Textbook Question
At 900 °C, titanium tetrachloride vapor reacts with molten magnesium metal to form solid titanium metal and molten magnesium chloride. (a) Write a balanced equation for this reaction.
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Ch.20 - Electrochemistry
Chapter 20, Problem 22c
Hydrazine (N2H4) and dinitrogen tetroxide (N2O4) form a self-igniting mixture that has been used as a rocket propellant. The reaction products are N2 and H2O. (c) Which substance serves as the reducing agent and which as the oxidizing agent?
Verified step by step guidance1
Identify the oxidation states of each element in the reactants and products.
Determine the changes in oxidation states for each element to identify which elements are oxidized and reduced.
Recall that the reducing agent is the substance that donates electrons (is oxidized) and the oxidizing agent is the substance that accepts electrons (is reduced).
Compare the oxidation states of nitrogen in N2H4 and N2O4 to those in the products N2 and H2O.
Assign the roles of reducing and oxidizing agents based on the changes in oxidation states.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Oxidation and Reduction
Oxidation and reduction are chemical processes that involve the transfer of electrons between substances. Oxidation refers to the loss of electrons, while reduction involves the gain of electrons. In a redox reaction, one substance is oxidized and another is reduced, which is essential for understanding the roles of reactants in chemical reactions.
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Oxidation and Reduction Reactions
Oxidizing and Reducing Agents
An oxidizing agent is a substance that causes another to be oxidized, meaning it gains electrons itself. Conversely, a reducing agent is a substance that donates electrons to another, causing it to be reduced. Identifying these agents in a reaction is crucial for determining the flow of electrons and understanding the overall reaction mechanism.
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01:01Oxidizing and Reducing Agents
Balancing Chemical Reactions
Balancing chemical reactions is the process of ensuring that the number of atoms for each element is the same on both sides of the equation. This is important for accurately representing the conservation of mass in a reaction. Balancing helps in identifying the stoichiometry of reactants and products, which is vital for determining the roles of substances in redox reactions.
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Related Practice
Textbook Question
At 900 °C, titanium tetrachloride vapor reacts with molten magnesium metal to form solid titanium metal and molten magnesium chloride (c) Which substance is the reductant, and which is the oxidant?
Textbook Question
Hydrazine (N2H4) and dinitrogen tetroxide (N2O4) form a self-igniting mixture that has been used as a rocket propellant. The reaction products are N2 and H2O. (a) Write a balanced chemical equation for this reaction.
Textbook Question
Complete and balance the following half-reactions. In each case, indicate whether the half-reaction is an oxidation or a reduction. (a) Sn2+(aq) → Sn4+(aq) (acidic solution) (b) TiO2(s) → Ti2+(aq) (acidic solution) (c) ClO3-(aq) → Cl-(aq) (acidic solution) (d) N2(g) → NH4+(aq) (acidic solution)
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Textbook Question
Complete and balance the following half-reactions. In each case, indicate whether the half-reaction is an oxidation or a reduction. (f) SO32-1aq2 ¡ SO42-1aq2 (basic solution)
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Textbook Question
Complete and balance the following half-reactions. In each case indicate whether the half-reaction is an oxidation or a reduction. (a) Mo3+(aq) → Mo(s) (acidic solution) (b) H2SO3(aq) → SO42-(aq) (acidic solution) (c) NO3-(aq) → NO(g) (acidic solution) (d) O2(g) → H2O(l) (acidic solution)
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