Interpretation:
The oxidizer and reducer with oxidized and reduced products are to be stated. The
Concept introduction:
The oxidizer is the species whose oxidation state falls 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 51E
The oxidizer is
The oxidation half-reaction equation is shown below.
The reduction half-reaction equation is shown below.
The balanced redox equation is shown below.
Explanation of Solution
The given redox reaction equation to be balanced 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 arsenic 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.
Divide the equation by two on both sides and simplify as shown below.
The oxidation state of arsenic in
The oxidation state of arsenic 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 arsenic in
The oxidation state of the nitrogen 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 nitrogen is
The oxidation number of nitrogen 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 nitrogen in
The nitrogen in
Therefore, the oxidizer is
The oxidation half-reaction equation for the above equation 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 arsenic is getting oxidized and the number of atoms of that is not balanced on both sides. Multiply
Step-2: Balance elements other than oxygen and hydrogen if any.
Step-3: Balance oxygen atoms by adding water on the appropriate side.
Oxygen atoms are balanced by adding five water molecule to the left-hand side of the equation.
Step-4: Balance the hydrogen atoms by adding
The number of hydrogen atoms is balanced by adding the ten
Step-5: Balance the charge by adding electrons to the appropriate side.
Six electrons are added to the right-hand side in order to balance the charge.
Step-6: Recheck the equation to be sure that it is perfectly balanced.
The equation is completely balanced and is shown below.
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 nitrogen is getting reduced and its number of atoms are balanced on both sides.
Step-2: Balance elements other than oxygen and hydrogen if any.
Step-3: Balance oxygen atoms by adding water on the appropriate side.
The number of oxygen atoms is balanced by adding two water molecules on the right-hand side of the equation.
Step-4: Balance the hydrogen atoms by adding
The number of hydrogen atoms is balanced by adding four
Step-5: Balance the charge by adding electrons to the appropriate side.
The charge is balanced by adding three 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 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 equation (2) by four in order to cancel out the number of electrons as shown below.
Add equation (3) and (1) to get a balanced redox equation as shown below.
The common things on both sides of the equation canceled out to give the balanced redox equation.
The balanced redox equation after adding these equations is shown below.
The oxidizer and reducer with oxidized and reduced products, oxidation and reduction half-reaction equations, and balanced redox equation are rightfully stated above.
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Chapter 19 Solutions
Introductory Chemistry: An Active Learning Approach
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