What is the A,G for the following reaction (in kJ mol-¹) at 298 K? 2 NO2 (g) = N2O4 (g) The conditions for this reaction are: PNO2 = 1.67 bar PN204 = 1.45 bar You will also need to use Appendix II in your textbook (containing standard Gibbs energies of formation). A copy of Appendix II has also been posted on eClass Please use the method of Gibbs energy of formation to calculate ArG° if needed. For partial credit, enter the value of "Q" for this reaction. Answer:

What is the A,G for the following reaction (in kJ mol-¹) at 298 K? 2 NO2 (g) = N2O4 (g) The conditions for this reaction are: PNO2 = 1.67 bar PN204 = 1.45 bar You will also need to use Appendix II in your textbook (containing standard Gibbs energies of formation). A copy of Appendix II has also been posted on eClass Please use the method of Gibbs energy of formation to calculate ArG° if needed. For partial credit, enter the value of "Q" for this reaction. Answer:

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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ju sited Free Online Survey... Search Home - Academia... Submit Answer Retry Entire Group Modules [References] Use the References to access important values if needed for this question. Consider the following reaction where Kp = 0.160 at 298 K. 2NOBr(g) 2NO(g) + Br₂(g) If the three gases are mixed in a rigid container at 298 K so that the partial pressure of each gas is initially one atm, what will happen? Indicate True (T) or False (F) for each of the following: 1. A reaction will occur in which NOBr(g) is produced. 2. K, will increase. 3. A reaction will occur in which NO is produced. 4. Qp is greater than Kp. 5. The reaction is at equilibrium. No further reaction will occur. hp 8 Create Your Rubric -... 8 more group attempts remaining || K The Utility Experts ... E P insert » C 4x 12/ bac
7. FREE GIBBS ENERGY RELATING TO KP ⚫ Consider the decomposition of barium carbonate BaCO3(s) BaO (s)+CO (g) Use data in Appendix A to calculate the equilibrium pressure of CO at a) 298 K and b) 1100 K.
a) For a reaction with AH = -152.6 kJ mol-¹ and AS°= -543.8 J K-¹ mol-¹ at 25 °C, how will AGº change if the reaction temperature is increased? Explain your answer. b) Calculate the equilibrium constant for the reaction at 80 °C, showing your working (assume AH and AS° are temperature independent).
For reaction of A and B: A + B C , rHo = -20 kJ mol-1 and K = 50 at 25C. Calculate K at 100 C.
Estimate the temperature in K at which the reaction will become nonspontaneous.
18. Given the AG°S for the reactions, calculate Ks. Values given for 298 K AG° -560.3 kJ 2 H2(g) a. CH4(g)+2 F2(g) 4(g) 2 NO)Cl2(g) 2 SO3() AG° +40.8 kJ b. 2 NOC (g) AG° = -140.0 kJ c. 2 SO2(g) O2(g)
#3 Calculate the standard entropy, AS in, of the reaction at 25.0 C using the table of thermodynamic properties. C₂H₂(g) + H₂O(1)→ C₂H₂OH(1) ASixn = Calculate the standard Gibbs free energy of the reaction, AGixn. The standard enthalpy of the reaction, AHxn, is -44.2 kJ.mol-¹. AGixn= TOOLS x10 Determine in which direction the reaction is spontaneous as written at 25.0 °C and standard pressure. $ 4 % 5 Okay MacBook Pro & N You 8 ( BABAE 9 J-K-¹-mol-1 A kJ-mol-1 O delet-
Consider the following system at equilibrium where K. = 34.5 and AH° = -198 kJ/mol at 1150 K. 2 So, (g) + 02 (g) =2 S03 (g) The production of S03 (g) is favored by: Indicate True (T) or False (F) for each of the following: ]1. decreasing the temperature. v 2. increasing the pressure (by changing the volume). | 3. decreasing the volume. 4. removing SO3 . 5. removing O2 -
Use the data below to calculate the value of the equilibrium constant for the following reaction at 298 K. Please give your answer with 2 significant figures. 3 NO2(g) + H2O(e) → 2 HNO3(e) + NO(g) AfG [H2O(l)] = -237.2 kJ mol-1 ; AFG°[HNO3(e)] = -79.9 kJ mol-1 ; AfG [NO(g)] = 86.7 kJ mol-1; AfG°[NO2(g)] = 51.8kJ mol-1