Textbook Question
Indicate whether the following balanced equations involve oxidation–reduction. If they do, identify the elements that undergo changes in oxidation number. (a) 2 AgNO3(aq) + CoCl2(aq) → 2 AgCl(s) + Co(NO3)2(aq)
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Ch.20 - Electrochemistry
Chapter 20, Problem 22a
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.
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Identify the reactants and products in the chemical reaction. The reactants are hydrazine (N2H4) and dinitrogen tetroxide (N2O4), and the products are nitrogen gas (N2) and water (H2O).
Write the unbalanced chemical equation using the chemical formulas of the reactants and products: N2H4 + N2O4 → N2 + H2O.
Count the number of atoms of each element on both sides of the equation. For nitrogen (N), hydrogen (H), and oxygen (O), ensure that the number of atoms is equal on both sides.
Balance the equation by adjusting the coefficients. Start by balancing the nitrogen atoms, then hydrogen, and finally oxygen. Use the smallest whole numbers possible.
Verify that the equation is balanced by recounting the atoms of each element on both sides of the equation. Ensure that the number of atoms for each element is the same on both sides.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Balancing Chemical Equations
Balancing chemical equations involves ensuring that the number of atoms of each element is the same on both the reactant and product sides of the equation. This is based on the law of conservation of mass, which states that matter cannot be created or destroyed in a chemical reaction. To balance an equation, coefficients are adjusted in front of the chemical formulas to achieve equal atom counts.
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Balancing Chemical Equations
Stoichiometry
Stoichiometry is the quantitative relationship between reactants and products in a chemical reaction. It allows chemists to predict the amounts of substances consumed and produced in a reaction based on balanced equations. Understanding stoichiometry is essential for calculating yields, determining limiting reactants, and scaling reactions for practical applications, such as in rocket propellant formulations.
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Combustion Reactions
Combustion reactions are exothermic reactions that typically involve a fuel reacting with an oxidant, producing heat and light. In the case of hydrazine and dinitrogen tetroxide, the reaction produces nitrogen gas (N2) and water (H2O) as products. Recognizing the characteristics of combustion reactions helps in understanding their applications, such as in propulsion systems for rockets.
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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. (a) Write a balanced equation for this reaction.
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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. (c) Which substance serves as the reducing agent and which as the oxidizing agent?
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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) 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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