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Chapter 20: Problem 22

Hydrazine \(\left(\mathrm{N}_{2} \mathrm{H}_{4}\right)\) and dinitrogen tetroxide \(\left(\mathrm{N}_{2} \mathrm{O}_{4}\right)\) form a self-igniting mixture that has been used as a rocket propellant. The reaction products are \(\mathrm{N}_{2}\) and \(\mathrm{H}_{2} \mathrm{O}\). (a) Write a balanced chemical equation for this reaction. (b) What is being oxidized, and what is being reduced? (c) Which substance serves as the reducing agent and which as the oxidizing agent?

Short Answer

Expert verified
(a) The balanced chemical equation for the reaction is: \[ N_{2}H_{4} + 2N_{2}O_{4} \rightarrow 3N_{2} + 4H_{2}O \] (b) Nitrogen in hydrazine is being oxidized, while nitrogen in dinitrogen tetroxide is being reduced. (c) Hydrazine \(N_{2}H_{4}\) serves as the reducing agent, and dinitrogen tetroxide \(N_{2}O_{4}\) serves as the oxidizing agent.

Step by step solution

01

Write the unbalanced chemical equation

The unbalanced chemical equation shows the reactants and products. In this case, they are hydrazine, dinitrogen tetroxide, nitrogen gas, and water: \[ N_{2}H_{4} + N_{2}O_{4} \rightarrow N_{2} + H_{2}O \]
02

Balance the chemical equation

To balance the chemical equation, we will adjust the coefficients in front of each molecule to ensure the same number of atoms on both sides of the equation. The balanced chemical equation is: \[ N_{2}H_{4} + 2N_{2}O_{4} \rightarrow 3N_{2} + 4H_{2}O \] Part B: Identify the substances being oxidized and reduced
03

Determine the oxidation states of each atom in the reactants and products

The oxidation states for each element in the reactants and products are: Hydrazine (N2H4): N: -2 (each) H: +1 (each) Dinitrogen Tetroxide (N2O4): N: +4 (each) O: -2 (each) Nitrogen Gas (N2): N: 0 Water (H2O): H: +1 (each) O: -2
04

Identify the substances being oxidized and reduced

Compare the oxidation states of elements in the reactants to those in the products: - Nitrogen in hydrazine (going from -2 to 0): Oxidized - Nitrogen in dinitrogen tetroxide (going from +4 to 0): Reduced Part C: Determine the reducing agent and the oxidizing agent
05

Identify the reducing agent and the oxidizing agent

Since hydrazine's nitrogen is being oxidized, hydrazine (N2H4) is the reducing agent. Similarly, since dinitrogen tetroxide's nitrogen is being reduced, dinitrogen tetroxide (N2O4) is the oxidizing agent.

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Most popular questions from this chapter

If the equilibrium censtant for a one-electron redox reaction at \(298 \mathrm{~K}\) is \(8.7 \times 10^{4}\), calculate the corresponding \(\Delta G^{\circ}\) and \(E_{\text {red }}\)

In each of the following balanced oxidation-reduction equations, identify those elements that undergo changes in oxidation number and indicate the magnitude of the change in each case. (a) \(\mathrm{I}_{2} \mathrm{O}_{\mathrm{s}}(s)+5 \mathrm{CO}(\mathrm{g}) \longrightarrow \mathrm{I}_{2}(s)+5 \mathrm{CO}_{2}(\mathrm{~g})\) (b) \(2 \mathrm{Hg}^{2+}(a q)+\mathrm{N}_{2} \mathrm{H}_{4}(a q) \longrightarrow 2 \mathrm{Hg}(l)+\mathrm{N}_{2}(g)+4 \mathrm{H}^{+}(a q)\) (c) \(3 \mathrm{H}_{2} \mathrm{~S}(a q)+2 \mathrm{H}^{+}(a q)+2 \mathrm{NO}_{3}^{-}(a q) \longrightarrow 3 \mathrm{~S}(s)+\) \(2 \mathrm{NO}(g)+4 \mathrm{H}_{2} \mathrm{O}(l)\)

Hydrogen gas has the potential for use as a clean fuel in reaction with oxygen. The relevant reaction is $$ 2 \mathrm{H}_{2}(g)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{H}_{2} \mathrm{O}(I) $$ Consider two possible ways of utilizing this reaction as an electrical energy source: (i) Hydrogen and oxygen gases are combusted and used to drive a generator, much as coal is currently used in the electric power industry; (ii) hydrogen and oxygen gases are used to generate electricity directly by using fuel cells that operate at \(85^{\circ} \mathrm{C}\). (a) Use data in Appendix C to calculate \(\Delta H^{t}\) and \(\Delta S^{\circ}\) for the reaction. We will assume that these values do not change appreciably with temperature. (b) Based on the values from part (a), what trend would you expect for the magnitude of \(\Delta G\) for the reaction as the temperature increases? (c) What is the significance of the change in the magnitude of \(\Delta G\) with temperature with respect to the utility of hydrogen as a fuel? (d) Based on the analysis here, would it be more efficient to use the combustion method or the fuel-cell method to generate electrical energy from hydrogen?

(a) What conditions must be met for a reduction potential to be a standard reduction potential? (b) What is the standard reduction potential of a standard hydrogen electrode? (c) Why is it impossible to measure the standard reduction potential of a single half-reaction?

The crude copper that is subjected to electrorefining contains tellurium as an impurity. The standard reduction potential between tellurium and its lowest common oxidation state, \(\mathrm{Te}^{4+}\), is $$ \mathrm{Te}^{4+}(a q)+4 e^{-} \longrightarrow \mathrm{Te}(s) \quad E_{\text {iod }}^{s}=0.57 \mathrm{~V} $$ Given this information, describe the probable fate of tellurium impurities during electrorefining. Do the impurities fall to the bottom of the refining bath, unchanged, as copper is oxidized, or do they go into solution as ions? If they go into solution, do they plate out on the cathode?
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