Please show detailed steps. The standard emf for the following voltaic cell is 1.10 V: Zn(s)/Zn2...
Consider the reaction corresponding to a voltaic cell and its standard cell potential. cell Zn(s) + Cu2+ (aq) + Cu(s) + Zn2+ (aq) E = 1.1032 V As What is the cell potential for a cell with a 2.573 M solution of Zn²+ (aq) and 0.1055 M solution of Cu²+ (aq) at 432.4 K?
Consider the reaction corresponding to a voltaic cell and its standard cell potential. Zn(s) + Cu2+ (aq) Cu(s) + Zn2+ (aq) ЕО cell = 1.1032 V What is the cell potential for a cell with a 2.440 M solution of Zn2+ (aq) and 0.1636 M solution of Cu²+ (aq) at 439.5 K?
8. The standard cell potential (E°cell) for the reaction below is +1.10 V. Calculate the cell potential for this reaction when the concentration of [Cu2+] = 1.0 × 10-5 M and [Zn2+] = 3.5 M. Zn (s) + Cu2+ (aq) → Cu (s) + Zn2+ (aq)
Question 2 (1 point) Consider the following voltaic (galvanic) cell: Zn(s) | 0.010 mol/L Zn2+ (aq) || 1.0 mol/L Cu2+(aq) | Cu(s) What is the predicted cell potential when this cell is operated? 1.04 V 1.10 V 0.76 V 0.34 V 1.16 V
Hello is the answer 1.041 or 1.16 point) Consider the following voltaic (galvanic) cell: Zn(s) 0.010 mol/L Zn2+ (aq) || 1.0 mol/L Cu2+(aq) | Cu(s) What is the predicted cell potential when this cell is operated? 1.04 V 1.10 V 0.76 V 0.34 V 1.16 V
Consider the reaction corresponding to a voltaic cell and its standard cell potential. Zn(s) + Cu²+ (aq) + Cu(s) + Zn2+ (aq) = 1.1032 V What is the cell potential for a cell with a 2.401 M solution of Zn2+ (aq) and 0.1776 M solution of Cu²+ (aq) at 420.4 K? Answer:
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+
Consider a voltaic cell where the anode half-reaction is Zn(s) → Zn2+(aq) + 2 e− and the cathode half-reaction is Sn2+(aq) + 2 e– → Sn(s). What is the concentration of Sn2+ if Zn2+ is 2.5 × 10−3 M and the cell emf is 0.660 V? The standard reduction potentials are given below Zn+2(aq) + 2 e− → Zn(s) E∘red == −0.76 V Sn2+(aq) + 2 e– → Sn(s) E∘red −0.136 V
A voltaic cell is constructed that uses the following reaction and operates at 298 K. Zn(s) + Ni2+(aq) Zn2+(aq) + Ni(s) (a) What is the emf of this cell under standard conditions? ___________ V (b) What is the emf of this cell when [Ni2+] = 2.88 M and [Zn2+] = 0.187 M? ___________ V c) What is the emf of the cell when [Ni2+] = 0.129 M and [Zn2+] = 0.961 M? ____________ V
A voltaic cell is constructed that uses the following reaction and operates at 298 K. Zn(s) + Ni2+(aq) Zn2+(aq) + Ni(s) (a) What is the emf of this cell under standard conditions? V (b) What is the emf of this cell when [Ni2+] = 3.51 M and [Zn2+] = 0.191 M? V (c) What is the emf of the cell when [Ni2+] = 0.137 M and [Zn2+] = 0.878 M? V