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O H20 - 2.5 QUESTION 11 Use the standard half-cell potentials listed below to calculate the...
Part A Use the standard hall-cell potentials listed below to calculate the standard cell potential for the following consumo Mg(s) + Cu2+ (aq) Cu(s) + Mg(4) Mg2 (na) + 20 Mg(s) E--238 V Cuzaq) +20 - Cu(s) E' = 40.34 V O2.72 V 204 V -1.36 V 204 V O 1.36 V Submit
Part A Use the standard hall-cell potentials listed below to calculate the standard cell potential for the following consumo Mg(s) + Cu2+ (aq) Cu(s) + Mg(4) Mg2 (na) + 20 Mg(s) E--238 V Cuzaq) +20 - Cu(s) E' = 40.34 V O2.72 V 204 V -1.36 V 204 V O 1.36 V Submit
Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical 3 C12(a) + 2 Fe(s) - 6 Cr(aq) + 2 Fe3+ (aq) Cl2(g) + 2 + 2 Cl(aq) Fe3+ (aq) + 36 - Fe(s) E' = +1.36 V E' = -0.04 V +1.40 V O-1.40 V 0 +4.16 V O +1.32 V O-1.32 V Submit Resvest Answer
24) Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25°C. (The equation is balanced.) 26). 3 Cl2(8) +2 Fe(s) - 6 Cl(aq) + 2 Fe3+ (aq) 12(8)+2 e 2Cl(aq) E° 1.36 V 3C1tbe ! Fe3+(aq) + 3 e → Fe(s) 80036V 2Fe > 25€ Ep 3 + the A) 240 V B) 4.16V ) -1.32 V D) -1.40 V E) 1.32 V
Use the standard half-cell potentials listed below to determine which the following metals will dissolve in hydrochloric acid. Cl2(g) + 2e + 2C1-(aq); E° = 1.36 V 2H+(aq) + 2e + H2(g); E° = 0.00 V O Cu; E°(Cu2+/Cu) = +0.34V O Au; E°(Au3+/Au) = +1.50V O Al; E°(A13+/Al) = -1.66V O Ag; E°(Ag+/Ag) = +0.80V O Pt; E°(Pt2+/Pt) = +1.19V
Use the standard half-cell potentials listed below to determine which the following metals will dissolve in hydrochloric acid. Cl2(g) + 2e -- 2014(aq); E° = 1.36 V 2H+(aq) + 2e - H2(g); E° = 0.00 V OPt; E°(P+2+/Pt) = +1.19V O Ag; E°(Ag+/Ag) = +0.80V O Au; EⓇ(Au3+/Au) = +1.50V O Al; E(A13+/Al) = -1.66V O Cu; E(Cu2+/Cu) = +0.34V
Question 56 (1 point) Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25°C. (The equation is balanced.) 3 Cl2(g) + 2 Fe(s) → 6 (aq) + 2 Fe3+(aq) E° = +1.36 V Cl2(g) + 2 e 2 Cl(aq) Fe3+(aq) + 3 e → Fe(s) E° = -0.04 V O-1.32 V +4.16 V +1.40 V -1.40 V +1.32 V Question 55 (1 point) Calculate AGrxn at...
Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25�C. (The equation is balanced.) Sn(s) + 2 Ag+(aq) ? Sn2+(aq) + 2 Ag(s) Sn2+(aq) + 2 e- ? Sn(s) E� = -0.14 V Ag+(aq) + e- ? Ag(s) E� = +0.80 V a)-1.08 V b)+1.74 V c)-1.74 V d)+0.94 V e)+1.08 V
Use the standard half-cell potentials listed below to calculate the standard free energy(K]for the following reaction occurring in an electrochemical cell at 25°C. Pb 2+ (aq) +2e--- Pb(s) E* - -0.13 Volt A13+ (aq) + 3 e-Al(s) E* =-1.66 volt a. 1.53 b. - 886 c-434 d. - 443 e. -1036 What is the standard free energy Gº) in Kilojoules for the reaction below at 298 Kelvin: Farady's constant = 96,485 joules/V. mole e Zn2+ (aq) + 2e ......> Zn(s)...
What would be the standard cell potential for a spontaneous electrochemical cell constructed with the two metals below? Cu2+(aq) + 2e– → Cu(s) E° = 0.34 V Sn4+(aq) + 2e– → Sn2+(aq) E° = 0.13 V