) favored under standard conditions at 321 K. The entropy change for the reaction of 2.38 moles of NH,NO3(aq) at this temperature would be J/K.What is the standard free-energy change for the following reaction: 2C6H6 (l) + 15O2 (g) 12CO2 (g) + 6H2O (l) at 25 0C? Values of delta Gf of substances at standard conditions are as follows: Benzene = 124.5 kJ/mol, Carbon dioxide = -394.4 kJ/mol, Oxygen gas = 0.0 kJ/mol, and Liquid water =A. -237.2 kJ/mol. B. -64.05 kJC. +640.5 kJD. -6405 kJE, None of the above
- For the reaction NH4NO3(aq) 1 N₂O(g) + 2 H₂0 (1) AG° -179.4 kJ and AH = -149.6 kJ at 298 K and 1 atm. This reaction is (reactant, product) favored under standard conditions at 298 K. The entropy change for the reaction of 1.51 moles of NH4NO3(aq) at this temperature would be J/K.Make a non-spontaneous process spontaneous A process that is nonspontaneous can be made spontaneous by coupling it with another process tha is highly spontaneous. The coupling of nonspontaneous reactions with highly spontaneous ones is important in biological system. The oxidization of glucose, for example, is highly spontaneous: C6H12O6(s) + 60₂(g) → 6 CO₂(g) + 6 H₂O(1) Spontaneous reactions such as this ultimately drive the nonspontaneous reactions necessary to sustain life. Can you use Gibbs free energy, enthalpy, and entropy to argue this reaction is highly spontaneous?Calculate the standard free-energy change AG® and the equilibrium constant K, for the following reaction at 25°C. CO(9) + 2H2 (9) CH; OH(9) AG¡ (kJ/mol) Substance CO(g) H2 (9) CHOН (9) -137.2 -162.0 AG" = kJ Ky
- P Please don't provide the handwriting solutionConsider the reaction scheme for degradation of water 1 atm: Reaction 1: H20 ↔ H2 + 1/2 O2 Reaction 2: H20 ↔ 1/2 H2 + OH Delta G1 = 228,566 kJ/kmol Delta G2 = 263.270 kJ/kmol Delta Hr,1° = 241,820 kJ/kmol Delta Hr,2° = 281,280 kJ/kmol A) Calculate the value of the equilibrium constant for each Reaction at 25°C. What does this tell you about the equilibrium composition B) Estimate the equilibrium constant for each reaction at 5,000°C. C) Fully set up and explain how you would solve for the equilibrium composition of reaction mixture which started with 1 mole of water. Include an expression for the equilibrium constant(s) in terms of composition as part of your answer.Use the References to access important values if needed for this question. For the reaction NH,Cl(aq)- NH3(g) + HCI(aq) AG° = 64.7 kJ and AH° =86.4 kJ at 274 K and 1 atm. This reaction is (reactant, product) favored under standard conditions at 274 K. The entropy change for the reaction of 2.44 moles of NH,Cl(aq) at this temperature would be J/K. Submit Answer Retry Entire Group 4 more group attempts remaining ed