3A. Calculate ΔG for the following reaction: Cu2+(1M,aq)+Zn(s)→Cu(s)+Zn2+(1Maq)
Report the answer with units of J to three significant figures
3A. Calculate ΔG for the following reaction: Cu2+(1M,aq)+Zn(s)→Cu(s)+Zn2+(1Maq) Report the answer with units of J to...
Given the following reaction, Cu2+(aq) + Zn(s) → Cu(s) + Zn2+(aq) E° = 1.10 V Use the Nernst equation to calculate the cell potential for the cell described with standard line notation below. Zn|Zn2+(0.5038 M)||Cu2+(0.3981 M)|Cu Units are not required. Report answer to three decimal places.
The Standard Cell Potential E0 for the following reaction: Zn(s) + Cu2+ (1M) --> Zn2+ (aq, 1M) + Cu(s) is E0=1.10V. What would be the cell potential E for reaction Zn(s) + Cu2+ (2M) --> Zn2+ (aq, 0.010M) + Cu(s) ? Is it smaller than 1.10V or larger than 1.10V? Explain your answer
Calculate for the reaction: Zn! Zn2+ (0.60M)| |Cu2+ (0.20M)|Cu Given the following: Cu2+(aq) + Zn(s) Cu(s) + Zn2+(aq) Eo-1.10V
Cell: Fe(s)| Fe2+(aq, 1M) | Cu2+(aq, 1M) | Cu(S) Calculated Values ΔG° = -nFE° = ΔH° - TΔS° ΔH° = -0.34905 J/C * 2 mols * 96485 C/mol = -67,356.18 J =67.36kJ ΔS° = 0.8597 x 10-3 J/C * 2 mols * 96485 C/mol = 165.89 J ΔG° =-67356.18 J – (298*165.9 J) = -116794.4 J = -116.79 kJ Theoretical Values ΔG⁰ = -(2 mols *96485 C/mol * 1.07 J/C) = -206.48 kJ ΔH⁰ = ΔS⁰ = Cell: Zn(s)| Zn2+(aq,...
Identify the oxidation half reaction of Zn(s). Select one: O Zn(s) + Cu2+ (aq) → Zn2+ (aq) + Cu(s) O Zn²+ (aq) + 2e + Zn(s) Zn(s) → Zn2+ (aq) + 2 e Zn(s) → Zn2+ (aq) +e
Browse My Computer QUESTION 45 For the following reaction: Zn (s) + Cu2+ (aq) → Zn2+ (aq) + Cu (8) is oxidized. is reduced. is an oxidizing reagent. is a reducing reagent. OUFSTION 46
Based on the reactions blow arrange the metals in their increasing reactivity. Cu(s)+ 2Ag+(aq)-->Cu2+(aq)+ 2Ag(s) 2Ag+(aq)+Zn(s)--->Zn2+(aq)+2Ag(s) Zn(s)+Cu2+(aq)-->Zn2+(aq)+Cu(s)
- Zn2+ Choose... Choose... (1pts) Identify the complete redox reaction for a ZnZn2+1|Cu2+1Cu cell. A. Zn(s) + Cu?+ (aq) (aq) + Cu(s) B. Zn(s) + Cu(s) → Zn2+ (aq) + Cu2+ (aq) C. Zn2+ (aq) + Cu(s) Zn(s) + Cu2+ (aq) D. Zn (s) + 2 Cu(s) — Zn2+ (aq) + 2 Cu2+ (aq) (1pts) Identify the complete redox reaction for a Zn/Zn2+||Pb2+1Pb cell. A. Zn (s) + Pb(s) Zn2+ (aq) + Pb2+ (aq) B. Zn2+ (aq) + Pb(s) Zn(s)...
What is the cathode in this reaction? Zn2+ + Cu → Zn + Cu2+ a) Cu b) There is no cathode in this reaction. c) This is not an oxidation/reduction reaction. d) Zn2+
Consider the cell: Zn(s)ǀ(Zn2+(0.20 M)ǁCu2+(0.20 M)ǀCu(s) with Eº(Cu2+/Cu = 0.34 v and Eº(Zn2+/Zn) = –0.76 v a) Write the cell reaction which occurs when the cell produces current and calculate Ecell. b) If each cell compartment contains 25.0 mL of the corresponding metal salt solution and 25.0 mL of 3.00 M NH3(aq) is added to the Cu2+ solution, Ecell = 0.68 v. Use these data to calculate Kf for Cu(NH3)42+. Cu2+(aq) + 4 NH3(aq) ⇄ Cu(NH3)42+