What is K for a reaction if AGº =-226.1 kJ/mol at 25 °C (or 298 K)? (R = 8.314 J/mol · K)

A chemical engineer is studying the two reactions shown in the table below. In each case, she fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 142.0 °C and constant total pressure. Then, she measures the reaction enthalpy AH and reaction entropy AS of the first reaction, and the reaction enthalpy AH and reaction free energy AG of the second reaction. The results of her measurements are shown in the table. Complete the table. That is, calculate AG for the first reaction and AS for the second. (Round your answer to zero decimal places.) Then, decide whether, under the conditions the engineer has set up, the reaction is spontaneous, the reverse reaction is spontaneous, or neither forward nor reverse reaction is spontaneous because the system is at equilibrium. 2NO(g) → N₂(g) + O₂(g) AH = -181. kJ AS = -436. AG = | KJ J K Which is spontaneous? this reaction the reverse reaction neither X Ś

19. Ammonia can be formed by the reaction of hydrogen with nitrogen gas 3H2 (g) + N2 (g) → 2NH3 (g). The value of AH° is –92.38 kJ/mol, and that of AS° is -198.2 J/mol·K. Determine AG° at 25°C. (A) -59.0 kJ/mol (B) 151 kJ/mol (C) -33.3 kJ/mol (D) -151 kJ/mol

Calculate the Kp.

What is AG for a reaction where AG° = -4.5 kJ/mol and Q = 2.8 at 295 K? (R = 8.314 J/mol K) 2.36 1 4 8 +/- 2.

Q4. (a) What is Eell for the following unbalanced reaction? Fe (s) + O2 (g) + 2H20 (4) Fe3 (aq) + 40H (aq) (b) Balance the reaction. (c) What is A,G° for the reaction? (d) What are the conditions of the above process?

Calculate the AH°, AS°, and AG° at 298 K for the following reaction: (Use the values found in Thermodynamic Properties to calculate your answers for questions a and b.) Al2O3(s) + 3 C(graphite) + 3 Cl₂(g) → 2 AICI3(s) + 3 CO(g) a) ΔΗο 400-64 kJ/mol b) AS° J/K.mol c) AGO 4.0 ✔ kJ/mol (Determine from the temperature, AH and AS) (d) Is the reaction extensive at standard conditions and 298 K? O Yes O NO 4.0 76.9 -89 (e) Write the expression for K. (Format example: Kp = pHC1² / pH₂. pCl2 would be entered as K_{p} = pHCI^{2}/pH_{2} . pCl_{2}.) Help chemPad X₁X (PCO)³ (pCl₂)3 Greek (PCO)^3/(pCl_2)^3 Your answer provides a different type of equation than was expected. (f) Calculate the value of K at 298 K 2.51e-16 X (Please answer to 3 significant figures.) (g) Estimate the value of K at 600 K. 1 79e-8 Ty (Please answer to 3 significant figures)

Given the following equation, H2O(g) + CO(g) → H2(g) + CO2(g) ΔG°rxn = -28.6 kJ Calculate ΔG°rxn for the following reaction. 8 H2O(g) + 8 CO(g) → 8 H2(g) + 8 CO2(g) Group of answer choices +3.57 kJ -228.8 kJ -3.57 kJ +228.8 kJ -71.5 kJ

Enter your answer in the provided box. 0 Find AG for the following reaction, at 25°C, using AH and Sº values. NH4Cl(s) NH3(g) + HCI(g) kJ Substance or Ion HCl(g) HCl(aq) NH3(g) NH3(aq) NH4Cl(s) A Standard Thermodynamic Values at 298 K AH (kJ/mol) -92.3 -167.46 -45.9 -80.83 -314.4 < Prev 0 S (J/mol K) 186.79 55.06 193 110 94.6 11 of 25 Next GL

# H₂O(1) H*(aq) + OH(aq) Calculate the pOH of a 0.0100 M HCl solution at 50.0 °C. AH = -55.8 kJ; K=1.0 x 10-¹4 (at 25.0 °C)