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Chapter 22: Problem 53

Complete and balance the following equations: (a) $\mathrm{Mg}_{3} \mathrm{~N}_{2}(s)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow$ (b) \(\mathrm{NO}(g)+\mathrm{O}_{2}(g) \longrightarrow\) (c) $\mathrm{N}_{2} \mathrm{O}_{5}(g)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow$ (d) \(\mathrm{NH}_{3}(a q)+\mathrm{H}^{+}(a q) \longrightarrow\) (e) \(\mathrm{N}_{2} \mathrm{H}_{4}(l)+\mathrm{O}_{2}(g) \longrightarrow\) Which ones of these are redox reactions?

Short Answer

Expert verified
The balanced equations are: (a) Mg₃N₂(s) + 6H₂O(l) → 3Mg(OH)₂(s) + 2NH₃(g) (redox) (b) 2NO(g) + O₂(g) → 2NO₂(g) (redox) (c) N₂O₅(g) + H₂O(l) → 2HNO₃(aq) (redox) (d) NH₃(aq) + H⁺(aq) → NH₄⁺(aq) (not redox) (e) N₂H₄(l) + 2O₂(g) → N₂(g) + 4H₂O(l) (redox) Redox reactions: (a), (b), (c), and (e).

Step by step solution

01

1. Complete and balance Reaction (a)

We need to balance the given equation: \[ \mathrm{Mg}_{3} \mathrm{N}_{2}(s)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \] First, complete the reaction by writing the expected product, which is magnesium hydroxide and ammonia gas: \[ \mathrm{Mg}_{3} \mathrm{N}_{2}(s)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \mathrm{Mg}(\mathrm{OH})_{2}(s)+\mathrm{NH}_{3}(g) \] Now, let's balance it by adjusting the number of moles of reactants and products: \[ \mathrm{Mg}_{3} \mathrm{N}_{2}(s)+6 \mathrm{H}_{2} \mathrm{O}(l) \longrightarrow 3 \mathrm{Mg}(\mathrm{OH})_{2}(s)+2 \mathrm{NH}_{3}(g) \]
02

2. Complete and balance Reaction (b)

We need to balance the given equation: \[ \mathrm{NO}(g)+\mathrm{O}_{2}(g) \longrightarrow \] First, complete the reaction by providing the expected product, which is nitrogen dioxide: \[ \mathrm{NO}(g)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{NO}_{2}(g) \] Now, let's balance the equation by adjusting the number of moles of reactants and products: \[ 2 \mathrm{NO}(g)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{NO}_{2}(g) \]
03

3. Complete and balance Reaction (c)

We need to balance the given equation: \[ \mathrm{N}_{2} \mathrm{O}_{5}(g)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \] First, complete the reaction by providing the expected product, which is nitric acid: \[ \mathrm{N}_{2} \mathrm{O}_{5}(g)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow 2 \mathrm{HNO}_{3}(aq) \] Now, let's balance the equation by adjusting the number of moles of reactants and products: \[ \mathrm{N}_{2} \mathrm{O}_{5}(g)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow 2 \mathrm{HNO}_{3}(aq) \]
04

4. Complete and balance Reaction (d)

We need to balance the given equation: \[ \mathrm{NH}_{3}(a q)+\mathrm{H}^{+}(a q) \longrightarrow \] First, complete the reaction by providing the expected product, which is ammonium ion: \[ \mathrm{NH}_{3}(a q)+\mathrm{H}^{+}(a q) \longrightarrow \mathrm{NH}_{4}^{+}(aq) \] The equation is already balanced.
05

5. Complete and balance Reaction (e)

We need to balance the given equation: \[ \mathrm{N}_{2} \mathrm{H}_{4}(l)+\mathrm{O}_{2}(g) \longrightarrow \] First, complete the reaction by providing the expected product, which is nitrogen gas and water: \[ \mathrm{N}_{2} \mathrm{H}_{4}(l)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{N}_{2}(g)+\mathrm{H}_{2}\mathrm{O}(l) \] Now, let's balance the equation by adjusting the number of moles of reactants and products: \[ \mathrm{N}_{2} \mathrm{H}_{4}(l)+2 \mathrm{O}_{2}(g) \longrightarrow \mathrm{N}_{2}(g)+4 \mathrm{H}_{2}\mathrm{O}(l) \]
06

6. Identify redox reactions

To find out which of these reactions are redox reactions, we need to check if there are any changes in the oxidation numbers of the elements in the reactants and products. (a) Mg₃N₂(s) + 6H₂O(l) → 3Mg(OH)₂(s) + 2NH₃(g) Oxidation numbers change, so it is a redox reaction. (b) 2NO(g) + O₂(g) → 2NO₂(g) Oxidation numbers change, so it is a redox reaction. (c) N₂O₅(g) + H₂O(l) → 2HNO₃(aq) Oxidation numbers change, so it is a redox reaction. (d) NH₃(aq) + H⁺(aq) → NH₄⁺(aq) No changes in oxidation numbers, so it is not a redox reaction. (e) N₂H₄(l) + 2O₂(g) → N₂(g) + 4H₂O(l) Oxidation numbers change, so it is a redox reaction. Hence, the redox reactions are (a), (b), (c), and (e).

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Most popular questions from this chapter

(a) Determine the number of calcium ions in the chemical formula of the mineral hardystonite, $\mathrm{Ca}_{x} \mathrm{Zn}\left(\mathrm{Si}_{2} \mathrm{O}_{7}\right)$. (b) Determine the number of hydroxide ions in the chemical formula of the mineral pyrophyllite, $\mathrm{Al}_{2}\left(\mathrm{Si}_{2} \mathrm{O}_{5}\right)_{2}(\mathrm{OH})_{x}$.

Account for the following observations: (a) Phosphorus forms a pentachloride, but nitrogen does not. (b) \(\mathrm{H}_{3} \mathrm{PO}_{2}\) is a monoprotic acid. (c) Phosphonium salts, such as \(\mathrm{PH}_{4} \mathrm{Cl}\), can be formed under anhydrous conditions, but they cannot be made in aqueous solution. (d) White phosphorus is more reactive than red phosphorus.

Write the Lewis structure for each of the following species, describe its geometry, and indicate the oxidation state of the nitrogen: $(\mathbf{a}) \mathrm{N}_{2} \mathrm{O}_{3},\( (b) \)\mathrm{NOCl}\( (c) \)\mathrm{NO}_{2} \mathrm{Cl}\( (d) \)\mathrm{N}_{2} \mathrm{O}_{4}$.

Although the \(\mathrm{ClO}_{4}^{-}\) and \(\mathrm{IO}_{4}^{-}\) ions have been known for a long time, \(\mathrm{BrO}_{4}^{-}\) was not synthesized until $1965 .$ The ion was synthesized by oxidizing the bromate ion with xenon difluoride, producing xenon, hydrofluoric acid, and the perbromate ion. (a) Write the balanced equation for this reaction. (b) What are the oxidation states of Br in the Br-containing species in this reaction?

Write balanced equations for each of the following reactions. (a) When mercury(II) oxide is heated, it decomposes to form \(\mathrm{O}_{2}\) and mercury metal. ( \(\mathbf{b}\) ) When copper(II) nitrate is heated strongly, it decomposes to form copper(II) oxide, nitrogen dioxide, and oxygen. (c) Lead(II) sulfide, \(\mathrm{PbS}(s)\) reacts with ozone to form \(\mathrm{PbSO}_{4}(s)\) and \(\mathrm{O}_{2}(g) .\) (d) When heated in air, \(\mathrm{ZnS}(s)\) is converted to \(\mathrm{ZnO}\). (e) Potassium peroxide reacts with \(\mathrm{CO}_{2}(g)\) to give potassium carbonate and \(\mathrm{O}_{2}\). (f) Oxygen is converted to ozone in the upper atmosphere.
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