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Consider a voltaic cell al 25 degree Celsius in which the reaction is: Zn (s) +...
In a test of a new reference electrode, a chemist constructs a voltaic cell consisting of a Zn/Zn2 half- cell and an H2/H half-cell under the following conditions: [Zn2] = 0.042 M [H]- 19 M partial pressure of H2 =0.37 atm. Calculate Ecell at 298 K (enter to 3 decimal places). Zn2 (aq) + 2e +2H (aq) + 2e1 Eo-0.76 V E 0.00 V Zn(s) H2(g)
In a test of a new reference electrode, a chemist constructs a voltaic cell consisting of a Zn/Zn2+ half-cell and an H2/H+ half-cell under the following conditions: [Zn2+ ] = 0.021 M [H+ ]= 1.3 M partial pressure of H2 = 0.32 atm. Calculate Ecell at 298 K (enter to 3 decimal places). Zn2+ (aq) + 2e − ⟶ Zn(s) E° = − 0.76 V 2H+ (aq) + 2e − ⟶ H2(g) E° = 0.00 V We were unable...
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)...
tion 3 of 40 ) A voltaic cell employs the redox reaction: Zn (s) + Pb2+ (aq) — Zn2+ (aq) + Pb () where Pb2+ (aq) + 2e Zn2+(aq) + 2e Pb(s) E = -0.1262 V Zn(s) E = -0.7618 V The cell potential (Ecell) of this voltaic cell when [Pb2+1 = 1.10 M and [Zn2+) = 0.00110 Mis:
Question 1 1 pts For the cell: Zn(s) + 2H+ (aq) + Zn2+(aq) + H2 (g) If [Zn2+) = 1 M, PH2 = 1 atm, and E = 0.549 V what is pH? Question 2 1 pts Calculate the voltage for the following cell at 25° ZnZn+2 ( 2.832 M) || Cd2+ (0.027 M)| Cd
If the potential of a Zn-H+ cell (see below) is 0.45 V at 25 C when the [Zn2+] = 1.0M and PH2 = 1 atm, what is the pH of the cathode solution? Zn(s)|Zn2+(aq)|| H+(aq)|H2 (g)|Pt
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 galvanic cell was constructed with a Zn/Zn2+ half cell and an H2/H+ half cell(standard hydrogen electrode, SHE). Calculate Ecell under the following conditions: [Zn2+] = 0.01 M, [H+] = 2.5 M, and PH2 = 0.30 atm at 25°C?
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) = 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: