41. What is observed if a piece of lead is placed in an aqueous solution of Cu(NO3)2? Half-Reaction 2+ Pb²+ (aq) + 2e → Pb(s) Cu²+ (aq) + 2e →→ Cu(s) Eº, V -0.13 (A) I only (C) Both I and II +0.34 I. The mass of the metal piece increases. II. The blue color of the solution becomes less intense. (B) II only (D) Neither I nor II

41. What is observed if a piece of lead is placed in an aqueous solution of Cu(NO3)2? Half-Reaction 2+ Pb²+ (aq) + 2e → Pb(s) Cu²+ (aq) + 2e →→ Cu(s) Eº, V -0.13 (A) I only (C) Both I and II +0.34 I. The mass of the metal piece increases. II. The blue color of the solution becomes less intense. (B) II only (D) Neither I nor II

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...

See similar textbooks

Similar questions

3) Calculate AG° Co* pe + 2es → Coc {Detailed calculation with units is a MUST} (aq)
Consider the galvanic cell based on the following half-reactions. Ag+ + e− → Ag ℰ° = +0.80 V Fe2+ + 2 e− → Fe ℰ° = −0.44 V (a) Determine the overall cell reaction and calculate ℰ ° cell . (b) Calculate ΔG° and K for the cell reaction at 25°C. (c) Calculate ℰcell at 25°C when [Ag+ ] = 1.0 ✕ 10−4 M and [Fe2+ ] = 1.0 ✕ 10−2 M.
Table 20.2 Half-reaction Ee (V) Cr3+ (aq) + 3e- ¬ Cr (s) -0.74 Fe2+ (aq) + 2e- - Fe (s) -0.440 Fe3+ (aq) + e- ¬ Fe2+ (s) +0.771 Sn4+ (aq) + 2e- - Sn2+ (aq) +0.154 ?Which of the following reactions will occur spontaneously as written Sn4+ (aq) + Fe2+ (aq) – Sn2+ (aq) + Fe (s) .a 3FE2+ (aq) - Fe (s) + 2Fe3+ (aq) .b O 3Fe (s) + 2Cr3+ (aq) - 2Cr (s) + 3FE2+ (aq) .c O 3Sn4+ (aq) + 2Cr (s) - 2Cr3+ (aq) + 3Sn2+ (aq) .d O Sn4+ (aq) + Fe3+ (aq) - Sn2+ (aq) + Fe2+ (aq) .e O
14 15 L What is AG for a redox reaction where 1 mole of electrons are transferred and Eº =-2.15 V? (F= 96,500 J/(V-mol)) What is the value of n in the Nernst equation for the reaction 2 Co³(aq) + Fe(s) → 2 Co²+ (aq) + Fe²+ (aq). > 7
Consider the following half-reactions: Half-reaction I₂(s) + 2e →→→→→21 (aq) 2H+(aq) + 2e™ Al³+ (aq) + 3e™ (1) The strongest oxidizing agent is: (2) The weakest oxidizing agent is: (3) The weakest reducing agent is: (4) The strongest reducing agent is: H₂(g) 0.000V →→→→Al(s) -1.660V (5) Will I₂(s) oxidize Al(s) to Al³+ (aq)? E° (V) 0.535V (6) Which species can be oxidized by H+ (aq)? leave box blank. If none, enter formula
For the following redox reaction calculate the Ecell and K at 298 K. 2Na+(aq) + Ca(s)→2Na(s) + Ca2+(aq) Half Reaction E(V) Na+(aq) + e- → Na(s) -2.71 Ca2+(aq) + 2e- → Ca(s) -2.87
(1) Identify each of the following half-reactions as either an oxidation half- reaction or a reduction half-reaction. half-reaction Cd(s) Cd²+ (aq) + 2e¯ 2H+ (aq) + 2e →→→H₂(g) identification (2) Write a balanced equation for the overall redox reaction. Use smallest possible integer coefficients. ]+[ +
Which of the following is the correct shorthand notation for the overall cell reaction given below. Mg(s) + Cu2+(aq) → Mg2+(aq) + Cu(s) Select one: a. Mg(s) | Mg2+(aq) || Cu2+(aq) | Cu(s) b. Cu(s) | Mg2+(aq) || Cu2+(aq) | Mg(s) c. Mg(s) | Cu2+(aq) || Mg2+(aq) | Cu(s) d. Cu(s) | Cu2+(aq) || Mg2+(aq) | Mg(s)
What are E°cell and ΔG° of a redox reaction at 25°C for which n=2 and K=0.065?
What are E°cell and ΔG° of a redox reaction at 25°C for which n=2 and K=65?
Which redox reaction is spontaneous? OCr(s) + Al³+ (aq) → Cr** (aq) + Al(s) OPb(s) + Co²+ (aq) - Pb2+ (aq) + Co(s) OCu(s) + Zn²+ (aq) Cu²+ (aq) + Zn(s) -> O Mn(s) + Fe2+ (aq) - Mn²+ (aq) + Fe(s)