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Use standard reduction potentials to predict whether the following reactions can occur under standard-state conditions. a)...
5 pts Question 6 Use standard reduction potentials to predict whether the following reactions can occur under standard-state conditions. a) oxidation of Sn2+ by Br2(aq) b) reduction of Ni2+ (aq) by Sn2+(aq) alyesbyes a) yes: b) no a) no; b) yes a) no, b) no
29. Use the Standard Reduction Potentials table to predict whether the redox reactions below would be spontaneous or nonspontaneous in the forward direction in 1.0 Maqueous solution 25°C. a) Snº+(ag) + Ni(s) → Ni2+(aq) + Sna+(aq) b) H2(g) + 2 OH- (aq) + Ca2+(ag) - Ca(s) + 2 H20 (1)
Selective Reduction The standard reduction potential for the half-reaction: Sn4+ + 2e - Sn2+ is +0.15 V. Consider data from the table of standard reduction potentials for common half-reactions, in your text. For a galvanic cell under standard conditions, which of the following anodic half reactions would produce, at the cathode a spontaneous reduction of Sn4+ to Sn2+ but not Sn2+ to Sn. no yes yes yes yes yes Fe — Fe2+ + 2e- Sn2+ Sn4+ + 2e- Sn Sn2+...
Use a table of Standard Reduction Potentials to predict if a reaction will occur between Co metal and Cl2(g), when the two are brought in contact via standard half-cells in a voltaic cell. If a reaction will occur, write a balanced net ionic equation for the reaction, assuming that the product ions are in aqueous solution. If no reaction will occur, leave all boxes blank. JC- DC Use a table of Standard Reduction Potentials to predict if a reaction will...
Predict whether the following reactions would occur spontaneously in aqueous solution at 25 °C. Assume that the initial concentrations of dissolved species are all 1.0 M Predict whether the following reactions would occur spontaneously in aqueous solution at 25 °C. Assume that the initial concentrations of dissolved species are all 1.0 M Predict whether the following reactions would occur spontaneously in aqueous solution at 25 °C. Assume that the initial concentrations of dissolved species are all 1.0 M Predict whether...
Relative Half-Cell Potentials Assuming standard conditions, answer the following questions. (Use the table of Standard Reduction Potentials for common Half-reactions from your text. If hydrogen is one of the reagents, assume acidic solution.) cf Table 11.1 on p 403 of Zumdahl 8th ed. D y Is Fe2+ (aq) capable of oxidizing Cr metal? Is Ag+ (aq) capable of oxidizing H2(g)? Is Cr3+ (aq) capable of oxidizing Fe2+(aq) to Fe3+ (aq)? Is Cr3+ (aq) capable of oxidizing Fe2+(aq)? Is Fe3+(aq) capable...
Using the standard reduction potentials given below, decide which of the following reactions will occur spontaneously as written. Fe3+(aq) + e + Fe2+(aq) E° = 0.77 V Sn4+ (aq) + 2e → Sn2+(aq) E° = 0.13V Zn2+(aq) + 2e → Zn(s) E° = -0.77 V Lit(aq) + e + Li(s) E° = -3.05 V 2Li+ (aq) + Sn2+(aq) → 2Li(s) + Sn4+(aq) Sn2+(aq) + Zn2+(aq) → Sn4+(aq) + Zn(s) Lit(aq) + Fe2+(aq) - Li(s) + Fe3+(aq) Sn4+(aq) + 2Fe2+(aq) →...
Use standard reduction potentials to calculate the standard free energy change in kJ for the reaction: 2Cu2+(aq) + Ni(s)2Cu+(aq) + Ni2+(aq) Answer: kJ K for this reaction would be _________ than one. Use standard reduction potentials to calculate the standard free energy change in kJ for the reaction: Sn2+(aq) + Cu(s) Sn(s) + Cu2+(aq) Answer: kJ K for this reaction would be _________ than one.
Selective Oxidation The standard reduction potential for the half-reaction Sn4+ + 2e - Sn2+ is +0.15 V. Consider data from the table of standard reduction potentials for common half-reactions, in your text. For a galvanic cell under standard conditions, which of the following cathodic half reactions would produce, at the anode, a spontaneous oxidation of Sn to Sn2+ but not Sn2+ to Sn4+. 2H+ + 2e - H2 Fe3+ + 3e + Fe Sn2+ + 2e Fe2+ + 2e →...
please show and explain all answers Relative Half-Cell Potentials Assuming standard conditions, answer the following questions. (Use the table of Standard Reduction Potentials for common Half-reactions from your text. If hydrogen is one of the reagents, assume acidic solution.) cf Table 11.1 on p 403 of Zumdahl 8th ed. Is Sn2+ (aq) capable of oxidizing Fe2+ (aq)? Is Sn metal capable of reducing Fe3+ (aq) to Fe2+ (aq)? Is VO2+ (aq) capable of oxidizing Fe2+ (aq)? Is Cr metal capable...