a. Calculate Ecell and AG° (in kJ) and determine if the reaction is spontaneous. b. Calculate the equilibrium constant, K, at 298 K for the reaction using AG° = -RT In K. 4 Ag(s) + O2(g) + 4 H*(aq) → 4 Ag*(aq) + 2 H,O(1) O2(g) + 4 H*(aq) + 4 e +1.23 2 H2O(1) - +1.06 Br2(1) + 2 e 2 Br (aq) NO, (aq) + 4 H*(aq) + 3 e¯ Ag*(aq) + e - → NO(g) + 2 H,O(I) +0.96 +0.80 Ag(s) Do the signs/values of AG° and K make sense for this reaction given the cell potential?

a. Calculate Ecell and AG° (in kJ) and determine if the reaction is spontaneous. b. Calculate the equilibrium constant, K, at 298 K for the reaction using AG° = -RT In K. 4 Ag(s) + O2(g) + 4 H(aq) → 4 Ag(aq) + 2 H,O(1) O2(g) + 4 H(aq) + 4 e +1.23 2 H2O(1) - +1.06 Br2(1) + 2 e 2 Br (aq) NO, (aq) + 4 H(aq) + 3 e¯ Ag*(aq) + e - → NO(g) + 2 H,O(I) +0.96 +0.80 Ag(s) Do the signs/values of AG° and K make sense for this reaction given the cell potential?

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

What is the lowest temperature at which the reaction is spontaneous under standard conditions? H2O (g) + C (s) -> H2 (g) + CO (g)
G.59.
9. What do you about the spontaneity of the following reactions? Remember that AG = AH-TAS. The first one is solved as an example a. If Ah for a reaction is negative and As is positive? if AH 0 then AG < 0 and the reaction is spontaneous. b. What if Ah is negative and As is negative? c. What if Ah is positive and As is negative? d. What if Ah is positive and As is positive?
365 Calculate the standard free energy change for the following reaction: = Drive 2XO(s)+O2(g)→ 2XO2(s) AG 298(XO2) = -219.1 AG 298 (XO) = -150 Use 4 significant figures in your answer. Do not include the unit.
Please help with # 39. I do not know how to solve
@ た曲8 [Review Topics] [References] Use the References to access important values if needed for this question. Consider the following reaction at 298 K. Cr³+ (aq) + Fe2+ (aq) → Cr²+ (aq) + Fe³+ (aq) Which of the following statements are correct? Choose all that apply. On =1 mol electrons OK>1 U The reaction is reactant-favored. OAG° <0 cell
Calculate AG for the following reaction at 25 °C: rxn 4CO₂(g) + 2H₂O(1) → 2C₂H₂(g) + 5O₂ (g) Round your answer to 5 significant digits. Note: Reference the Thermodynamic properties of pure substances table for additional information. kJ mol ☐ x10 X
3. If 20 g of KNO3 is dissolved in 50 mL of water at 4 °C, is the system in equilibrium? If not, what spontaneous process will occur? What is the value of AG (NOT AG) for the system, as prepared, before any reaction occurs? KNO3, K², NO₂ (44) NO3(aq) AH R
Calculate standard free energy change using AGf values. Consider the reaction 2NH3(g) + 3N₂O(g)4N₂(g) + 3H₂O(g) Use standard free energies of formation to calculate the standard free energy change for this reaction at 25°C. kJ/mol AG° = rxn
14
Under the conditions shown below for the following reaction. Fe2O3(s) + 3 CO(g) → 2 Fe(s) + 3 CO2(g) AG° = -28.0 kJ P(CO) = 4.2 atm, P(CO2) = 1.8 atm Calculate AGrxn at 298 K, and indicate if the reaction is more or less spontaneous under these conditions than under standard conditions?
I need the answer as soon as possible