Practice: Calculate AG˚ for the followingreaction. Is it spontaneous?• 2Na + 2H2O H2 + 2OH + 2Na+AG°AG°=-nFE cellAG° = -RT In K21500/) | 2e(aq) +2>₂()+2011 (aq)0.83Mn(s)-1.18A+ (aq) +3eAls)1.66Me (aq) + 2e<-Ma(s)-2.37Na (aq) + e-Na(s)-2.71KExcellExcell0.0592 Vlog KCopyright © 2008 Pearson Prentice Hall Inc-

Step 1:An electrochemical cell is an apparatus in which the standard cell potential, Eocell > 0…

Answered: Practice: Calculate AG˚ for the…

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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need it with detailed explanation don't copy from other sources I will downvote
Chemistry emergency.
Considering the reaction and the information in the Excel table below, what should be entered into cell D3 to calculate Kc? Fe3+(aq) + 2 SCN (aq) = Fe(SCN),"(aq) (bp).2( A 1 Equilibrium Concentration (M) B 2 Fe3+ SCN Fe(SCN)2+ Equilibrium Constant 3 9.70E-04 1.70E-04 2.60E-05 =C3/(A3*B3^2) O =C3/(A3^2*B3) O =A3*B3^2/C3 O =C3/(A3*B3)^2 O =C3/(A3*B3)
(A) -0.23 V (C) -1.23 V (B) -0.85 V (D) -1.69 V 41. What is observed if a piece of lead is placed in an aqueous solution of Cu(NO3)2? Half-Reaction Pb²+ (aq) + 2e → Pb(s) Cu²+ (aq) + 2e → Cu(s) Eº, V -0.13 +0.34 I. The mass of the metal piece increases. II. The blue color of the solution becomes less intense. (A) I only (B) II only (C) Both I and II (D) Neither I nor II 42. If water is electrolyzed for 2.0 hr with a current of 10.0
Please answer fast I'll rate you sure
7>) True or False
just a&b
Im using this formula: E = Ecell - 0.0257/n (ln) (Q)
+ Cell Potential and Equilibrium The equilibrium constant, K, for a redox reaction is related to the standard potential, E, by the equation In K FE RT where 72 is the number of moles of electrons transferred, F (the Faraday constant) is equal to 96,500 C/(mol e-). R (the gas constant) is equal to 8.314 J/(mol K), and T is the Kelvin temperature. Standard reduction potentials ▾ Part A Use the table Express your answer numerically. ▸ View Available Hint(s) K= ΥΠΙ ΑΣΦ 9 Reduction half-reaction Ag+ (aq) +eAg(s) Cu²+ (aq) +201 >Cu(s) Sn+ (aq) + 4e →→Sn(s) 2H+ (aq) +2e →H₂(g) Ni2+ (aq) + 2e →Ni(s) Fe²+ (aq) + 2e →Fe(s) Zn²+ (aq) +2e →Zn(s) Al³+ (aq) + 3e →Al(s) Mg²+ (aq) + 2e →Mg(s) standard reduction potentials given above to calculate the equilibrium constant at standard temperature (25 °C) for the following reaction: Fe(s) + Ni²+ (aq) →>Fe²+ (aq) + Ni(s) ? E (V) 0.80 0.34 0.15 0 0.26 -0.45 0.76 -1.66 2.37 29 o Review | Constants | Period
▾ Part A For the reaction 2Co³+ (aq) + 2Cl(aq)-2Co2+ (aq) + Cl₂(g). E = 0.483 V what is the cell potential at 25°C if the concentrations are [Co³+] = 0.495 M. [Co²+] = 0.295 M, and [CI] = 0.272 M, and the pressure of Cl₂ is Pc, = 8.50 atm ? Express your answer with the appropriate units. View Available Hint(s) E= Submit 0 HA Value Units GAEC LIST onstans Periodic Table ?
Half-Reaction E° (V) 2H* (aq) + 2e¯ - H2 (9) 0.000 Ag* (aq) + e¯ → Ag (s) 0.7996 2H20 (I) + 2e¯ - H2 (g) + 20OH" (aq) -0.8277 AI3+ (aq) + 3e¯ → Al (s) -1.676 H2O2 (aq) + 2H* (aq) + 2e¯ → 2H20 (1I) 1.776 Au+ (aq) + e¯→ Au (s) 1.692 I2 (s) + 2e¯ → 21¯ (aq) 0.5355 Au3+ (aq) + 3e¯ → Au (s) 1.498 2103- (aq) + 12H* (aq) + 10e¯ → I2 (s) + 6H2O (1) Mg2+ (aq) + 2e - Mg (s) 1.195 Ba2+ (aq) + 2e¯ → Ba (s) -2.912 -2.372 Br2 (1) + 2e¯ → 2B1¯ (aq) 1.066 Mn2+ (aq) + 2e" → Mn (s) -1.185 Ca2+ (aq) + 2e¯ → Ca (s) -2.868 Mno2 (s) + 4H+ (aq) + 2e¯ → Mn2+ (aq) + 2H20 (1) 1.224 Cl2 (g) + 2e¯ → 2C1- (aq) 1.35827 Mno4- (aq) + 8H* (aq) + 5e¯ → Mn2+ (aq) + 4H2O (1) 1.507 Co2+ (aq) + 2e¯ → Co (s) -0.28 Mnog- (aq) + 2H20 (I) + 3e¯ → MnO2 (s) + 40H¯ (aq) 0.595 Co3+ (aq) + e¯ → Co2+ (aq) 1.92 HNO2 (aq) + H+ (aq) + e¯ → NO (g) + H2O (I) 0.983 Cr2+ (aq) + 2e¯ → Cr (s) -0.913 N2 (g) + 4H2O (1) + 4e¯ → 40H" (aq) + N2H4 (aq) -1.16 Cr3+ (aq) + 3e¯ → Cr (s) -0.744 NO3- (aq) + 4H* (aq) + 3e¯ → NO (g) + 2H2O (1) 0.957 Cr3+…
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