What is E for a cell where E°=1.10 (Cu2++Zn→Cu+Zn2+), [Cu2+]=1.25 M, and [Zn2+]=0.0075 M at SATP? 1.25 V 0.95 V 1.03 V 1.17 V
What is E for a cell where E°=1.10 (Cu2++Zn→Cu+Zn2+), [Cu2+]=1.25 M, and [Zn2+]=0.0075 M at SATP?...
What is E for a cell where Eº=1.10 (Cu2++Zn--Cu+Zn2+), [Cu2+3=1.50 M, and [Zn2+2=0.0050 M at SATP? 0.93 V 1.27 V 1.17 V 1.03 V
Choose the correct Nernst equation for the cell Zn + Cu2+ à Zn2+ + Cu E = E° - 0.0296 log(Cu / Zn) E=E° - 0.059 log([Zn2+] / [Cu2+]) E = E° - 0.0296 log(Zn / Cu) E = E° - 0.0296 log([Zn2+] / [Cu2+]) E = E° - 0.0296 log([Cu2+] / [Zn2+]) 20 points
Given: Zn2+ (aq) + 2e Zn(s); E--0.76 V Cu²+ (aq) +20 Cu(s); E° -0.34 V What is the cell potential of the following electrochemical cell at 25°C? Zn(s) | Zn2+(1.0 M) || Cu2+(0.0010 M) Cu(s) a) greater than 1.10 v b) between 0.76 and 1.10 V c) less than 0.42 V d) between 0.00 and 0.76 V e) between 0.34 and 0.76 V
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+
What is the potential of a cell made up of Zn/Zn2+ and Cu/Cu2+ half-cells at 25°C if [Zn²+1 -1.00 Mand (Cu2+] = 0.05 M?
What is the potential of a cell made up of Zn / Zn2+ and Cu / Cu2+ half-cells at 25°C if[Zn2+] = 0.31 M and [Cu2+] = 0.51 M ?
The voltage of the cell combination of Cu/Cu2+ and Zn/Zn2+ is 0.953V. The standard reduction potential for Cu/Cu2+ is expected to be 0.34V. Determine the reduction potential for Zn/Zn2+
For the following cell what is the cell potential under standard conditions? Zn + Cu2+ → Cu + Zn2+ If Cu2+ + 2e- → Cu E° = 0.34V and Zn2+ + 2e- → Zn E° = -0.76 V
The value of Eº for the following reaction is 1.10 V. What is the value of E (V) for this reaction when the concentration of Cu2+ is 1.0 x 10- M and the concentration of Zn2+ is 1.0 M? Zn (s) + Cu²+ (aq) → Cu (s) + Zn2(aq) a) 1.40 b) 1.25 c) 0.95 d) 0.80 a C с
Please show detailed steps.
The standard emf for the following voltaic cell is 1.10 V: Zn(s)/Zn2 (aq)Cu+(aq)Cu(s) 4. (4 Pts) Calculate the equilibrium constant for the reaction: Zn(s)+Cu2 (aq) Zn2 (aq) + Cu(s)