Consider the following electrochemical cell at 25 C: Pt|H2(g,p)|HCl(aq), 0.010 mol.kg-1|AgCl(s)|Ag For this cell the cell reaction is as follows: 2AgCl(s) + H2(g)  2Ag(s) + 2HCl (a) Write the reaction quotient (Q) and the Nernst equation for this cell reaction expressed in terms of activity coefficients. (b) Calculate the standard Gibbs free energy for the cell reaction.  (c) If the mean activity coefficient has a value of 0.889, calculate the cell potential for this cell.

For the following electrolyte-concentration cell consisting of two cells back to back by electrodes, What is the suitable Nernst Equation at 25 0C? Pt;H2,HCl(a1),AgCl(s),Ag,| Ag, AgCl(s),HCl(a2),H2;Pt

Prepare a sketch and write the half-reactions and overall cell reaction for the electrochemical cell designated by:       Pt(s) | Ag(s) |AgCl(s) | Cl-(a = 1) | Cl2(g, 1 bar)| C(graphite) | Pt(s)

A cell at 25oC is described by the following cell notationZn(s) | Zn2+(aq) || Zn2+(aq) | Zn(s)The concentration of zinc ions at the cathode is 0.50M while the concentration of zinc ions at the anode is 0.10M. Based on the given cell notation and concentrations, (show proper units and box final answers)A) Calculate the standard free energy change.B) Calculate the cell potential.C) If the given concentrations of zinc ions for anode and cathode are reversed, will the reaction proceed forward or backward?

Consider the following electrochemical cell at 25 C: Pt|H2(g,p)|HCl(aq), 0.010 mol.kg-1|AgCl(s)|Ag For this cell the cell reaction is as follows: 2AgCl(s) + H2(g)  2Ag(s) + 2HCl(aq) (a) Give the electrode half-reactions and determine the standard cell potential.

Consider the reaction corresponding to a voltaic cell and its standard cell potential. Zn(s)+Cu2+(aq)⟶Cu(s) +Zn2+(aq)          Eocell=1.1032 V What is the cell potential for a cell with a 2.214 M solution of Zn2+(aq) and 0.1456 M solution of  Cu2+(aq) at 437.7 K?

The cell notation of a voltaic cell is: Zn(s) | Zn2+(aq; 0.02M) || Zn2+(aq; 1.0 M) | Zn (s) Draw a diagram of the cell and each half-reaction. Label the anode, cathode, and each relevant reaction. What is Eocell at equilibrium? Why? What is the expected Ecell at T = 273K? Given this Ecell, will the Q of this cell increase or decrease to reach equilibrium?

Consider the same diagram of a galvanic cell as in previous question, conventional current anode X X+ (aq) (C) 0.76 V (D) 0.91 V A e flow Salt bridge Y+ (aq) cathode where the half-cells are Ag|AgNO3(aq) and Ni|Ni(NO3)2(aq). Given the following electrode potentials: Ag (aq) + e-> Ag(s); E° = 0.80 V Ni²+ (aq) + 2e --> Ni(s): E = -0.23 V What is the Ecell at 25°C when the electrolyte concentrations are [Ag*] = 1.3 x 10-5 M and [Ni²+] = 0.10 M. (A) 1.15 V (B) 1.30 V

Calculate AG for the following cell reaction: Tl(s) | Tl+ (aq) || Ni²+ (aq) | Ni(s) From AG, determine the standard potential for the half-reaction Tl+ (aq) + e → Tl(s) AG; for Tl+ (aq) is -32.4 kJ/mol. 2+ AG; for Ni²+ (aq) is -45.60 kJ/mol. Standard Electrode (Reduction) Potentials in Aqueous Solution at 25°C Cathode (Reduction) Half-Reaction Ni²+ (aq) + 2e Ni(s) AG = J Standard Potential, E° (V) -0.23 Standard reduction potential for the half-reaction = V

Circle any of the following that would be classified as a heterocyclic amine. NH₂ NH₂ NH₂