Interpretation:
The balanced equation for the
Concept introduction:
The oxidizer is the species whose oxidation state decreases during the course of reaction and reducer is the species whose oxidation number increases. Oxidized product is the oxidation product of the reducer and reduced product is the reduction product of the oxidizer.
Answer to Problem 28E
The balanced equation for the redox reaction
Explanation of Solution
The given redox reaction is shown below.
The oxidation state of the central metal atom is calculated by knowing the standard oxidation states of few elements.
The oxidation state of the chlorine in
Step-1: Write down the oxidation number of every element and for unknown take “n”.
Step-2: Multiply the oxidation state with their number of atoms of an element.
Step-3: Add the oxidation numbers and set them equal to the charge of the species.
Calculate the value of n by simplifying the equation as shown below.
The oxidation state of chlorine is
The oxidation number of chlorine is
The oxidation number of chlorine is zero in
The chlorine is reduced on going from
The chlorine is oxidized on going from
The reduction half-reaction for the above reaction is shown below.
The balancing of the half-reactions is done by the following the steps shown below.
Step-1: Identify and balance the element getting oxidized or reduced.
The chlorine is getting reduced and its number of atoms is not balanced on both sides. Balance them by multiplying the
Step-2: Balance elements other than oxygen and hydrogen if any.
Step-3: Balance oxygen atoms by adding water on the appropriate side.
Step-4: Balance the hydrogen atoms by adding
Step-5: Balance the charge by adding electrons to the appropriate side.
The charge is balanced by adding two electrons on the left-hand side of the equation.
Step-6: Recheck the equation to be sure that it is perfectly balanced.
The equation is completely balanced and is shown below.
The oxidation half-reaction for the above reaction is shown below.
The balancing of the half-reactions is done by the following the steps shown below.
Step-1: Identify and balance the element getting oxidized or reduced.
The chlorine is getting oxidized and its number of atoms is not balanced on both sides. Balance them by multiplying
Step-2: Balance elements other than oxygen and hydrogen if any.
Step-3: Balance oxygen atoms by adding water on the appropriate side.
Add four water molecules on the left-hand side of the equation.
Step-4: Balance the hydrogen atoms by adding
To balance hydrogen atoms add eight
Step-5: Balance the charge by adding electrons to the appropriate side.
The charge is balanced by adding two electrons on the right-hand side of the equation.
Step-6: Neutralize all the
Four hydroxide ions are added to both sides of the equation.
Simplify the above equation by making the water of neutralized protons and balance out water molecules.
Step-7: Recheck the equation to be sure that it is perfectly balanced.
The equation is completely balanced and is shown below.
The balanced redox equation is obtained by adding equation (1) and (2) in such a way that electrons are canceled out.
Multiply equation (1) by three and then add to equation (2)
The equation obtained after adding these equations is shown below.
Divide whole equation by two to eliminate the common factor.
The equation is now completely balanced equation.
The
Want to see more full solutions like this?
Chapter 17 Solutions
Introductory Chemistry: Concepts and Critical Thinking (8th Edition)
- Gold can be dissolved from gold-bearing rock by treating the rock with sodium cyanide in the presence of oxygen. 4 Au(s) + 8 NaCN(aq) + O2(g) + 2 H2O() 4 NaAu(CN)2(aq) + 4 NaOH(aq) (a) Name the oxidizing and reducing agents in this reaction. What has been oxidized, and what has been reduced? (b) If you have exactly one metric ton (1 metric ton = 1000 kg) of gold-bearing rock, what volume of 0.075 M NaCN, in liters, do you need to extract the gold if the rock is 0.019% gold?arrow_forwardWrite balanced net ionic equations for the following reactions in acid solution. (a) Liquid hydrazine reacts with an aqueous solution of sodium bromate. Nitrogen gas and bromide ions are formed. (b) Solid phosphorus (P4) reacts with an aqueous solution of nitrate to form nitrogen oxide gas and dihydrogen phosphate (H2PO4-) ions. (c) Aqueous solutions of potassium sulfite and potassium permanganate react. Sulfate and manganese(II) ions are formed.arrow_forwardBromine is obtained from sea water by the following redox reaction: Cl2(g) + 2 NaBr(aq) 2 NaCl(aq) + Br2() (a) What has been oxidized? What has been reduced? (b) Identify the oxidizing and reducing agents.arrow_forward
- 1. Sometimes a reaction can fall in more than one category. Into what category (or categories) does the reaction of Ba(OH)2(aq) + H+PO4(aq) fit? acid-base and oxidation-reduction oxidation-reduction acid-base and precipitation precipitationarrow_forwardWrite the net ionic equation for the reaction, if any, that occurs on mixing (a) solutions of sodium hydroxide and magnesium chloride. (b) solutions of sodium nitrate and magnesium bromide. (c) magnesium metal and a solution of hydrochloric acid to produce magnesium chloride and hydrogen. Magnesium metal reacting with HCl.arrow_forwardFour metals, A, B, C, and D, exhibit the following properties: (a) Only A and C react with 1.0 M hydrochloric acid to give H2(g). (b) When C is added to solutions of the ions of the other metals, metallic B, D, and A are formed. (c) Metal D reduces Bn+ to give metallic B and Dn+. Based on this information, arrange the four metals in order of increasing ability to act as reducing agents.arrow_forward
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningIntroduction to General, Organic and BiochemistryChemistryISBN:9781285869759Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar TorresPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
- Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage LearningChemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning