37. What is the Ecell at 25°C for the following reaction and is it spontaneous? Zn(s)...
Page 2 of 14 5) Which of the following reactions would be the most spontaneous t 298 K? B) A + B → 2 C; E"cell =-0.030 V C) A + B--3 C; E"cell-+0.15 V D)A+B-, C; E"cell-+1.22 V E) More information is needed to determine. 6) Which of the following is the best reducing agent? Ni2.(aq) + 2 e-→ Ni(s)-0.23 V Zn2(aq) + 2e-Zn(s)-0.76 V Ag+(aq) + e-→ Ag(s) 0.80 V a) Ni2+ b) Ni c) Zn d) Ag
38. The following redox half reactions are combined in a voltaic cell. Which reaction occurs at the cathode and what is the Eceu? Fe2+(aq) + 2e → Fe(s) E°=-0.44 V Cu²+(aq) + 2e → Cu(s) E°= 0.34 V a) b) c) d) Cu2+(aq) + 2e → Cu(s), Ecell = 0.78 V Fe2+(aq) + 2e → Fe(s), Ecel = 0.78 V Fe2+(aq) + 2e → Fe(s), Ecell =-0.10 V Cu²+(aq) + 2e → Cu(s), Ecel = 0.10 V Cu²+ (aq) +...
Calculate the standard free-energy change at 25 ∘C for the following reaction: Mg2+(aq) + Zn(s) → Mg(s) + Zn2+(aq) Express your answer to three significant figures and in units of kJ/mol. Consider constructing a voltaic cell with one compartment containing a Zn(s) electrode immersed in a Zn2+ aqueous solution and the other compartment containing an Al(s) electrode immersed in an Al3+ aqueous solution. What is the spontaneous reaction in this cell? Group of answer choices Zn + Al3+ → Al...
46 AM Tue 23 Jun T3-EOY-CHM61 + 12 - 15 35:3 Consider the following spontaneous reaction that describes a galvanic cell and the information below: Zn (s) + Fe2+ (aq) Zn2+ (aq) + Fe (s) Zn2+(aq) + 2 e- → Zn(s) E° = -0.76 V Fe2+ * (aq) + 2 e- → Fe(s) E° = +0.44 V The Ecell V. O a. +1.20 O b. - 1.20 с
1.) For the complete balanced redox reaction below, what is the Eocell? Zn(s) + 2Cu+(aq) ⟶ 2Cu(s) + Zn2+(aq) Zn2+ + 2e- Zn(s) Eo = -0.76 V Cu+ + e- Cu(s) Eo = 0.52 A) -1.28 V B) +1.28 V C) 0.24 V D) -0.24 V E) +2.56 V 2.) For the redox reaction below, what is the Ecell if [Zn2+] = 0.072 M and [Cu+] = 1.27 M? T = 298 K Zn(s) + 2Cu+(aq) ⟶ 2Cu(s) + Zn2+(aq) Half Reactions:...
A voltaic cell consists of a Zn/Zn2+ half-cell and a Ni/Ni2+ half-cell at 25 ∘C. The initial concentrations of Ni2+ and Zn2+ are 1.80 molL−1 and 0.130 molL−1, respectively. Zn2+(aq)+2e−→Zn(s)E∘=−0.76V Ni2+(aq)+2e−→Ni(s)E∘=−0.23V A) What is the cell potential when the concentration of Ni2+ has fallen to 0.600 molL−1? B) What are the concentrations of Ni2+ and Zn2+ when the cell potential falls to 0.45 V?
this is the complete question (no more info) Determine the voltage (V) of the following cell at 25°C: Zn(s) | Zn2+(aq, 0.37 M) || Cl-laq, 0.75 M) C12(g, 0.750 atm)| Pt Standard reduction potentials, 298 K, Aqueous Solution (pH = 0): Cl2(g) + 2e --> 2C1-(aq); E° = +1.36 V Hg2Cl2(s) + 2e --> 2Hg(l) + 2Cl(aq); E° = +0.27 V AgCl(s) + e --> Ag(s) + Cl (aq); E° = +0.22 V Ni2+(aq) + 2e --> Ni(s); E° =...
A voltaic cell consists of a Zn/Zn2+ half-cell and a Ni/Ni2+ half-cell at 25 ∘C. The initial concentrations of Ni2+ and Zn2+ are 1.60molL−1 and 0.130 molL−1, respectively. Zn2+(aq)+2e−→Zn(s)E∘=−0.76V Ni2+(aq)+2e−→Ni(s)E∘=−0.23V Part A What is the initial cell potential? Part B What is the cell potential when the concentration of Ni2+ has fallen to 0.600 molL−1? Part C What are the concentrations of Ni2+ and Zn2+ when the cell potential falls to 0.45 V?
Consider the voltaic cell and reduction half potentials: Zn(s) | Zn 2+(aq) (0.100 M) || Ni2+(aq) (1.50 M) | Ni(s) Zn 2+ (aq)/Zn (s) E o = - 0.760 V Ni2+ (aq)/Ni (s) E o = - 0.230 V a) Sketch the voltaic cell represented with the above line notation. Label the anode and cathode and indicate the half-reactions occurring at each electrode and the species present in each solution. Also indicate the direction of electron flow (3 marks). b)...
4. Write a balanced equation from each cell notation, then calculate thee of the cell, is it spontaneous or nonspontaneous? A. Cr(s) Crot || Cui Cu(s) B. Al(s) Al* | Ce Ce Pt C. Cu (s) Cu? || Al Al (s) Useful information: F= 96485 J/V mol electrons, AG ----F-Ecell AG --RTINK: Ece 0.0592/n*logK; EcellEcett -0.0592/n*logQ Ce (aq) + Ag+ (aq) + e Fet (aq) + Cu" (aq) + Cu (aq) + 2e 2H(aq) + 2 Pb (aq) + 2e...