1) Instead of using zinc, a student accidentally used a 1 M solution of silver (Ag). Based on the information in the table below, what would be the theoretical cell voltage, Eocell, when it is used in a galvanic cell with copper? |
now new reaction which will occur
2Ag+(aq) + 2e = 2Ag(s) E*= 0.80 V
Cu(s) = Cu2+(aq) + 2e E* = -0.34V
add both reactions
Cu(s) + 2Ag+(aq) = Cu2+(aq) + 2Ag(s)
E*(cell) = 0.80 + (-0.34)
= 0.46 V
any query please comment
if satisfied please rate it thnaks
1) Instead of using zinc, a student accidentally used a 1 M solution of silver (Ag)....
Instead of using zinc, a student accidentally used a 1 M solution of silver (Ag). Based on the information in the table below, what would be the theoretical cell voltage, Eocell, when it is used in a galvanic cell with copper? Electrode Eo Ag+ + e- à Ag +0.80 V Cu2+ + 2e- à Cu +0.34 V Pb2+ + 2e- à Pb -0.13 V Zn2+ + 2e- à Zn -0.76 V Al3+ + 3e- à Al -1.66 V
A galvanic cell is constructed using a zinc electrode immersed in a 1.0 M Zn2+ solution and a silver electrode immersed in a 1.0 M Ag+ solution. What is the overall equation for this cell?
Consider an electrochemical cell with a zinc electrode immersed in a solution of ZnT and in electrical contact with a silver electrode immersed in a solution of Ag. If the initial concentrations of Zinc and Silver ions are 0.0050 M and 16.00 M respectively, calculate +2 cell Consider an electrochemical cell with a zinc electrode immersed in a solution of ZnT and in electrical contact with a silver electrode immersed in a solution of Ag. If the initial concentrations of...
The silver oxide-zinc battery used in watches delivers a voltage of 1.60 V. Using this information and the balanced chemical equation, calculate the standard free energy change for the cell reaction at 25C. Balanced equation: Zn(s) + Ag2O(s) --> ZnO(s) + 2 Ag(s)
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.
can u answer the following questions? 4. Silver oxide is used in "button batteries to power electric watches and other trinkets. These batteries generate a potential of 1.55 V and consist of a Zn anode and a Ag20 cathode immersed in a concentrated solution of KOH. The cathode reaction is based on the reduction of Ag20 to Ag metal. At the anode, Zn is oxidized to solid Zn(OH)2. Write the net ionic balanced electrochemical cell reaction and calculate the value...
13. A zinc electrode is submerged in an acidic 0.40 M Zn? solution which is connected by a salt bridge to a 1.50 M Ag solution containing a silver electrode. Determine the initial voltage of the cell at 298K 32
A student accidentally used phthalic acid, which has 2 ioniozable protons instead of KHP as the primary standard. What effect would this have on the calculation for determining the molarity of the NaOH solution?
8 pts Question 5 The silver oxide-zinc battery used in watches delivers a voltage of 1.60 V. Using this information and the balanced chemical equation calculate the standard free energy change for the cell reaction at 25C. Balanced equation: Zn(s) + Ag2015) --> ZnO(s) + 2 Ag(s) 154) 154] 310 -310
5. A voltaic cell is constructed based on the oxidation of zinc metal and the reduction of silver (I) ions. Solutions of 1.00 M silver nitrate and zinc nitrate also were used. The anode is on the left, the cathode is on the right. Where does oxidation occur? 5. A voltaic cell is constructed based on the oxidation of zinc metal and the reduction of silver (I) ions. Solutions of 1.00 M silver nitrate and zinc nitrate also were used....