1 Introduction To Chemistry 2 Atoms And Molecules 3 Molecules, Moles, And Chemical Equations 4 Stoichiometry 5 Gases 6 The Periodic Table And Atomic Structure 7 Chemical Bonding And Molecular Structure 8 Molecules And Materials 9 Energy And Chemistry 10 Entropy And The Second Law Of Thermodynamics 11 Chemical Kinetics 12 Chemical Equilibrium 13 Electrochemistry 14 Nuclear Chemistry Chapter13: Electrochemistry
Chapter Questions Section: Chapter Questions
Problem 1CO Problem 2CO Problem 3CO: • write and balance half-reactions for simple redox processes. Problem 4CO Problem 5CO Problem 6CO: • use standard reduction potentials to predict the spontaneous direction of a redox reaction. Problem 7CO: • calculate the amount of metal plated, the amount of current needed, or the time required for an... Problem 8CO Problem 9CO Problem 10CO Problem 13.1PAE Problem 13.2PAE Problem 13.3PAE Problem 13.4PAE Problem 13.5PAE: For the following oxidationreduction reactions, identify the half-reactions and label them as... Problem 13.6PAE Problem 13.7PAE Problem 13.8PAE: Which half-reaction takes place at the anode of an electrochemical cell? Which half-reaction takes... Problem 13.9PAE: If a salt bridge contains KNO3 as its electrolyte, which ions diffuse into solution in the anode... Problem 13.10PAE: If a salt bridge contains KNO3 as its electrolyte, which ions diffuse into solution in the cathode... Problem 13.11PAE: The following oxidationreduction reactions are used in electrochemical cells. Write them using cell... Problem 13.12PAE: Write a balanced chemical equation for the overall reaction in each of the following galvanic cells.... Problem 13.13PAE: For the reactions in parts (a) and (b) in the preceding problem, no anions at all are shown in the... Problem 13.14PAE: Explain why the terms cell potential and electromotive force mean the same thing in electrochemical... Problem 13.15PAE: How does galvanic corrosion differ from uniform corrosion of iron? Problem 13.16PAE Problem 13.17PAE: A student who has mercury amalgam fillings in some of her teeth is eating a piece of candy. She... Problem 13.18PAE: Based on the cell potential measured for the cells Co(s)|Co2+(aq) Cu 2+( aq)|Cu(... Problem 13.19PAE Problem 13.20PAE: Four voltaic cells are set up. In each, one half-cell contains a standard hydrogen electrode. The... Problem 13.21PAE Problem 13.22PAE: Explain why a large negative value for the standard reduction potential indicates a half-cell that... Problem 13.23PAE: In tables of standard reduction potentials that start from large positive values at the top and... Problem 13.24PAE: In the table of standard reduction potentials, locate the half-reactions for the reductions of the... Problem 13.25PAE: Using values from the table of standard reduction potentials, calculate the cell potentials of the... Problem 13.26PAE: Using values from the table of standard reduction potentials, calculate the cell potentials of the... Problem 13.27PAE: One half-cell in a voltaic cell is constructed from a copper wire dipped into a 4.8103 M solution of... Problem 13.28PAE: Four metals, A, B, C, and D, exhibit the following properties. (i) Only A and C react with 1.0 M... Problem 13.29PAE: Use the Nernst equation to calculate the cell potentials of the following cells at 298 K. (a)... Problem 13.30PAE: One half-cell in a voltaic cell is constructed from a silver wire dipped into a AgNO3 solution of... Problem 13.31PAE: We noted that a tin-plated steel can corrodes more quickly than an unplated steel can. In cases of... Problem 13.32PAE: The following half-cells are available: Ag(s);... Problem 13.33PAE Problem 13.34PAE Problem 13.35PAE: In May 2000, a concrete pedestrian walkway collapsed in North Carolina, injuring more than 100... Problem 13.36PAE Problem 13.37PAE Problem 13.38PAE Problem 13.39PAE: Calculate the standard free energy change for the following reactions using the standard cell... Problem 13.40PAE: Suppose that you cannot find a table of standard reduction potentials. You remember that the... Problem 13.41PAE Problem 13.42PAE: Which of the following reactions is (are) spontaneous at standard conditions? (a)... Problem 13.43PAE: Consult a table of standard reduction potentials and determine which of the following reactions are... Problem 13.44PAE: The equilibrium constant for a reaction is 31015 (a) Without carrying out any calculation, discuss... Problem 13.45PAE: Some calculators cannot display results of an antilog calculation if the power of 10 is greater than... Problem 13.46PAE: Calculate the equilibrium constant for the following reactions using data from the standard... Problem 13.47PAE: Use the standard reduction potentials for the reactions: AgCl(s)+eAg(s)+Cl-(aq) and Ag+(aq)+eAg(s)... Problem 13.48PAE: Hydrogen peroxide is often stored in the refrigerator to help keep it from decomposing according to... Problem 13.49PAE: Calculate the equilibrium constant for the redox reactions that could occur in the following... Problem 13.50PAE Problem 13.51PAE: An engineer is assigned to design an electrochemical cell that will deliver a potential of exactly... Problem 13.52PAE: A magnesium bar with a mass of 6.0 kg is attached to a buried iron pipe to serve as a sacrificial... Problem 13.53PAE Problem 13.54PAE Problem 13.55PAE Problem 13.56PAE Problem 13.57PAE Problem 13.58PAE: If you put a 9-volt battery in a smoke detector in your home or apartment, you are not installing a... Problem 13.59PAE: If alkaline batteries were not alkaline but rather acidic (as in the older dry cell batteries), what... Problem 13.60PAE: What would happen to the voltage of an alkaline battery if the zinc were replaced by steel? Assume... Problem 13.61PAE: Battery manufacturers often assess batteries in terms of their specific energy (or energy capacity).... Problem 13.62PAE Problem 13.63PAE: What product forms from the lead components of a lead storage battery? Why does mechanical shock... Problem 13.64PAE Problem 13.65PAE Problem 13.66PAE: Assume the specifications of a Ni-Cd voltaic cell include delivery of 0.25 A of current for 1.00 h.... Problem 13.67PAE Problem 13.68PAE: What is the difference between active and passive electrolysis? Based on the common meanings of the... Problem 13.69PAE Problem 13.70PAE Problem 13.71PAE Problem 13.72PAE Problem 13.73PAE: In an electroplating operation, the cell potential is sometimes 0 V. Why is a zero potential... Problem 13.74PAE Problem 13.75PAE Problem 13.76PAE Problem 13.77PAE: Use the Internet to find electroplating companies that carry out silver plating. Popular impressions... Problem 13.78PAE Problem 13.79PAE: If a current of 15 A is run through an electrolysis cell for 2.0 hours, how many moles of electrons... Problem 13.80PAE: Suppose somebody in a laboratory doesn't quite turn off the current in an electrolysis cell so that... Problem 13.81PAE: If a barrel plating run uses 200.0 A for exactly 6 hours for an electroplating application at 0.30... Problem 13.82PAE: An electrical engineer is analyzing an electroplating run and wants to calculate the charge that has... Problem 13.83PAE: In a copper plating experiment in which copper metal is deposited from a copper(ll) ion solution,... Problem 13.84PAE: A metallurgist wants to gold-plate a thin sheet with the following dimensions: 1.5in8.5in0.0012in .... Problem 13.85PAE: Tin-plated steel is used for "tin" cans. Suppose that in the production of sheets of tin-plated... Problem 13.86PAE: An electrolysis cell for aluminum production operates at 5.0 V and a current of 1.0105 A. Calculate... Problem 13.87PAE: If a plating line that deposits nickel (from NiCl2 solutions) operates at a voltage of 0.40 V with a... Problem 13.88PAE Problem 13.89PAE Problem 13.90PAE: A small part with a surface area of 2.62 cm2 is plated with a gold coating that is 5.00104 mm thick.... Problem 13.91PAE: An engineer is designing a mirror for an optical system. A piece of metal that measures 1.3 cm by... Problem 13.92PAE Problem 13.93PAE Problem 13.94PAE: What characteristic of lithium ions makes it practical to build a semipermeable separator that... Problem 13.95PAE: Looking at Figure 13.23, describe how the operation of a lithium-ion battery does not lead to a... Problem 13.96PAE Problem 13.97PAE: For a voltage-sensitive application, you are working on a battery that must have a working voltage... Problem 13.98PAE Problem 13.99PAE Problem 13.100PAE Problem 13.101PAE Problem 13.102PAE: 13.104 (a) What happens when a current is passed through a solution of dilute sulfuric acid to carry... Problem 13.103PAE: A current is passed through a solution of copper(II) sulfate long enough to deposit 14.5 g of... Problem 13.104PAE: 13.106 Hydrazine, N2H4 , has been proposed as the fuel in a fuel cell in which oxygen is the... Problem 13.105PAE Problem 13.62PAE
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Discuss the chemical reactions involves in this experiment.
Transcribed Image Text: EXPERIMENT : BATTERY FROM CITRUS FRUITS
МЕТНODS
1. Carefully clean your zinc and copper electrodes to remove any dirt or grease (Do
not scrub all of the zinc coating off the galvanized nails).
2. Roll and squeeze the lemons to release the juice and pulp inside.
3. Insert one galvanized nail and one piece of copper coins into each lemon.
4. Connect the ends of one wire to a galvanized nail in one lemon and then to a piece
of copper coins in another lemon. Repeat this procedure with each of the
remaining lemons until all of them are connected. When you are finished, you
should have one nail and one piece of copper coin unattached.
5. Connect the unattached piece of copper (positive) and the unattached nail
(negative) to the LED.
i)
ii)
Gently bend the lead wires of the LED apart from each other.
Connect a lead wire from the copper electrode of the first lemon cell to the
longer lead wire from the LED.
iii)
Connect a lead wire from the zinc electrode of the third cell to the shorter
wire of the LED.
6. Turn on your light and record how long can this battery light up the LED.
7. Repeat all the procedures (Step 1-5) using calamansis and oranges and compare
the results of all the citrus fruits.
Definition Definition Transformation of a chemical species into another chemical species. A chemical reaction consists of breaking existing bonds and forming new ones by changing the position of electrons. These reactions are best explained using a chemical equation.
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Step 2 Reactions is fruit battery
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