2. Calculate AG from standard enthalpy of formation and standard molarentropy values and predict whether the following reactions is spontaneous ornot, at 25 °C.А.H21 + COzH2O+ COAH (kJ/mol)S° (J/mol.K)130.6H2CO2H2OCO-393.5-241.8-110.5213.6188.8197.9B. Fe Oa)3H22Fe + 3H2OAH (kJ/mol)S° (J/mol.K)Fe203l-822.290.0FelH2O130.627.2188.8-241.8

Given reactions: A. H2 (g) + CO2 (g) →H2O (g) + CO (g) B. Fe2O3 (s) + 3H2 (g) → 2Fe (s) + 3H2O (g)…

2. Calculate AG° from standard enthalpy of formation and standard molar entropy values and predict whether the following reactions is spontaneous or not, at 25 °C. А. Hao + COzi H2O + CO S° (J/mol.K) 130.6 213.6 188.8 197.9 AH (kJ/mol) CO2 H2O CO -393.5 -241.8 -110.5 B. Fe Oa + 3H2 2Fe + 3H2O AH (kJ/mol) S° (J/mol.K) Fe203) -822.2 90.0 Fel H2O 130.6 27.2 188.8 -241.8

2. Calculate AG° from standard enthalpy of formation and standard molar entropy values and predict whether the following reactions is spontaneous or not, at 25 °C. А. Hao + COzi H2O + CO S° (J/mol.K) 130.6 213.6 188.8 197.9 AH (kJ/mol) CO2 H2O CO -393.5 -241.8 -110.5 B. Fe Oa + 3H2 2Fe + 3H2O AH (kJ/mol) S° (J/mol.K) Fe203) -822.2 90.0 Fel H2O 130.6 27.2 188.8 -241.8

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

The value of G° for the conversion of ATP to ADP is -35.6 kJ/mol.The reaction is: ATP(aq) → ADP(aq)Calculate K at 25°C. K =b. Consider the metabolism of glucose C6H12O6(s) + 6 O2(g) 6 CO2(g) + 6 H2O(l) Determine the standard free energy for the metabolism reaction. c. If 100% of the free energy from the metabolism of glucose is used for the conversion of ADP to ATP, how manymolecules of ATP can be produced from each gram of glucose (mm = 180.16)?
Activity 5: Spontaneity and Gibbs' Free Energy Directions: Calculate AG°, AH°, AS° then predict whether the reaction is spontaneous. Consider the following reaction: N2(g) + 3H2(g) → 2NH3(g) 1. AH = - 92.4 kJ/mol (a) The absolute entropy values, S, at 238 K for N2(g), H2(g) and NH3(g) are 192 J/Kmol, 131 J/Kmol and 193 J/Kmol respectively. Calculate AS° for the reaction and explain the sign of AS°. Calculate AG° for the reaction at 238 K. State and explain whether the reaction (b) is spontaneous.
Use thermodynamic values in the table provided to calculate the ΔG for the following process in two ways. 4NH3 (g) + 5O2 (g) → 4NO (g) + 6H2O (g) at 25˚C a) Use Free Energy values to calculate ΔG. b) Use Enthalpy and Entropy values with Gibbs Equation to calculate ΔG. c) What do your final ΔG values tell us about this reaction?
Consider the following reaction, the equilibrium constant for this reaction at 298 K is 0.113: 2NO2(g) ⇌ N2O4(g) A) You have a system with 5.00 atm of NO2 and 7.00 atm of N2O4 is this reaction at equilibrium? Calculate Q tosupport your answer.B) Which way will the reaction proceed to reach equilibrium? C) Using the value of K, calculate the value for ΔG°.
13)The reaction 2NOBr(g) → 2NO(g) + Br₂(g) has AG° = 6.28 kJ. a. Calculate Q when [NOBr] = 0.15 M, [NO] = 0.096 M, and [Br₂] = 0.081 M. b. Calculate AG for the reaction at 150°C. c. Is this reaction spontaneous or non-spontaneous under these conditions? Scanned with CamScanner
Fill the table with their respective standard entropy of reaction and show the solutions.
In a biochemical reaction, A + B ® C with DG= 30 kJ/mol. Which of the following reactions, if any, might be effectively coupled to this reaction so that it becomes more spontaneous? I. C + D -> B + E Delta G = –40 kJ/mol II. C + D -> B + E Delta G = +40 kJ/mol
Plz do Asap...!
What is the free energy change for the following reaction at 25 oC if the entropy change at this temperature is - 10 J/molK? 3 A (g) + B (s) ------ 2 C (g) + 3.40 kJ A. - 3.30 kJ/mol B. + 6.38 kJ/mol C. + 0.420 kJ/mol D. - 6.38 kJ/mol E. - 0.420 kJ/mol
Table 2. Gibbs Free Energies of formation (kJ), ∆G°f, for Ions in 1M Solution and Ionic Solids Cations Cl--131.228 I--51.57 NO3--108.74 SO4-2-744.53 Ag+77.107 AgCl -109.789 -66.19 -33.41 -618.41 Calculated values of ∆G°rxn and the ∆Grxn of each box, Predicted results (ppt or no ppt).Observations (Rxn or No Rxn). S or support and R for Refute Cations Cl- I- NO3- SO4-2 Ag+ Ba+2
2. Consider the reaction below. 4NH3(g) + 5O₂ (g) 4NO (g) + 6H₂O (g) a. Using the provided AGf values, calculate AG° for the above reaction at 25 °C. Species AG (kJ/mol) NH3) NO(g) H₂O -16.5 87.6 -228.6 b. Is the reaction spontaneous at 25 °C? c. What is the sign of the change in entropy for the reaction?
11. Calculate the ASsys, ASsurr, and AS,univ of the process below at 25°C and determine whether it is spontaneous, at equilibrium, or nonspontaneous. Removal of Ozone in the Stratosphere 2 03 (g) -> 3 02 (g) Оз (д) 02 (g) Substance Entropy 238.9 J/mol-K 205.2 J/ mol-K Enthalpy 142.7 kJ/mol