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(4 points) A simple battery is constructed using zinc and copper as electrodes. The chemical equation...
equation in graph: E=1.13E+00-1.08E-04T 8. (10 pts) A cell is constructed Cu2+ to Cu, while the zinc is oxidized from Zn to Zn+. The cell potential is measured as temperature, yielding the graph below. with a copper anode and a zinc cathode. The copper is reduced from 1 3E-00-1.08E-04 T e» 1 8 280 290 300 310 320 330 340 350 Determine Δrrn // and ΔrrnS for this reaction from the data given. 8. (10 pts) A cell is constructed...
It is expected that a chemical reaction will occur when copper metal is combined with aqueous zinc sulfate. Explain why there will be no reaction when zinc metal and aqueous copper sulfate solution are combined. Identify the anode and the cathode, assuming a voltaic cell is constructed. Note: Be careful in the calculation of the standard cell potential ( Eo cathode - Eo anode). Do not change the sign of the given reduction potential. The sign is already taken care...
how would you go about solving this problem via using equations just looking for the equation order i should go about solving this problem In this experiment you will be using the two half reactions Cu?"/Cu and Zn2 /Zn. The standard electrode potential, E°, for these half reactions is +0.34V and-0.76V respectively, so the Nernst Equation for these half reactions is the following Cu ea)+2e - Cus) E - 0.34V 0.0592V Cu2+] 0.0592V Zn 2 Note that solids by definition...
A zinc air battery has the following reactions at the two electrodes: 1⁄2 O2 + H2O + 2e- -> 2OH- Zn -> Zn2+ +2e- Zn&2+ + 2OH- -> Zn(OH)^2 a) Which of these reactions occurs at the anode and which at the cathode? Explain your answer. b) Determine the two half-cell potentials at the electrode-electrolyte interfaces using standard Gibbs free energy values (Note: Assume the phase of the Zn(OH)2 is the epsilon phase.) c) A zinc air battery is typically...
What is the reduction half-reaction? In the electrolytic cell of this experiment, copper metal is the anode and zinc metal the cathode. The electrolyte solution is sulfuric acid, H2SO4. Oxidation occurs at the copper anode, where Cu is oxidized to Cu^2+: Cu (s) → Cu^2+ (aq) + 2 e– During the experiment, you might have noticed that at the end of the trials, the solution becomes slightly blue, which proves the existence of aqueous Cu^2+. What is the reduction half-reaction...
1. Write a balanced chemical equation for the oxidation of zinc metal (Zn) by copper(II) ions (Cu?") in a copper sulfate solution. Note that copper(II) sulfate completely dissociates in aqueous solution and forms Cu2+ (aq) and SO,- (aq) in water. Zinc metal is a solid and should be represented as Zn (3) Write a chemical equation for the decomposition of limestone (CaCO,) by heating to high temperature to drive off carbon dioxide. The other product of this decomposition reaction is...
Name: Recitation Day, Time: CHM 116 Recitation #12 1. A working voltaic cell is constructed with copper and silver. The solutions are Cu(NO,) and AgNO, Silver is identified to be the cathode. Answer the following questions Voltmeter At NO 3 An ode Cath ode In the diagram above, a) Label the cathode and anode. b) On the two metal bars above, show where Cu and Ag would be placed. c) In the two beakers above, show where solutions of Cu(Nos)2...
In a copper-zinc voltaic cell, one half-cell consists of a ZnZn electrode inserted in a solution of zinc sulfate and the other half-cell consists of a CuCu electrode inserted in a copper sulfate solution. These two half-cells are separated by a salt bridge. At the zinc electrode (anode), ZnZn metal undergoes oxidation by losing two electrons and enters the solution as Zn2+Zn2+ ions. The oxidation half-cell reaction that takes place at the anode is Zn(s)→Zn2+(aq)+2e−Zn(s)→Zn2+(aq)+2e− The CuCu ions undergo reduction...
The following data were measured using a nickel electrode as the standard: Cu2+(aq) + 2e- ⟶ Cu(s) Ni2+(aq) + 2e- ⟶ Ni(s) Fe2+(aq) + 2e- ⟶ Fe(s) Al3+(aq) + 3e- ⟶ Al(s) The copper and aluminum electrodes are connected in a battery. A) Which is the anode? Cathode? Why? B) Which is oxidized? Reduced? Why? C) What will the battery voltage be? Eo =0.62V Eo =0.00V Eo =-0.15V Eo =-1.38V D) Write a balanced net ionic equation for the reaction...
A Cu-Zn voltaic cell based on the reaction in the equation given below. Zn(s)+Cu2+(aq)àZn2+(aq)+Cu(s) Which metal is oxidized in this voltaic cell? A. Copper B. Zinc