Question 9 What is the cell notation for a voltaic cell that incorporates the following redox...
3) A voltaic cell employs the following redox reaction: Sn2+ (aq) + Mn (s) →Sn (s) + Mn2+ (aq) a) Make a sketch of the cell. Label the cathode, anode, Sn2+, Mn, Sn, Mn?, and salt bridge. Indicate the direction of electron flow and the direction of ion flow from the salt bridge. b) Use line notation to represent the cell. c) What is the cell potential at 25°C when [Sn?] is 0.002 M and [Mn2+] is 0.050 M?
A voltaic cell is constructed in which the following cell reaction occurs. The half-cell compartments are connected by a salt bridge.question 1 - Sn2+(aq)+ Co(s) ----------> Sn(s)+ Co2+(aq)The anode reaction (including states) is:The cathode reaction (including states) is:In the external circuit, electrons migrate _____fromto the Co|Co2+ electrode _____fromto the Sn|Sn2+ electrode.In the salt bridge, anions migrate _____fromto the Sn|Sn2+ compartment _____fromto the Co|Co2+ compartment.question 2 -A voltaic cell is constructed in which the anode is a Cd|Cd2+ half cell and the cathode is a Cu+|Cu2+ half cell. The half-cell...
Given the following standard reduction potentials choose the cell which will work as a voltaic cell. All cells below are written according to the usual cell diagram convention. Cu2+(aq) + 2e → Cu(s) E° = 0.34 V 2H+(aq) + 2e → H2(g) E° = 0.00 V Sn2+ (aq) + 2e → Sn(s) E° = -0.14 V Ni2+(aq) + 2e → Ni(s) E° = -0.26 V Cd2+(aq) + 2e → → Cd(s) E° = -0.40 V Sn(s) | Sn2+(aq) || Ni2+(aq)...
Question 5 (Q3) The cell notation for a voltaic cell with the following redox reaction is: Fe2+ (aq) + 2e → Fe(s) (oxidation) » Cr3+ (aq) + 3e" (reduction) Cr(s) Cr3+ (aq) | Cr (s) "Fe (s) | Fe2+ (aq) Cr3+ (aq) | Cr (s) " Fe2+ (aq) | Fe (s) Fe2+ (aq)| Fe (s) "Cr (s) [Cr3+ (aq) II Cr(s) | Cr3+ (aq) Fe2+ (aq)| Fe (s) None of the above
A voltaic cell is constructed using silver and aluminum. The following is the unbalanced redox reaction: Ag+ (aq) + Al(s) Ag (s) + A13+ (aq) What is the correct, balanced redox reaction that occurs in the cell? O A 5 Ag+ (aq) + 3 AI (5) - 5 Ag (s) + 3 A13+ (aq) O B. Ag* (aq) + 4 AI (5) ► Ag (s) + 4 A13+ (aq) OC 3 Ag* (aq) + Al(s) — 3 Ag (s) +...
26. Determine the redox reaction represented by the following cell notation. Fe(s) I Fe2+(aq) I| Cu2+(aq) I Cu(s) A) Cu(s) + Fe2+(aq) B) Fe(s)+Cu2+(aq) Cu(s)+ Fe2+(aq) C) 2 Fe(s)+ Cu2+(aq)Cu(s) + 2 Fe2+(aq) D) 2 Cu(s) + Fe2+(aq)Fe(s)+ 2 Cu2+(aq) E) 3 Fe(s) + 2 Cu2+(aq) 2 Cu(s)+3 Fe2+(aq) Fe(s) + Cu2+(aq)
Which of the following is the cell notation for a voltaic cell based on the following reaction? Y(s) + X(NO3)2(aq) - Y(NO3)2(aq) + X(s) X(s)[X?" (aq) || Y?"(aq)|Y(s) Y()NO, (aq) | NO, (aq) X(s) OYS)Y?"(aq) || X2(aq) || X(s) X(s) X(NO3)2(aq) | Y(NO3)2(aq) (s) Question 22 AG for the ionization of a salt in water is -13.41 kJ/mol under standard conditions. Which is the equilibrium constant for this reaction? (R = 8.314 J/K mol) In the context of the diagram...
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
b. Write the cell notation for the following redox reaction. Here, Cu+ or CuNO3 is oxidized to Cu2+ or Cu(NO3)2in the oxidation half-cell. Since there is only aqueous species and there is no electrode (metal) in the oxidation half-cell, use platinum (Pt) as an inert electrode in the oxidation half-cell. 3CuNO3(aq) + Au(NO3)3(aq) ⟶ 3Cu(NO3)2(aq) + Au(s)
Exercise 18.15 The voltaic cell is represented with the line notation. Standard Reduction Half-Cell Potentials at 25 °C Half Reaction HNO2 (aq) + 2 H+ (aq) + e--+ NO(g) + H20(1) NO. (aq) + 4 H + (aq) + e-? NO(g) + 2 H2O(1) sn't (aq) + 2 e-? Sn2 + (aq) 2H+ (aq) + 2e-?H2(g) Sn2+ (aq) + 2 e-? Sn(s) E (V) 0.98 0.96 0.15 0.00 -0.14