6-gibbsA student determines the value of the equilibrium constant to be 4.01×10-18 for the following reaction.Fe;04(s) + 4H,(g)-→3FE(s) + 4H20(g)Based on this value of KegiAG° for this reaction is expected to be (greater, less)than zero.Calculate the free energy change for the reaction of 2.03 moles of Fe,04(s) at standard conditions at 298K.AG°,kJ||rxntables are linked

Answered: Image /qna-images/answer/cd4e73fd-8c57-4ab7-8024-3ab8aea68463.jpg

6-gibbs A student determines the value of the equilibrium constant to be 4.01×10-18 for the following reaction. ezO4(s) + 4H2(g)- →3F€(s) + 4H2O(g) Based on this value of Keqi 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 Fe;O4(s) at standard conditions at 298K. AG°. kJ rxn tables are linked

6-gibbs A student determines the value of the equilibrium constant to be 4.01×10-18 for the following reaction. ezO4(s) + 4H2(g)- →3F€(s) + 4H2O(g) Based on this value of Keqi 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 Fe;O4(s) at standard conditions at 298K. AG°. kJ rxn tables are linked

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...

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For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all species. For the reaction 2 NO(g) + 0,(g) =2 NO,(g) the standard change in Gibbs free energy is AG° = -32.8 kJ/mol. What is AG for this reaction at 298 K when the partial pressures are PNO = 0.500 atm, Po, = 0.350 atm, and PNO, = 0.800 atm?
For a certain chemical reaction, the equilibrium constant K = 4.5 × 10 - 10 at 5.00 °C. Calculate the standard Gibbs free energy of reaction. %3D Round your answer to 2 significant digits. AG° = | kJ |x10
For a certain chemical reaction, the equilibrium constant K = 1.9 × 10¯¯ at 5.00 °C. Calculate the standard Gibbs free energy of reaction. -4 Round your answer to 2 significant digits. AG° = | KJ x10 ? X Ś
[References] Calculate the standard free-energy change AG" and the equilibrium constant K, for the following reaction at 25°C. CO(g) + 2H2 (g) CH3 OH(g) Substance AG; (kJ/mol) CO(g) -137.2 H2 (g) 0. CH3OH(g) -162.0 AG kJ K, = | d.
Using reaction free energy to predict equilibrium composition Consider the following equilibrium: 2NOCI (g) = 2NO (g) + Cl2 (g) AGº =41. kJ Now suppose a reaction vessel is filled with 7.85 atm of nitrosyl chloride (NOCI) and 5.15 atm of chlorine (C12) at 834. °C. Answer the following questions about this system: rise Under these conditions, will the pressure of C₁₂ tend to rise or fall? ☐ x10 fall Is it possible to reverse this tendency by adding NO? In other words, if you said the pressure of C12 will tend to rise, can that be changed to a tendency to fall by adding NO? Similarly, if you said the pressure of C₁₂ will tend to fall, can that be changed to a tendency to rise by adding NO? If you said the tendency can be reversed in the second question, calculate the minimum pressure of NO needed to reverse it. Round your answer to 2 significant digits. yes no atm ☑ 00. 18 Ar
4
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7. The equilibrium constant for the reac- tion N,(g) + Oz(g) 2 2NO(g) at 2130°C is 2.5 X 10-3. Why is it un- necessary to be told whether the value is for K, or K.? The reaction absorbs heat. For the following conditions, determine whether the reaction is spontaneous for- ward or in reverse, or whether it is at equilibrium: a) A 1-liter box contains 0.02 mole of NO, 0.01 mole of O,, and 0.02 mole of N, at 2130°C. b) A 20-liter box contains 0.01 mole of N,, 0.001 mole of O,, and 0.02 mole of NO at 2130°C. c) A 1-liter box contains 1.00 mole of N2, 16 moles of O,, and 0.2 mole of NO at 2500°C.
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