Based on the electrode potentials given for the metals below, which of the following statements is correct? Au+3 + 3e → Au (s) E° = 1.50 V Ag* + e → Ag (s) E° = 0.800 V Cut2 + 2e- Cu(s) E° = 0.339V %3D Zn+2 + 2e- Zn(s) E° =- 0.762V It is possible to precipitate metallic silver from silver nitrate solution using copper metal It is possible to precipitate metallic zinc from zinc sulfate solution using gold metal It is possible to precipitate metallic copper from cupric sulfate solution using silver metal It is possible to precipitate metallic zinc from zinc sulfate solution using silver metal 0000

Based on the electrode potentials given for the metals below, which of the following statements is correct? Au+3 + 3e → Au (s) E° = 1.50 V Ag* + e → Ag (s) E° = 0.800 V Cut2 + 2e- Cu(s) E° = 0.339V %3D Zn+2 + 2e- Zn(s) E° =- 0.762V It is possible to precipitate metallic silver from silver nitrate solution using copper metal It is possible to precipitate metallic zinc from zinc sulfate solution using gold metal It is possible to precipitate metallic copper from cupric sulfate solution using silver metal It is possible to precipitate metallic zinc from zinc sulfate solution using silver metal 0000

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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Use the appropriate standard reduction potentials below to determine the equilibrium constant at 386 Kfor the following reaction under acidic conditions. 4H* (ag) + MnO, (s) +2Fe²*(aq) Mn²+ (aq) + 2Fe³+(aq) +2H,0(1) Standard reduction potentials: Mn²+ (aq) +2H,o(1) E° = 1.23 V MnO, (s) +4H*(aq) +2e¯ Fe+ (aq) +e¯ → Fe2+(ag) E° = 0.770 V
Cr3+(aq) + 3e- à Cr(s) -0.763 V Au+(aq) + e- à Au(s) 1.680 V Determine the products of the aqueous salt solution of your choice from the standard reduction potential above, if it undergoes electrolysis.
Using the following standard reduction potentials, 34 Fe *(aq) + e - Fe2*(aq) Ni2*(ag) + 2 e -Ni(s) E° = +0.77 V E° = -0.26 V calculate the standard cell potential for the cell reaction given below, and determine whether or not this reaction is spontaneous under standard conditions 34, Ni 2*( aq) + 2 Fe 2*( aq) → 2 Fe *( aq) + Ni( s) E° = +1.03, nonspontaneous E° = + 1.03, spontaneous E° = -1.03 V, spontaneous E° = -1.03 V, nonspontaneous
Based on the reduction potential data, what is the standard cell potential for the following electrochemical cell reaction: Cu(s) + 2Ag* → Cu2+(aq) + 2Ag(s) E°red = +0.800 V for Ag*(aq) + e → Ag(s) E°red = +0.340 V for Cu2"(aq) + 2e → Cu(s) O +0.460 V O +1.14 V O +1.26 V -0.460 V
Use the standard reduction potentials given below to predict if a reaction will occur when Zn metal is put into a 1 M aqueous Ag solution. Ag+ (aq) + e → Ag(s) E red Zn²+ (aq) + 2e¯ → Zn(s) Ee -0.763 V Fred = 0.799 V 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.) + -> +
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.) +
True or False: The reaction, S₂082- + Ni(OH)2 + 2OH2SO42- + NiO2 + 2H₂O, will occur spontaneously under standard state conditions. Following are the standard reduction potentials that may be useful: NiO2 + 2H₂O +2e=Ni(OH)2 +2OH E = 0.49 V S2082 +2e=2SO4²- True False E° = 2.01 V
Given the following electrochemical cell, calculate the potential for the cell in which the concentration of Ag+ is 0.0765 M, the pH of the H* cell is 2.700, and the pressure for H₂ is held constant at 1 atm. The temperature is held constant at 55°C. Ag Ag+ H+ Standard reduction potentials: 2H+ +2e¯ → H₂ Eº = 0 V Ag+ le - H₂(g) → Ag Eº=0.800 V
1. Consider the following standard reduction potentials in acid solution: E°(V) -1.66 +0.07 +0.14 Fe³+ + e +0.77 The strongest reducing agent among those shown above is Hint: If answer is with charge, type this way: X2+ Al³+ + 3e → Al(s) AgBr(s) + e → Ag(s) + Brā Sn4+ + 2e → + 2e → Sn²+ Fe²+
Standard Electrode Potentials at 25 °C Reduction Half-Reaction 2 H₂O(0+2 e Mn²+ (aq) + 2 e Al³+ (aq) + 3 e. Mg²+ (aq) +2 e Na (aq) + e Ca²+ (aq) + 2 e Bat (aq) +2 e K¹(aq) + e consider the following redox reaction: 2 Al(s) +3 Mg2+ (aq)-2 Al³+ (aq) + 3 Mg(s) 1) What is the Eº for the reaction? 2) Calculate AG for the redox reaction at 25°C. The answer to 1) is [Select] The answer to 2) is [Select] A →→H₂(g) + 2 OH(aq) - Mn(s) -Al(s) Mg(s) -Na(s) -Ca(s) -Ba(s) -K(s) E° (V) -0.83 -1.18 -1.66 -2.37 -2.71 -2.76 -2.90 -2.92
What is the equilibrium constant for the following reaction at 25 °C? Round your answer to 1 decimal place. 2 Cu(s) + 2 Ag+ (aq) ⇒ Cu²+ (aq) + 2 Ag (s) = Note: Reference the Standard reduction potentials at 25 °C table for additional information. K = = x10
Use standard reduction potentials to calculate the standard free energy change in kJ for the reaction: 2H+ (aq) + Hg(1)→ H₂(g) + Hg²+ (aq) 2H+ (aq) + 2e¯ → H₂(g) Fº red 2+ Hg2 (aq) + 2e¯ → Hg(1) AGO = || kJ K for this reaction would be Eº red = 0.000 V = = 0.855 V than one.