Table 20.1 Standard reduction potentials at 25°C*Increasing strength as oxidizing agentHalf-ReactionLi*(aq) + eK+ (aq) + eBa²+ (aq) + 2eSr²+ (aq) + 2e-Ca²+ (aq) + 2eNa + (aq) + eMg²+ (aq) + 2eBe²+ (aq) + 2eAl³+ (aq) + 3eMn²+ (aq) + 2e2H₂O + 2e™Zn²+ (aq) + 2e-Cr³+ (aq) + 3eFe²+ (aq) + 2eCd²+ (aq) + 2ePbSO4(s) + 2eCo²+ (aq) + 2eNi²+ (aq) + 2e2+Sn²+ (aq) + 2ePb²+ (aq) + 2eLi(s)K(s)Ba(s)→ Sr(s)Ca(s)Na(s)Mg(s)Be(s)Al(s)→→ Mn(s)H₂(g) + 2OH(aq)Zn(s)Cr(s)Fe(s)Cd(s)Pb(s) +Co(s)Ni(s)Sn(s)Pb(s)H₂(g)Sn²+ (aq)+ SO² (aq)4+2H¹ (aq) + 2eSn¹+ (aq) + 2eCu²+ (aq) + e→ Cut (aq)SO (aq) + 4H+ (aq) + 2e SO₂(g) + 2H₂OAgCl(s) + e → Ag(s) + Cl(aq)Cu²+ (aq) + 2eCu(s)O₂(g) + 2H₂O + 4e¯¯ →[₂ (s) + 2e →→→→→→→ 21 (aq)MnO4 (aq) + 2H₂O + 3e -O₂(g) + 2H+ (aq) + 2e¯Fe²+ (aq)Fe³+ (aq) + eAg (aq) + eAg(s)Hg2+ (aq) + 2e2Hg²+ (aq) + 2e →NO3(aq) + 4H+ (aq) + 3e2Hg(1)40H (aq)H₂O₂(aq) + 2H+ (aq) + 2e¯Co³+ (aq) + eO3(g) + 2H+ (aq) + 2eF₂(g) + 2e →→→ 2F (aq)Hg2+ (aq)MnO₂ (s) + 4OH(aq)H,Oz(aq)Br₂(l) + 2e →→→ 2Br (aq)O₂(g) + 4H+ (aq) + 4e¯MnO₂ (s) + 4H+ (aq) + 2e →Cr₂O² (aq) + 14H+ (aq) + 6eCl₂(g) + 2e →Au³+ (aq) + 3e2C1 (aq)-Au(s)MnO4 (aq) + 8H+ (aq) + Se¯→→→→→Ce+ (aq) + eCe ³+ (aq)PbO₂ (s) + 4H+ (aq) + SO² (aq) + 2e¯2H₂OO₂(g) + H₂O(l)NO(g) + 2H₂OCo*(aq)2H₂OMn²+ (aq) + 2H₂O2Cr³+ (aq) + 7H₂O2+Mn²+ (aq) + 4H₂O-> PbSO4(s) + 2H₂O8° (V)-3.05.-2.93-2.90-2.89-2.87-2.71-2.37-1.85-1.66-1.18-0.83-0.76-0.74-0.44-0.40-0.31-0.28-0.25-0.14-0.130.00+0.13+0.15+0.20+0.22+0.34+0.40+0.53+0.59+0.68+0.77+0.80+0.85+0.92+0.96+1.07+1.23+1.23+1.33+1.36+1.50+1.51+1.61+1.70+1.77+1.82+2.07+2.87Increasing strength as reducing agent*For all half-reactions the concentration is 1 M for dissolved species and the pressure is 1 atm for gases.These are the standard-state values. 1. Calculate AG and predict whether the following reaction would proceed spontaneously aswritten at 298K:2+Mg(s) + Sn²+ (aq)Mg²+ (aq) + Sn(s)given that [Mg2+]=0.045 M, [Sn²+1=0.035M. (R:8.314J/mol.K, 96500 J/V.mol)

•Given cell reaction:- Mg(s) + Sn2+(aq) ==> Mg2+(aq) + Sn(s) •Transferred electron (n) = 2 =>…

1. Calculate AG and predict whether the following reaction would proceed spontaneously as written at 298K: 2+ Mg(s) + Sn²+ (aq) Mg²+ (aq) + Sn(s) given that [Mg2+]=0.045 M, [Sn²+]=0.035M. (R:8.314J/mol.K, 96500 J/V.mol)

1. Calculate AG and predict whether the following reaction would proceed spontaneously as written at 298K: 2+ Mg(s) + Sn²+ (aq) Mg²+ (aq) + Sn(s) given that [Mg2+]=0.045 M, [Sn²+]=0.035M. (R:8.314J/mol.K, 96500 J/V.mol)

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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Consider the following reaction: E 2NO₂(g) N₂O4(9) -> Type here to search Q W S E Bi C R Part B F Calculate AG at 298 K if the partial pressures of NO₂ and N₂O4 are 0.38 atm and 1.63 atm, respectively. Express the free energy in kilojoules to two decimal places. AG= -6 Submit VΞΑΣΦ h a xa xô x + √x √xxx Provide Feedback Previous Answers Request Answer T P B 1X1 H X Incorrect; Try Again; 3 attempts remaining This value of free energy is more negative than AG for the reaction (i.e., more spontaneous), but the partial pressu times greater than that of the reactant, so the free-energy change is expected to be more positive than AG (Le., les N Given that AG-AG + RTIn Q, calculate the value of Q (it should be greater than 1 for the specified conditions) energy from Part A to find the free-energy change at the given partial pressures. Make certain values are expressed in summing them LOWE O ? M X.10n F20 kJ 4 90°F Clear
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