i)
Hg/Hg2+(aq,0.020M) is anode
ii)
E°cell = E°red,cathode- E°red,anode
= + 0.770V - (+0.850V)
= - 0.080V
iii)
Oxidation half reaction
Hg(s) -------> Hg2+(aq) + 2e
Reduction half reaction
2Fe3+(aq) + 2e --------> 2Fe2+(aq)
Overall reaction
Hg(s) + 2Fe3+(aq) -------> 2Fe2+(aq) + Hg2+(aq)
Q= [Hg2+][Fe2+]2/[Fe3+]2
Q =( (0.020M)(0.00001M)2)/(0.50M)2
Q= 8.0×10-12
Number of electron transfer,n = 2
iv)
Nernst equation at 298.15K is as follows
Ecell = E°cell - (0.0592V/n)logQ
= -0.080V - (0.0592V/2)log(8.0×10-12)
= -0.080V + 0.328V
= 0.248V
79. Two half-cells, PtlFe3+(aq, 0.50 M), Fe2 +(aq, 1.0 x 10-5 M) and Hg (aq, 0.020...
Section 16.5: Voltaic Cells under Non-standard Conditions 16.64 The half-cells Fe2+ (aq, 0.024 mol L-'Fe(s) and H(aq, 0.056 mol L-)H2(1.0 bar) are linked by a salt bridge to create a voltaic cell. Determine the cell emf (Ecell) at 298 K.
question 16.46 UU 15 - UU UL ut tu uve- 16.46 The half-cells Fe2+ (aq)|Fe(s) and O2(g)|H2O (in acid solution) are linked to create a voltaic cell. (a) Write equations for the oxidation and reduction half- reactions and for the overall cell reaction. (b) Which half-reaction occurs in the anode compart- ment and which occurs in the cathode compartment? (c) Complete the following sentences: Electrons in the external circuit flow from the — electrode to the electrode. Negative ions move...
19 20 Question 16 Half-cell Potentials: Half Reaction: E' value + 0.80 V +0.77 V Agte → AS Fe3+ + + Fe2+ Cu2+ 2e → Cu Pb2+ + 2e → Pb +0.34 V -0.13 V Ni2+ + 2e → NI -0.25 V - 0.40 V Cd2+ +2e → ca Fe2+ + 2e → Fe Zn2+ + 2e → Zn -0.44 V - 0.76 V A13+ +3 → AI - 1.66 V Consider an electrochemical cell constructed from the following half...
2. A standard state galvanic cell is constructed using the following half-reactions. Fe3+ (aq) + Fe2(aq) Fe2(aq) + 2e → Fe(s) a. Fill in the cell diagram. Label the anode, cathode, the reactants and products in each solu direction of electron flow through the wire, and ion flow through the salt bridge. (5 pts) KNO, Salt Bridge (+) electrode (-) electrode b. Calculate the concentration of each ion in the cell at equilibrium. (10 pts)
The following half-cells are availble: (i) Ag+ (1.0 M) ∣ Ag (s) 0.7994 v (ii) Zn2+ (1.0 M) ∣ Zn (s) -0.76 v (iii) Cu2+ (1.0 M) ∣ Cu (s) 0.337 v (iv) Co2+ (1.0 M) ∣ Co (s) -0.28 v Linking any two half-cells makes a voltaic cell. Given four different half-cells, six voltaic cells are possible. These are labeled, for simplicity, Ag - Zn, Ag-Cu, Ag-Co, Zn - Cu, Zn-Co, and Cu-Co. (the first metal is the anode...
a.) A voltaic cell is constructed in which the cathode is a standard hydrogen electrode and the anode is a hydrogen electrode (P(H2) = 1 atm) immersed in a solution of unknown [H+]. If the cell potential is 0.204 V, what is the pH of the unknown solution at 298 K? b.) An electrochemical cell is constructed in which a Cr3+(1.00 M)|Cr(s) half-cell is connected to an H3O+(aq)|H2(1 atm) half-cell with unknown H3O+ concentration. The measured cell voltage is 0.366...
let me know the one has (aq) (s) (l) or (g) Enter electrons as e half cell and the cathode is a C A voltaic cell is constructed in which the anode is a Ma Min bridge. h alf cell. The half-cell compartments are connected by a salt (Use the lowest possible coefficients. Use the pull-down boxes to specify states such as (aq) or(s). If a box is not needed, leave it blank.) The anode reaction is: The cathode reaction...
For a voltaic (or galvanic) cell using Ag, Ag+ (1.0M) and Zn Zn2+ (1.0 M) half-cells, which of the following statements is incorrect? (a) The zinc electrode is the anode. (b) Electrons will flow through the external circuit from the zinc electrode to the silver electrode. (c) The mass of the zinc electrode will decrease as the cell operates. (d) The concentration of Ag will decrease as the cell operates. (e) Reduction occurs at the zinc electrode as the cell operates.
Consider an electrochemical cell constructed from the following half cells, linked by a KCl salt bridge. a Fe electrode in 1.0 M FeCl2 solution a Sn electrode in 1.0 M Sn(NO3)2 solution Fe2+ + 2e- → Fe Eo = -0.44 V Sn2+ + 2e- → Sn Eo = -0.14 V When the cell is running spontaneously, which choice includes only true statements and no false ones? Select one: a. The iron electrode gains mass and the iron electrode is the...
The following half-cells are availble: (i) Agt (1.0 M) TAg (s) (ii) Zn2+ (1.0 M) | Zn (s) (iii) Cu2+(1.0 M) Cu(s) (iv) Co2+ (1.0 M) Co (s) 0.7994 v -0.76 v 0.337 v -0.28 v Linking any two half cells makes a voltaic cell. Given four different half-cells, six voltaic cells are possible. These are labeled, for simplicity, Ag - Zn, Ag-Cu, Ag-Co, Zn-Cu, Zn-Co, and Cu-Co. (the first metal is the anode and the second is the cathode.)...