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Questions and Answers
What is the final balanced reaction for the reduction of nitrate in alkaline conditions?
What is the final balanced reaction for the reduction of nitrate in alkaline conditions?
In the first half-reaction for the oxidation of zinc, which is the correct balanced equation?
In the first half-reaction for the oxidation of zinc, which is the correct balanced equation?
Which species is being reduced in the given chemical reaction?
Which species is being reduced in the given chemical reaction?
What is the role of electrons in the two half-reactions presented?
What is the role of electrons in the two half-reactions presented?
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How many hydroxide ions are consumed in the final balanced reaction?
How many hydroxide ions are consumed in the final balanced reaction?
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Which of the following steps correctly balances hydrogen in the half-reaction involving nitrate?
Which of the following steps correctly balances hydrogen in the half-reaction involving nitrate?
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What is the total charge on the left-hand side of the reaction after balancing it with hydroxide ions?
What is the total charge on the left-hand side of the reaction after balancing it with hydroxide ions?
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In the context of the overall reaction, what occurs to the water molecules after all balancing is completed?
In the context of the overall reaction, what occurs to the water molecules after all balancing is completed?
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Which step involves converting the reaction from acidic to basic conditions?
Which step involves converting the reaction from acidic to basic conditions?
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When balancing elements other than hydrogen and oxygen, which of the following methods is NOT used?
When balancing elements other than hydrogen and oxygen, which of the following methods is NOT used?
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Study Notes
Identifying Oxidation and Reduction Species
- The species being oxidized is the species that loses electrons - the Zn becomes Zn(OH)42-
- The species being reduced is the species that gains electrons - the NO3- becomes NH3
Balancing the Chemical Equation
- The first step is to write two skeletal half-reactions.
- Balance all elements except H and charge by inspection.
- Balance oxygen by adding water molecules to the side that needs more oxygen.
- Balance hydrogen by adding H+ ions to the side that needs more hydrogen.
- Convert the acidic half-reactions to basic. Add enough OH- ions to each side of the equation to neutralize all of the H+ ions.
- Combine H+ and OH- ions to form water molecules and place the water molecules on one side of the equation.
- Balance the charge by adding electrons to the appropriate side of each half-reaction.
- Multiply the half-reactions by the appropriate factors to ensure that the number of electrons lost in the oxidation half-reaction equals the number of electrons gained in the reduction half-reaction.
- Combine the two half-reactions, canceling out any common species on both sides of the equation.
Checking the Balanced Equation
- Ensure that the number of atoms of each element is the same on both sides of the equation.
- Ensure that the total charge on both sides of the equation is the same.
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Description
Explore the concepts of oxidation and reduction through a detailed quiz. Learn to identify oxidized and reduced species and master the techniques for balancing chemical equations. Test your understanding with practical examples and clarify your chemistry knowledge.
