The equilibrium constant (Kp) for the balanced reaction Alg) + Bg) <--> C(g) + D(g) is Kp = 4.61 at 2000.0 K and the value for the standard free energy of this reaction is-31.5 kJ/mol also at 2000.0K. What is the value of the non-standard free energy (in units of kJ/mol) for the reaction at the same temperature if the partial pressures of the mixture are: PA= 0.260 atm; Pg = 0.790 atm; Pc=0.660 atm; and PD = 1.20 atm

The equilibrium constant (Kp) for the balanced reaction Alg) + Bg) <--> C(g) + D(g) is Kp = 4.61 at 2000.0 K and the value for the standard free energy of this reaction is-31.5 kJ/mol also at 2000.0K. What is the value of the non-standard free energy (in units of kJ/mol) for the reaction at the same temperature if the partial pressures of the mixture are: PA= 0.260 atm; Pg = 0.790 atm; Pc=0.660 atm; and PD = 1.20 atm

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Consider the reaction A(g) + B(g) → 2C(g). For this reaction, ΔHo = -116 kJ mol-1 and the equilibrium constant Kp is 140 at 600 K. Calculate for this reaction (i) ΔGo and (ii) ΔSo at 600 K.
Given the following and that R= 8.314 J/K mol, determine the equilibrium constant, K, at 298K for the following reaction: AgI(s)→ Ag (aq) + (aq) Substance (aq) Ag (aq) AgI(s) AG (kJ/mol) at 298 K 51.59 77.12 -66.2
Given equilibrium constant K = 0.051, please calculate the A,G° in unit of kJ for the following reaction at 489 °C, 2 HI(g) --> H2(g) + 12(g) (R = 8.314 J/K-mol). Please keep your answer to two decimal places.
4
Determine the equilibrium vapor pressure of germanium metal at 326.0 °C. The standard enthalpy of vaporization of germanium is 376.6 kJ/mol and the vapor pressure at 100.0 °C is 1.6E-32 Pa.
Calculate the standard change in Gibbs free energy for the reaction at 25 °C. Standard Gibbs free energy of formation values can be found in this table. 3 NO₂(g) + H₂O(1) – 2 HNO3 (1)+NO(g) -52.83 kJ/mol AGTxn Incorrect
A2(g) + 3B2(g) -> 2AB3(g) where the ΔGorxn is -140 kJ and equilibrium constant at standard conditions is 3.5x1024. a) If we place 0.100 atm of AB3, 0.050 atm of B2, and 0.500 atm of A2 in a container at 25oC, which direction will the reaction go (if any) to reach equilibrium?
A reaction has a standard free energy change of -15.0 kJ mol-¹. What is the equilibrium constant of the reaction at 25 °C?
The thermodynamic values from part A will be useful as you work through part B: ΔH∘rxn 243.5kJ/mol ΔS∘rxn 172.0J/(mol⋅K) Calculate the equilibrium constant for the following reaction at room temperature, 25 ∘C BaCO3(s)→BaO(s)+CO2(g)
Consider the reaction: H2( g) + I2( g)Δ2 HI( g)The following data show the equilibrium constant for this reaction measured at several different temperatures. Use the data to find ΔH°rxn and ΔS°rxn for the reaction.Temperature Kp150 K 1.4 * 10- 6175 K 4.6 * 10- 4200 K 3.6 * 10- 2225 K 1.1250 K 15.5
9. The K, value of the reaction N₂04 2NO, is 0.113. What is the Gibbs free energy, AG, of the reaction if the initial pressure of N₂O4 is 1.23 atm while NO₂ is 0.750 atm? Is the process spontaneous? 10. The molar heat of vaporization of ammonia is 23.4 kJ/mol while its boiling point is -33.34 °C. Calculate the AS for the vaporization of 0.75 moles of ammonia. Express your answer with unit J/K.