21.30 Consider the following voltaic cell: Voltmeter Zn Co Salt bridge 1 M Co2+ (a) In which direction do electrons flow in the external circuit? (b) In which half-cell does reduction occur? (c) In which half-cell do electrons leave the cell? (d) At which electrode are electrons generated? (e) Which electrode is positively charged?

Given the following data, answer the following questions: Fe2+(aq) + 2e- → Fe(s) E○red = -0.44 v, Cr3+(aq) + e- → Cr2+(aq) E○red = -0.407 v (a) What is the spontaneous cell reaction when a voltaic cell is constructed using these two half- reactions? (b) What is the E○ for the reaction?(c) What is equilibrium constant and deltaG?(d) If the concentration of Cr3+ and Cr2+ are each 0.10 M and the cell potential is 0.100 v, what is the concentration of Fe2+?(e) What is E for the reaction at equilibrium?

Consider the galvanic cell based on the following half-reactions. Ag+ + e → Ag Cd²+ + 2e →→ Cd (a) Determine the overall cell reaction and calculate º chemPad XX² cell 8° = +0.80 V 8⁰ = -0.40 V V AGO K Help Greek (b) Calculate AGº (in kJ) and K for the cell reaction at 25°C. kJ (in V). (Use the lowest possible whole number coefficients. Omit states-of-matter from your answer.) cell (c) Calculate cell (in V) at 25°C when [Ag+ ] = V 1.0×10-4 M and [Cd²+] = 1.0×10-² M.

Consider the following line notation:       Cu(s)│Cu(NO3)2 (aq) (0.00678 M)║ Al(NO3)3 (aq) (0.00345M)│Al(s)         Calculate E for this electrochemical cell set up ignoring activity coefficients.  Recalculate E for the electrochemical cell with activity coefficients. (

A voltaic cell operating under standard conditions (1.0 M ion concentrations) utilizes the following reaction: What is the effect on the cell emf of each of the following changes? (a) Water is added to the anode compartment, diluting the solution. O The positive cell emf rises, becoming more positive. O The positive cell emf drops closer to zero. O The negative cell emf rises closer to zero. O The negative cell emf drops, becoming more negative. No change in cell emf occurs. (b) The size of the chromium electrode is increased. The positive cell emf rises, becoming more positive. O The positive cell emf drops closer to zero. O The negative cell emf rises closer to zero. O The negative cell emf drops, becoming more negative. O No change in cell emf occurs. x (c) A solution of 1.0 M CrCl3 is added to the anode compartment. The positive cell emf rises, becoming more positive. O The positive cell emf drops closer to zero. O The negative cell emf rises closer to zero. O The negative cell emf…

Predict the potential for the following voltaic cell at 25 C:Cu(s)|CuSO4(1.29 M)||AgNO3(0.7 M)|Ag(s)

a) Balance the following redox reaction in basic solution: H2O2(aq) + ClO2(aq) → ClO2-(aq) + O2(g) b) Sketch the voltaic cell for the redox reaction, labeling the direction for electron flow, the anode and cathode , and the species present in each half-cell. Show all the work please!

19.37