Given:E0 -0.49VFe (ag) t 2e teu)fe *"E -0.04V(aq) +3e tela)E +0 77 VFe " (aqlte Fe "(aq).Cl2(g) + 2e 7 201 (aq).34E': +1-36 VCal oulate the AE° for the reaction2tFe(s) t Claca) - te "(aq) t 2ci Caq).

We have asked to find out the ∆E° for the following reaction Fe(s) + Cl2 (g) → Fe(aq)2+ +…

Answered: Given: Fe * (a) t 2e teu). E0:-0.49V fe…

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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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?
Give hand written answer
Incorrect ASuniv ASin = Calculate AGian AGin Incorrect ASS O forward O both O reverse surr Incorrect AS sys 11 Consider the reaction described by the chemical equation shown. 3C₂H₂(g) →CH (1) AH = -633.1 kJ Use the data from the table of thermodynamic properties to calculate the value of ASi at 25.0 °C. 384.92 In which direction is the reaction, as written, spontaneous at 25 °C and standard pressure? Macmillan Learning Calculate the following quantities. Refer to the standard entropy values as needed. 2 C(graphite) + O₂(g) → 2 CO(g) Consider the following reaction at 298 K. AH = -221.0 kJ
What volume of oxygen gas at STP must be consumed to produce the corrosion of 200 g of iron? Hint. Fe- Fe2+ +2e (one mole of Fe produces 2 moles of electrons) 4OH-O2+2H2O+4e (1/2mole O2 = 1 mole Fe) V=nRT/p =(8.314J/mol)
Calculate [OH] for a HNO;(aq) solution at 25°C where [H'] = 4.3 x 10 M. Show all work and units.
Calculate ΔG. For the following process at 25°C: BaF2 (s) = Ba2 + (aq) + 2F - (aq) The Ksp of BaF2 is 1.7 x 10^-6 ΔG° = _____ kJ/mol
From data given below, calculate AH°, AS“, and AG° for the following reaction at 25°C. + NH3 (9) + NHẠCI(s) HCI(9) AH; -92 kJ/mol AG -95 kJ/mol -46 -314 -17 -203 187 J/K-mol 193 96 kJ AS° J/K AG° : kJ
R = 8.314 mol·K F = 96,485 mol AG° + RT · In(Q) AE° () · In(Q) AG ΔΕ %3D Half Reaction (Note: All given as reduction) E° (V) 02 (g) + 4 H*(aq) + 4 e → 2 H20 (I0) 1.229 Z2 (s) + 2 e - → 2Z (aq) 0.426 (aq) + 3 e A (s) 0.292 2 H20 (1) + 2 e G2+ (aq) + 2 e M2+ (aq) + 2 e Н2 (в) + 2 ОН" (aq) - 0.828 G (s) - 1.245 M (s) - 1.893 Using a U-tube, a student sets up a non-spontaneous electrochemical cell with a battery connected to two carbon electrodes that are submerged in 1 M MZ2 (aq) solution (M is a metal and Z is an anion composed of the newly discovered element Z). Use the reference information given in the table above to answer the following three questions. Question 10 Oxidation will occur at the while reduction will occur at the Possible answers are "anode" and "cathode".
just a&b
4
Be sure to answer all parts. Calculate the emf for the following reaction. Will the reaction occur spontaneously at 25°C, given that [Fe ]-0.400 M and [Ca2*]-0.00790 M? Cd(s) + Fe*(ag) Ca2*(ag) + Fe(s) Caca -0.40 V E rere --0,44 V E- The reaction as written is O spontaneous O not spontaneous
R = 8.314 mol-K F = 96,485 mol AG = AG° + RT · In(Q) ΔΕ - (E) · In(Q) ΔΕ. Half Reaction (Note: All given as reduction) E° (V) 02 (g) + 4 H*(aq) + 4 e 2 H20 (1) 1.229 Z2 (s) + 2 e 3+ (aq) + 3 e 2z (aq) 0.426 A (s) 0.292 2 H20 (1) + 2 e G2+ (aq) + 2 e M²+ (aq) + 2 e¯ H2 (g) + 2 OH¯ (aq) - 0.828 G (s) - 1.245 M (s) - 1.893 A student constructs a voltaic electrochemical cell with two metal electrodes [metal G and metal A] in their respective aqueous nitrate solutions [G(NO3)2 and A(NO3)3]. Use this information, as well as the reduction potentials in the table above to complete each statement below. Consider the same cell from the above prompt. Calculate A E°. cell for this galvanic cell given the reference information given at the top of the quiz. Report your answer with 3 decimal places. You do not need to report units with your answer.

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Given: Fe * (a) t 2e teu). E0:-0.49V fe * E 0.04. (aq) +3e te la). Fe "( aqlte 7 Fe "(aq). Cl2(g) + 2e 7 201" (aq). Eo +0 77 V 31 E : +1-36 V Caloulate the AE° for the reaction 2t Fe(s) + Clacg) - te "(aq) t 2C1 (aq)