What condition must be met for a battery to be rechargeable? O The electrochemical reaction of the battery must be reversible. O Either its anode or its cathode must generate a gas as a result of the electrochemical reaction. O It must generate electricity via an acid-base reaction rather than via an oxidation-reduction reaction. O The battery must use liquid and aqueous solutions.

If the given statement is true, write T. Otherwise, write F and explain why it is false 1)An electrolytic cell is used to generate electricity from chemical reactions 2) The reactant and the product need to have equal concentrations for a chemical reaction to be in equilibrium.

The process of decomposition of an electrolyte by passing electric current through its solution is called as Electrochemical cell .a O Electrolysis .b O Electrolyte .c O Electrode .d O

06. Show Solutions

What are the products obtained by the electrolysis of a solution of aluminum chloride? Cl2(g), H2(g), OH"(aq) O H2(g), O2(g) Al(s), O2(g), H*(aq) O Al(s), Cl2(g)

A rod made of an unknown metal, M, is dipped into a solution containing both X2+ and Z2+ cations. q1: Will a reaction occur when the rod is dipped into the solution? And if so what solid will begin to form? q2: If you were to create a voltaic cell using M, which (single) metal would you put as the cathode and anode, respectively? q3: f Z is Zinc, identify metals X and M

Write your answer in the blank provided. Examine the following balanced half-reaction:  2H2O + CrO2 → CrO4 2- + 3e- + 4H+  1. Is this an oxidation or a reduction? 2. What element is oxidized or reduced?      Balance the following half-equation in acid. ClO3 - → Cl2 The above reaction occurs along with the reaction given above before Part 1 of this problem.  Write a balanced equation for the overall reaction that occurs.  What is the coefficient of water in the balanced overall equation? Which reactant is the oxidizing agent?

* The voltmeter is usually used to measure The electrical potential of the anode O The electrical potential of the cathode O The difference in electrical potential between the cathode and the anode O None of the above O

Using the table of half-reactions, write a balanced equation for a redox reaction where chlorine oxidies iron. Then write a balanced equation for a redox reaction where calcium reduces water to produce hydrogen gas.

The same amount of electricity (same number of moles of electrons) is used to carry out the electrolysis of PdCl2(aq) and AgN03(aq) solutions in separate cells. The masses of Pd and Ag produced were measured and compared. Which of the following is true about the mass Pd produced? A The mass of Pd produced is not related to the mass of Ag. B. The mass of Pd produced is approximately half that of Ag. C. The mass of Pd produced is approximately twice that of Ag. D. The mass of Pd produced is approximately the same as that of Ag.