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Foll for the following galvanic cell is -0.39 V Sn+(aq) +2 I(aq) Sn2 (aq) + 2(s)...
20iii please and thanks
Long Answer 20. A galvanic (voltaic) cell consists of Ag/Ag* and Sn/Sn2 half cells at standard conditions with a salt bridge containing KCI. Sn2+ (aq) + 2 e-→ Sn (s) Eo =-0.137 V Ag (aq) e > Ag (s)+0.800 V i. ii. Write a balanced equation for the spontaneous redox reaction and determine Ee Sketch this galvanic cell. Label the anode, the cathode, the direction of flow of electrons in the external circuit and the direction...
40 points A galvanic cell is constructed using the following half reactions: Sn2++ 2 e-Sn(s) -0.14 V Cu2+ + 2 e Cu (s) +0.34 V Based on their reduction half-potentials, which metal will likely serve as the cathode and what would be the Eºcell for the cell? -0.20 V; Sn O +0.48 V; Cu +0.20 V; Cu -0.48 V; Sn O +0.20 V; Sn Previous Submit
5. The overall cell reaction in a galvanic cell is Sn(s) + Cu* (aq)>Sn (aq)+ Cu (s). (a) Draw a diagram of this cell (similar to Figure 2) (b) Use standard reduction potentials (Table 1) to calculate the theoretical cell voltage, el
What is the shorthand notation that represents the following galvanic cell reaction? Sn2+(aq) + Cl2(g) → Sn3+(aq) + 2 Cl-(aq) A) Pt(s) ∣ Sn2+(aq), Sn3+(aq) ∣∣ Cl2(g) ∣ Cl-(aq) ∣ C(s) B) Sn(s) ∣ Sn2+(aq) ∣∣ Sn4+(aq) Cl2(g) ∣ Cl-(aq) ∣ C(s) C) Pt(s) ∣ Sn4+(aq), Sn2+(aq), Cl2(g) ∣∣ Cl-(aq) ∣ C(s) D) Sn2+(aq) ∣ Sn3+(aq) ∣∣ Cl2(g) ∣ Cl-(aq)
A voltaic cell is constructed that is based on the following reaction: Sn2+(aq)+Pb(s)→Sn(s)+Pb2+(aq). a. If the concentration of Sn2+ in the cathode compartment is 1.50 M and the cell generates an emf of 0.22 V , what is the concentration of Pb2+ in the anode compartment? b. If the anode compartment contains [SO2−4]= 1.50 M in equilibrium with PbSO4(s), what is the Kspof PbSO4?
QUESTION 5 The following reaction takes place in the galvanic cell below: Zn(s) + Sn2+(aq) + Zn2+(aq) + Sn(s) IT Select all statements that are true. A. Zn is the anode. B. Electrons flow from the zinc electrode to the tin electrode. Anions flow from the salt bridge toward the zinc electrode. UD. The mass of zinc electrode decreases while the mass of the tin electrode increases as the reaction progresses,
QUESTION 5 The following reaction takes place in the galvanic cell below: Zn(s) + Sn2+(aq) + Zn2+(aq) + Sn(s) IT Select all statements that are true. A. Zn is the anode. B. Electrons flow from the zinc electrode to the tin electrode. Anions flow from the salt bridge toward the zinc electrode. UD. The mass of zinc electrode decreases while the mass of the tin electrode increases as the reaction progresses,
A voltaic cell employs the following redox reaction: Sn2+(aq)+Mn(s)---- Sn(s)+Mn2+(aq) Calculate the cell potential of 25 degrees Celsius under each of the following conditions. Part A: Sn2+= 1.15*10^-2 M; and Mn2+= 2.37 M Part B: Sn2+= 2.37 M; and Mn2+= 1.15*10^-2
A standard galvanic cell is constructed in which a Sn2+ | Sn half cell acts as the cathode. Which of the following statements are correct? Hint: Refer to a table of standard reduction potentials. (Choose all that apply.) The anode reaction could be Mg -> Mg2+ + 2e-. Br2|Br- could be the other standard half cell. Sn is oxidized at the cathode. In the external circuit, electrons flow from the other compartment to the Sn2+|Sn compartment. As the cell runs,...
For a galvanic cell using the reaction Cu2+ (aq) + Sn2+ (aq) Cu (s) + Sn4+ (aq), calculate the cell potential at 25°C when [Cu2+] = 2.5 × 10-3 M, [Sn2+] = 2.5 × 10-4 M and [Sn4+] = 3.5 × 10-3 M