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Given: Zn2+ (aq) + 2e Zn(s); E--0.76 V Cu²+ (aq) +20 Cu(s); E° -0.34 V What...
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+
Half-Reaction Fe2+(aq) + 2e Fe(s) Hg2+ (aq) + 2e Hg() Ag+ (aq) + e + Ag(s) Cu2+ (aq) + 2e + Cu(s) Zn2+ (aq) + 2e → Zn(s) E (V) -0.44 0.86 0.80 0.34 - 0.76 Using the table, calculate Eºcell for the following electrochemical cell under standard conditions voltmeter a) 1.24 V Fe. salt bridge Ag b) -1.24 V c) 2.04 V d) - 2.04 V Ag a b С
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
Using the information in the table: Which combination of metals, if used to create an electrochemical cell, would produce the largest voltage? Liu lur the reaction between Zn and Cu2+ ions is 1.1030 V, we can use the known value for the half-cell potential for zinc to determine the half-cell potential for copper: Zn(s) → Zn2+(aq) + 2e + Cu2+(aq) + 2e → Cu(s) Zn(s) + Cu2+ (aq) → Zn2+ (aq) + Cu(s) E half-cell = 0.7628 V Eºhalf-cell =...
4. Zn2+(aq) + 2e Zn(s) E = -0.762 V Ag+ (aq) + e # Ag(s) E = 0.799 V Determine the voltage of the galvanic cell generated from these two half reactions, and calculate E of the cell when Zn2+ (aq) = 0.0100 M and Ag+ (aq) = 0.900 M at 25°C. Report the value of E
Using the table below: 19. Three combinations of metals are listed below, which combination would produce the largest voltage if they were used to construct an electrochemical cell? Copper (Cu) with zinc (Zn) Lead (Pb) with zinc (Zn) Lead (Pb) with cadmium (Cd) Liu lur the reaction between Zn and Cu2+ ions is 1.1030 V, we can use the known value for the half-cell potential for zinc to determine the half-cell potential for copper: Zn(s) → Zn2+(aq) + 2e +...
Candidate l: Zn(s) | Zn2+(aq,0.500 M) I Cu2+(aq, 1.00 M) Cu(s) Candidate 2: Pb(s) | Pb2+(aq, 0.500 M) || Cu2+(aq, 1.00 M) Cu(s) Candidate 3: Mg(s) | Mg2+(aq, 0.500 M) | Pb2+(aq, 1.00 M)| Pb(s) (a) 6 pts) Choose one of the candidate voltaic cells #1, #2, or #3. Draw a schematic cell diagram for the candidate voltaic cell of choice. Clearly label anode, cathode, electrodes, ions and their concentrations, salt bridge, and the flow of electrons. (b) (5 pts)...
Given are two half-cells, described by the equations: Zn^(2+)(aq) + 2e- -> Zn(s) E(standard) = -0.76 V Ag^(+)(aq) + e- -> Ag(s) E(standard) = +0.80 V A. Write down the net equation for the spontaneous reaction that takes place in the cell. B. Draw the two half cells and mark the anode and the cathode. C. Mark the solutions' concentration necessary in order to reach the standard potential. D. How will the cell's potential be influenced by the addition of...
Given the following half-cell potentials, i. Zn2+ + 2 e– → Zn (E° = –0.76 V) ii. Cr3+ + 3 e– → Cr (E° = –0.74 V) determine the cell potential whose overall redox reaction under standard conditions is 3 Zn(s) + 2 Cr3+(aq) → 3 Zn2+(aq) + 2 Cr(s): * A. –0.80 V B. –0.02 V C. +0.02 V D. +0.80 V