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What is the balanced redox reaction between zinc and hydrochloric acid?
What is the balanced redox reaction between zinc and hydrochloric acid?
What is the fundamental type of chemical reaction where electrons are transferred between reactants?
What is the fundamental type of chemical reaction where electrons are transferred between reactants?
In the provided half-reactions, what is the product of Zn(s) oxidation?
In the provided half-reactions, what is the product of Zn(s) oxidation?
In a redox reaction, which reactant undergoes oxidation?
In a redox reaction, which reactant undergoes oxidation?
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What does the reduction of hydrogen ions produce in this redox reaction?
What does the reduction of hydrogen ions produce in this redox reaction?
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What is a half-reaction in the context of redox chemistry?
What is a half-reaction in the context of redox chemistry?
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What is the purpose of balancing electrons in redox reactions?
What is the purpose of balancing electrons in redox reactions?
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How should you balance the overall redox equation to ensure conservation of mass and charge?
How should you balance the overall redox equation to ensure conservation of mass and charge?
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Why is it necessary to simplify redox reactions into half-reactions?
Why is it necessary to simplify redox reactions into half-reactions?
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Which step is involved in writing a balanced redox equation?
Which step is involved in writing a balanced redox equation?
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In a half-reaction for reduction, what does it include?
In a half-reaction for reduction, what does it include?
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Study Notes
Redox Reactions in Chemical Equations
Redox reactions, short for reduction-oxidation reactions, are a fundamental type of chemical reaction where electrons are transferred between the reactants, resulting in the oxidation of one reactant and the reduction of another. These reactions are crucial in various applications, from energy production to environmental processes.
Writing Redox Equations
To write a redox equation, follow these steps:
- Identify the substance being oxidized (loses electrons) and reduced (gains electrons).
- Balance the overall equation, ensuring that the number of electrons gained equals the number of electrons lost.
- Use half-reactions to balance the redox pair.
Half-Reactions
Half-reactions are simplified versions of redox reactions, focusing on either the oxidation or reduction of a substance.
A half-reaction for oxidation includes the substance being oxidized and the electrons gained during the reaction. For example:
[ \text{Zn}(s) \rightarrow \text{Zn}^{2+}(aq) + 2e^{-} ]
A half-reaction for reduction includes the substance being reduced and the electrons lost during the reaction. For example:
[ 2\text{H}^{+}(aq) + 2e^{-} \rightarrow \text{H}_2(g) ]
Writing a Redox Equation
To write a balanced redox equation, sum the half-reactions:
- Choose the half-reaction with the lowest number of electrons gained or lost.
- Balance the electrons using the coefficients.
- Multiply the half-reactions by appropriate integers to balance the atoms.
For example, consider the following redox reaction between zinc and hydrochloric acid:
[ \text{Zn}(s) + 2\text{HCl}(aq) \rightarrow \text{ZnCl}_2(aq) + \text{H}_2(g) ]
To simplify this reaction into half-reactions, write:
[ \text{Zn}(s) \rightarrow \text{Zn}^{2+}(aq) + 2e^{-} ]
[ 2\text{H}^{+}(aq) + 2e^{-} \rightarrow \text{H}_2(g) ]
Balance the electrons by multiplying the second half-reaction with 1:
[ 2\text{H}^{+}(aq) + 2e^{-} \rightarrow \text{H}_2(g) ]
Combine the half-reactions:
[ \text{Zn}(s) + 2\text{H}^{+}(aq) + \underbrace{2e^{-}}_{\text{from 2H}^{+}} \rightarrow \text{Zn}^{2+}(aq) + \text{H}_2(g) ]
Now, remove the common electrons:
[ \text{Zn}(s) + 2\text{HCl}(aq) \rightarrow \text{ZnCl}_2(aq) + \text{H}_2(g) ]
This balanced redox equation demonstrates the oxidation of zinc and the reduction of hydrogen ions during the reaction.
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Description
Test your understanding of redox reactions by learning to balance redox equations using half-reactions. Practice identifying the substances being oxidized and reduced, balancing electrons, and combining half-reactions to write a balanced redox equation.
