Use the References to access important values if needed for this question. Use the standard reduction potentials given below to predict if a reaction will occur when Co metal is put into a 1 M aqueous Fe²+ solution. Co2+ (aq) + 2e Fe2+ (aq) + 2e → Fe(s) Ee = -0.440 V red →Co(s) Ee -0.280 V red If a reaction will occur, write a balanced net ionic equation for the reaction. If no reaction w Occur, leave all boxes blank. + = (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) Submit Answer Try Another Version + 1 item attempt remaining

Rank the following in increasing ability as oxidizing agents. The reduction potentials of all species are shown below. Cl, (g) + 2e → 2C1 (aq) E° = 1.3583 V Ag*(aq) + le Cu²+ (aq) + 2e¯ → Ag(s) E° = 0.7996 V → Cu(s) E° = 0.342 V Sn²+ (aq) + 2e → Sn(s) E° = - 0.136 V к"(ад) + 1е — → K(s) E° - 2.95 V 1st attempt

Just the last one. And use table if needed

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Use standard reduction potentials to calculate the standard free energy change in kJ for the reaction: Pb²+ (aq) + Cu(s) - → Pb(s) + Cu²+ (aq) AG° Pb²+ (aq) + 2e¯¯ → Pb(s) Ee Cu²+ (aq) + 2e¯ → Cu(s) Fre red = kJ K for this reaction would be = -0.126 V = 0.337 V + than one.

Use the standard reduction potentials given below to predict if a reaction will occur when Al metal is put into a 1 M Fe²+ solution. aqueous Fe2+ (aq) + 2e → Fe(s) E red Al³+ (aq) + 3e →→ Al(s) E + red = If a reaction will occur, write a balanced net ionic equation for the reaction. If no reaction will occur, leave all boxes blank. ― -0.440 V -1.660 V (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) +

Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free energy AGO for the following redox reaction. Round your answer to 3 significant digits. 2C1 (aq) + 2HNO₂ (aq) + 2H* (aq) → Cl₂ (g) + x10 +2NO(g) + 2H₂O (1) X

Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free energy AG for the following redox reaction. Round your answer to 2 significant digits. 2Cr(OH)3 (s) +100H¯ (aq) +3Zn²+ (aq) → 2CrO²¯ (aq) +8H₂O (1) + 3 Zn (s) 0 x10 X

Use the standard reduction potentials given below to predict if a reaction will occur when Mg metal is put into a 1 M aqueous Cd²+ solution. Cd(s) Eº = -0.403 V red Eº → Mg(s) Fred = -2.370 V Cd2+ (aq) + 2e → 2+ Mg²+ (aq) + 2e If a reaction will occur, write a balanced net ionic equation for the reaction. If no reaction will occur, leave all boxes blank. (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) +

Consider a cell that uses the redox reaction: 3 Na (s) + La3+ (aq) → 3 Na+ (aq) + La (s). Calculate the equilibrium constant (K) for this reaction at 25 ºC, given the following standard reduction potentials: La3+ (aq) + 3 e- →  La (s)     E° = -2.37 V Na+ (aq) + e- → Na (s)         E° = -2.71 V       1.8 x 10-6     5.7 x 10-18     5.6 x 105     1.7 x 1017