Electrochemical cell

It is given that the electrochemical cell is at 298K. At time zero [Zn 2+ ]= 1.0 x 10 ^-3 M and [Ag +] = 0.500 M. Calculate the molarities of zinc and silver ions after a current of 2.00 amperes flow for 20 hours. Please show step by step and the units you are using.

Simple multiple choice questions, general acid base n kinetics ???

Question 1 (0.8 points) N2O5 is classified as an acidic oxide because it: a. ) reacts with acids to produce a salt. b. ) is insoluble in water. c. ) reacts with water to produce OH-. d. ) gives a solution of nitric acid, HNO3, on dissolving. e. ) can act as a Lewis base by donating electron pairs. ________________________________________ Question 2 (0.8 points) Which of the following is a Lewis acid? a. ) NH3 b. ) F- c. ) H2O d. ) NH4+ e. ) BF3 ________________________________________ Question 3 (1.0 points) For the following: i) -OCl > -OClO > -OClO2 > -OClO3 ii) [H2SbO4]- > [H2AsO4]- > [H2PO4]- iii... click for more

electrolytic cell

During lab I made 4 cells using CuSO4(aq) solution 1. one with a Cu (s) electrode on the negative terminal, and Al(s) on the positive terminal.....nothing appeared to happen during this reaction 2. Cu (s) on negative, Ni (s) on positive....bubbles formed at the anode 3. Cu (s) on positive, Al (s) on negative..... Cu plated out onto Al cathode 4. Cu (s) on positive, Ni (s) on negative ....Cu plated onto Ni for each of these reactions I have to give half-reactions consistant with the observations, and then write the overall equation I know that this shouldn't be difficult, but I'm not sure what I'm doing, especially for the overall equation for the cells with Cu at the anode.... click for more

electrochemistry

I am trying to determine the separate half reactions and overall cell process for the following and need some help: a minature battery is composed of Zn and a paste of KOH, water, mercury (II) oxide, and mercury. Zinc and potassium hydroxide are consumed, mercury is deposited, and potassium zincate is formed. Also, what would be the notation for this cell? Thanks for helping!

Kinetics

Hemoglobin (Hb) molecules in blood bind oxygen and carry it to the cells, where it takes part in respiration. The first step in the binding of oxygen is first order in hemoglobin and first order in dissolved oxygen, with a rate constant of 4 x 10^7 L mol-1 S-1. Hb(aq) + O2(aq) ------------> (HbO2) (aq) How can I calculate the initial rate at which oxygen is bound to hemoglobin if the concentration of hemoglobin is 2 x 10 ^-9 Mol/L and that of oxygen is 5 x 10^-5 mol/L ?