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

Answered: Image /qna-images/answer/f598ccc0-7c56-455c-bbde-659bb38b5014.jpg

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...

See similar textbooks

Similar questions

Help 2
5-7
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
Determine E°cell for the reaction below. 3 D2 (l) + 2 Z (s) → 2 Z3+(aq) + 6 D–(aq) Z3+(aq) + 3 e– → Z (s) E° = –0.04 V D2 (l) + 2 e– → 2 D– (aq) E° = +1.36 V Group of answer choices -1.40 V +1.32 V -1.32 V +4.16 V +1.40 V
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
TUTOR Voltaic Cells Under Non-Standard Conditions Calculate the potential developed by a voltaic cell using the following reaction if all dissolved species are 0.033 M at 25 °C. 2 Fe2"(aq) + H2O2(aq) + 2 H"(aq) → 2 Fe"(aq) + 2 H,O(E) Acidic Solution Standard Electrode Potential, E°(volts) H2O2(aq) + 2 H'(aq) + 2 e →2 H2O(E) Au*(aq) + e – Au(s) Au3 (aq) + 3 e →Au(s) +1.77 +1.68 +1.50 Br2(t) + 2 e -→2 Br(aq) +1.08 NO3 (aq) + 4 H'(aq) + 3 e → NO(g) + 2 H20 +0.96 Ag*(aq) + e –Ag(s) Hgz2"(aq) + 2 e →2 Hg(8) Fe (aq) + e--→ Fe²"(aq) Cu2"(aq) + 2 e → Cu(s) +0.80 +0.789 +0.77 +0.337 HgzClz(s) + 2 e →2 Hg(t) + 2 C(aq) Sn**(aq) + 2e → Sn2*(aq) +0.27 +0.15 2 H*(aq) + 2 e →H2(g) Pb?*(aq) + 2 e → Pb(s) 0.00 -0.126 Sn2*(aq) + 2 e → Sn(s) Ni2"(aq) + 2 e → Ni(s) Cd2*(aq) + 2 e → Cd(s) Cr**(aq) + e – Cr**(aq) Fe2"(aq) + 2 e → Fe(s) Zn2"(aq) + 2 e → Zn(s) Cr2*( aq) + 2 e → Cr(s) A* (aq) + 3 e Mg2*(aq) + 2 e → Mg(s) -0.14 -0.25 -0.40 -0.408 -0.44 -0.763 -0.91 Al(s) -1.66 -2.37
Can you also show me how to answer this please?
image 6-b
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
None
VISUALIZATION Batteries Zn(s) + 2 OH"(aq) → Zno(s) + H20(e) + 2e Hg0(s) + H,0(8) + 2e→ Hg(e) + 20H"(aq)* Consider the animation describing opperation of the mercury battery. What is the formula of the oxidizing agent used in the battery? Check Next (1 of 6)