A student determines the value of the equilibrium constant to be 4.09×10-18 for the following reaction. Fe;O4(s) + 4H2(g)→3FE(s) + 4H,O(g) Based on this value of Kegi AG° for this reaction is expected to be (greater, less) greater than zero. Calculate the free energy change for the reaction of 1.76 moles of Fe;0,(s) at standard conditions at 298K. AG°. rxn = 190.5 kJ

A student determines the value of the equilibrium constant to be 4.09×10-18 for the following reaction. Fe;O4(s) + 4H2(g)→3FE(s) + 4H,O(g) Based on this value of Kegi AG° for this reaction is expected to be (greater, less) greater than zero. Calculate the free energy change for the reaction of 1.76 moles of Fe;0,(s) at standard conditions at 298K. AG°. rxn = 190.5 kJ

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

For the reaction 4HCI(g) + O2(9)– →2H20(g) + 2Cl,(g) AH° = -114.4 kJ and AS° = -128.9 J/K The standard free energy change for the reaction of 1.84 moles of HCI(g) at 296 K, 1 atm would be kJ. This reaction is (reactant, product) favored under standard conditions at 296 K. Assume that AH° and AS° are independent of temperature.
48 Use data to compute ΔG° at 57.0°C for the following reaction. 2ClO2−(aq) + O2(g) → 2ClO3−(aq) ΔH°f (ClO2−(aq)) = -67 kJ mol-1ΔH°f (ClO3−(aq)) = -104 kJ mol-1ΔS° (ClO2−(aq)) = 101 J mol-1 K-1ΔS° (O2(g)) = 205.152 J mol-1 K-1ΔS° (ClO3−(aq)) = 162 J mol-1 K-1ΔG°f (ClO2−(aq)) = 17 kJ mol-1ΔG°f (ClO3−(aq)) = -3 kJ mol-1
For the reaction CHĄ(g) + H,O(g)–→3H2(g) + CO(g) AH° = 206.1 kJ and AS° = 214.7 J/K %3D The standard free energy change for the reaction of 1.55 moles of CH,(g) at 320 K, 1 atm would be kJ. This reaction is (reactant, product) favored under standard conditions at 320 K. Assume that AH° and ASº are independent of temperature.
A student determines the value of the equilibrium constant to be 8.14x10-37 for the following reaction. H,S(g) + 2H,0(1)–→3H,(g) + SO>(g) Based on this value of Keg AG° for this reaction is expected to be (greater, less) than zero. Calculate the free energy change for the reaction of 2.03 moles of H,S(g) at standard conditions at 298K. AG°rxn kJ Ixn
[2] In the figure below, the standard free energy change is plotted in function of the temperature for the reactions: 20(s) +0,(g) → 20o(g) en C(s) +0,(g) → CO,(g) AG (kJ) -380 -400 -420 -440 800 900 1000 1100 T(K) How is it possible, starting from this drawing, to calculate the standard free energy change for the reaction below at a certain temperature?: CO2(9) + C(s) > 2CO(g)
1. Which of the following processes are spontaneous: spreading of a bad odour through a room; separating a mixture of O2 and N2 into two separate samples, one that is pure H2 and one that is pure N2; the reaction of sodium metal with oxygen gas to form a metal oxide; (a) (b)
A reaction has a standard free-energy change of –13.20 kJ mol-(-3.155 kcal mol-). Calculate the equilibrium constant for the reaction at 25 °C. Keg
None
This reaction is _______ (product or reactant) favored under standard conditions at 330 K
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?
A student determines the value of the equilibrium constant to be 2.33×1016 for the following reaction.Ca(OH)2(aq) + 2HCl(aq) ----> CaCl2(s) + 2H2O(l)Based on this value of Keq:ΔG° for this reaction is expected to be (greater, less) ____ than zero.Calculate the free energy change for the reaction of 2.34 moles of Ca(OH)2(aq) at standard conditions at 298K.ΔG°rxn = _______ kJ
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 AICI 3(s) + 3 CO(g) 4.0 -64 a) ΔΗΟ kJ/mol b) AS° ✓ J/K.mol kJ/mol (Determine from the temperature, AH and AS) c) AGO 4.0 76.9 4.0 -89 (d) Is the reaction extensive at standard conditions and 298 K? O Yes O NO (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 XX (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 X (Please answer to 3 significant figures.)