Explanation When an atom loses electrons, it undergoes oxidation and has an increase in its oxidation state, which is an increase in the charge. The reverse is true for a reduction, where reduction is when an atom gains electrons and has a decrease in oxidation state which decreases the charge on the atom. To properly balance a redox reaction , you must balance both number of atoms on each side of the reaction and the charge. Therefore, we use something called the half-reaction method of balancing which is described below: A l ( s ) + C u 2 + ( a q ) → A l 3 + ( a q ) + C u ( s ) First you can assign oxidation states to each atom to find which atoms are being oxidized and reduced. We can see that Al goes from a charge of 0 to 3+, therefore, it is being oxidized. The Cu goes from 2+ to 0, which is a reduction. So, now we separate the two processes into two half reactions: Oxidation: A l → A l 3 + Reduction: C u 2 + → C u Now, we need to balance the atoms of each half reaction, but in this case they are already balanced

Chemistry: Structure and Properties Plus MasteringChemistry with eText -- Access Card Package

1st Edition

ISBN: 9780321729736

Author: Nivaldo J. Tro

Publisher: PEARSON

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Redox Reactions

Redox reactions are considered to be the chemical reactions involving both oxidation and reduction processes. They are actually oxidation-reduction reactions. The term redox is made from two words where “red” comes from reduction and “ox” comes from oxid…

Question

Chapter 20, Problem 1E

Interpretation Introduction

To determine: Define oxidation and reduction and the basic procedure for balancing redox reactions.

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Chapter 20 Solutions

Chemistry: Structure and Properties Plus MasteringChemistry with eText -- Access Card Package

Ch. 20 - Balance the redox reaction equation (occurring in...Ch. 20 - Prob. 2SAQ Ch. 20 - Prob. 3SAQ Ch. 20 - Refer to Table 19.1 to determine which statement...Ch. 20 - Prob. 5SAQ Ch. 20 - The Zn/Zn2+ electrode has a standard electrode...Ch. 20 - Refer to Table 19.1 to calculate G for the...Ch. 20 - A redox reaction has an Ecell=0.56V . What can you...Ch. 20 - Prob. 9SAQ Ch. 20 - Prob. 10SAQ

Ch. 20 - Prob. 11SAQ Ch. 20 - Prob. 12SAQ Ch. 20 - Which reaction occurs at the cathode of an...Ch. 20 - Copper is plated onto the cathode of an...Ch. 20 - Prob. 15SAQ Ch. 20 - Prob. 1E Ch. 20 - Explain the difference between a voltaic (or...Ch. 20 - Prob. 3E Ch. 20 - Prob. 4E Ch. 20 - Prob. 5E Ch. 20 - Prob. 6E Ch. 20 - What is the definition of the standard cell...Ch. 20 - Describe the basic features of a cell diagram (or...Ch. 20 - Why do some electrochemical cells employ inert...Ch. 20 - Describe the standard hydrogen electrode (SHE) and...Ch. 20 - How is the cell potential of an electrochemical...Ch. 20 - Prob. 12E Ch. 20 - Prob. 13E Ch. 20 - How can Table 19.1be used to predict whether or...Ch. 20 - Explain why Ecell , Grxn , and K are all...Ch. 20 - Does a redox reaction with a small equilibrium...Ch. 20 - How does Ecell depend on the concentrations of the...Ch. 20 - Prob. 18E Ch. 20 - What is a concentration electrochemical cell?Ch. 20 - What are the anode and cathode reactions in a...Ch. 20 - What are the anode and cathode reactions in a...Ch. 20 - Prob. 22E Ch. 20 - What is a fuel cell? What is the most common type...Ch. 20 - The anode of an electrolytic cell must be...Ch. 20 - What species is oxidized, and what species is...Ch. 20 - If an electrolytic cell contains a mixture of...Ch. 20 - Why does the electrolysis of an aqueous sodium...Ch. 20 - What is overvoltage in an electrochemical cell?...Ch. 20 - How is the amount of current flowing through an...Ch. 20 - Prob. 30E Ch. 20 - Prob. 31E Ch. 20 - Prob. 32E Ch. 20 - Balance each redox reaction occurring in acidic...Ch. 20 - Prob. 34E Ch. 20 - Balance each redox reaction occurring in acidic...Ch. 20 - Prob. 36E Ch. 20 - Prob. 37E Ch. 20 - Balance each redox reaction occurring in basic...Ch. 20 - Prob. 39E Ch. 20 - Prob. 40E Ch. 20 - Calculate the standard cell potential for each of...Ch. 20 - Prob. 42E Ch. 20 - Consider the voltaic cell: Determine the direction...Ch. 20 - Prob. 44E Ch. 20 - Use line notation to represent each...Ch. 20 - Use line notation to represent each...Ch. 20 - a sketch of the voltaic cell represented by the...Ch. 20 - Prob. 48E Ch. 20 - Determine whether or not each redox reaction...Ch. 20 - Prob. 50E Ch. 20 - Which metal could you use to reduce Mn2+ ions but...Ch. 20 - Prob. 52E Ch. 20 - Prob. 53E Ch. 20 - Prob. 54E Ch. 20 - Prob. 55E Ch. 20 - Prob. 56E Ch. 20 - Calculate Ecell for each balanced redox reaction...Ch. 20 - Prob. 58E Ch. 20 - Prob. 59E Ch. 20 - Which metal is the best reducing agent? Mn Al Ni...Ch. 20 - Use tabulated electrode potentials to calculate...Ch. 20 - Use tabulated electrode potentials to calculate...Ch. 20 - Prob. 63E Ch. 20 - Calculate the equilibrium constant for each of the...Ch. 20 - Calculate the equilibrium constant for the...Ch. 20 - Prob. 66E Ch. 20 - Calculate Grxn and Ecell for a redox reaction with...Ch. 20 - Prob. 68E Ch. 20 - Prob. 69E Ch. 20 - Prob. 70E Ch. 20 - Prob. 71E Ch. 20 - Prob. 72E Ch. 20 - Prob. 73E Ch. 20 - Prob. 74E Ch. 20 - Prob. 75E Ch. 20 - Consider the concentration cell: Label the anode...Ch. 20 - Prob. 77E Ch. 20 - Prob. 78E Ch. 20 - Prob. 79E Ch. 20 - Prob. 80E Ch. 20 - Refer to the tabulated values of Gf in Appendix...Ch. 20 - Refer to the tabulated values of Gf in Appendix...Ch. 20 - Prob. 83E Ch. 20 - Prob. 84E Ch. 20 - Prob. 85E Ch. 20 - Prob. 86E Ch. 20 - Prob. 87E Ch. 20 - Which products are obtained in the electrolysis of...Ch. 20 - Write equations for the half-reactions that occur...Ch. 20 - Which products are obtained in the electrolysis of...Ch. 20 - Prob. 91E Ch. 20 - Write equations for the half-reactions that occur...Ch. 20 - Prob. 93E Ch. 20 - Prob. 94E Ch. 20 - Prob. 95E Ch. 20 - Silver can be electroplated at the cathode of an...Ch. 20 - A major source of sodium metal is the electrolysis...Ch. 20 - Prob. 98E Ch. 20 - Prob. 99E Ch. 20 - Prob. 100E Ch. 20 - Consider the molecular view of an AL strip and...Ch. 20 - Consider the molecular view of an electrochemical...Ch. 20 - Prob. 103E Ch. 20 - Prob. 104E Ch. 20 - The cell potential of this electrochemical cell...Ch. 20 - Prob. 106E Ch. 20 - Prob. 107E Ch. 20 - What voltage can theoretically be achieved in a...Ch. 20 - A battery relies on the oxidation of magnesium and...Ch. 20 - A rechargeable battery is constructed based on a...Ch. 20 - If a water electrolysis cell operates at a current...Ch. 20 - Prob. 112E Ch. 20 - Prob. 113E Ch. 20 - Prob. 114E Ch. 20 - Calculate Grxn and K for each reaction. The...Ch. 20 - Calculate Grxn and K for each reaction. The...Ch. 20 - The molar mass of a metal (M) is 50.9 g/mol; it...Ch. 20 - A metal forms the fluoride MF3. Electrolysis of...Ch. 20 - A sample of impure tin of mass 0.535 g is...Ch. 20 - Prob. 120E Ch. 20 - Prob. 121E Ch. 20 - A 215 mL sample of a 0.500 M NaCl solution with an...Ch. 20 - Prob. 123E Ch. 20 - Prob. 124E Ch. 20 - Prob. 125E Ch. 20 - Prob. 126E Ch. 20 - Prob. 127E Ch. 20 - Prob. 128E Ch. 20 - Prob. 129E Ch. 20 - Three electrolytic cells are connected in a...Ch. 20 - Prob. 131E Ch. 20 - Prob. 132E Ch. 20 - Prob. 133E Ch. 20 - Prob. 134E Ch. 20 - Prob. 135E

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