Given the following half-reactions:3-AIF6 +3e Al + 6F E° = -2.07 VAl+ + 3e - AlE° = –1.66 VCalculate the equilibrium constant at 25°C for the reaction3-Al+ (ag) + 6F (ag) = AIF, (aq)(Enter your answer to two significant figures.)K =|Submit AnswerTry Another Version10 item attempts remaining

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Given the following half-reactions: 3- AIF6 +3e → Al + 6F E° = –2.07 V %3D Al+ + 3e Al E° = –1.66 V Calculate the equilibrium constant at 25°C for the reaction Al+ (aq) + 6F (ag) = AIF6 (ag) 3- (Enter your answer to two significant figures.) %3D Submit Answer Try Another Version 10 item attempts remaining

Given the following half-reactions: 3- AIF6 +3e → Al + 6F E° = –2.07 V %3D Al+ + 3e Al E° = –1.66 V Calculate the equilibrium constant at 25°C for the reaction Al+ (aq) + 6F (ag) = AIF6 (ag) 3- (Enter your answer to two significant figures.) %3D Submit Answer Try Another Version 10 item attempts remaining

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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Given the following half-reactions: AIF6 + 3e- Al + 6F A13+ + 3e Al E = -2.07 V %3D E = -1.66 V %3D Calculate the equilibrium constant at 25°C for the reaction 3- A1$+ (aq) + 6F(aq) AIF6 (aq) (Enter your answer to two significant figures.) K
The following skeletal oxidation-reduction reaction occurs under basic conditions. Write the balanced OXIDATION half reaction. F + Br₂-F₂ + Br Br₂+2e Reactants Search ] % 5 Submit Answer T 2Br Products G H Retry Entire Group & 4- 7 U J + Enter electrons as e 7 more group attempts remaining 8 KAA ( K 9 ►|| O L P { + = insert } prt sc 1 7:57 1 12/3/20 ← backspace
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Perform the following calculations for the unbalanced reaction S40 (aq) + 21 (aq) →→ 1₂(s) + S₂0₂² (aq) (a) Identify the oxidizing and reducing agents. Oxidizing agent: O S40,² (aq) I (aq) 1₂(s) $₂0,² (aq) 0 (b) Calculate the E -0.45 and calculate E 2- 0 E +2e S in S40: 2.5 S in $₂0,²": Oxidation numbers: 0:-2✔ half-cell cell (c) For the reduction half-reaction, write a balanced equation, give the oxidation number of each element, 0 half-cell --0.45 2- -25₂03 Reducing agent: ⒸS40,² (aq) O I (aq) 1₂(s) S₂03² (aq) AG-87.8 kJ/mol 0 E anode =0.53 V
MISSED THIS? Read Section 20.5 (Pages 913 - 917) ; Watch KCV 20.5. Calculate AG°n and Ecell at 25° C for a redox reaction with n = 4 that has an equilibrium constant of K = 4.8x10-2. Part A Express your answer using two significant figures. AG° rxn = kJ Submit Request Answer Part B Express your answer using two significant figures. να ΑΣφ E cell = Submit Request Answer Provide Feedback
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