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Chapter 4: Problem 68

Write balanced net ionic equations for the following reactions in acid solution. (a) Nitrogen oxide and hydrogen gases react to form ammonia gas and steam. (b) Hydrogen peroxide reacts with an aqueous solution of sodium hypochlorite to form oxygen and chlorine gases. (c) Zinc metal reduces the vanadyl ion \(\left(\mathrm{VO}^{2+}\right)\) to vanadium(III) ions. Zinc ions are also formed.

Short Answer

Expert verified
Question: Provide the balanced net ionic equation for the reaction between nitrogen oxide and hydrogen gases to form ammonia gas and steam in acidic solution. Answer: The balanced net ionic equation for the reaction is: $$2\,H_2(\text{g}) + 3\text{NO(g)} + 4\,H^+(aq) \rightarrow 2\text{NH}_3(\text{g})+\text{ H}_2\text{O}(\text{l})$$

Step by step solution

01

Write the unbalanced equation

The unbalanced equation for the reaction is: $$\text{NO}(\text{g}) + \text{H}_2(\text{g}) \rightarrow \text{NH}_3(\text{g}) + \text{H}_2\text{O}(\text{l})$$
02

Determine oxidation states of elements

Assign oxidation states to all the elements in the unbalanced equation: N: +2 (in NO), -3 (in NH3), O: -2 (in H2O), H: +1 (in H2 and H2O, and NH3).
03

Identify the redox half-reactions

The oxidation half-reaction is H2(g) -> H2O(l). The reduction half-reaction is NO(g) -> NH3(g).
04

Balance atoms and charges in half-reactions

Balance the two half-reactions, separately: Oxidation half-reaction: $$2\,H_2(\text{g}) \rightarrow 4\,\text{H}^+(aq) + 4\text{ e}^{-}$$ Reduction half-reaction: $$3\text{NO (g)} + 8\text{ H}^{+}(aq) + 3\text{ e}^{-}\rightarrow 2\text{NH}_3(\text{g})+\text{ H}_2\text{O}(\text{l})$$
05

Combine the balanced half-reactions and cancel spectator ions

Combine the balanced half-reactions to obtain the balanced net ionic equation: $$2\,H_2(\text{g}) + 3\text{NO(g)} + 8\text{ H}^{+}(aq) \rightarrow 4\,\text{H}^+(aq) + 2\text{NH}_3(\text{g})+\text{ H}_2\text{O}(\text{l})$$ Cancel out the spectator ions (4H+) to get the final balanced net ionic equation: $$2\,H_2(\text{g}) + 3\text{NO(g)} + 4\,H^+(aq) \rightarrow 2\text{NH}_3(\text{g})+\text{ H}_2\text{O}(\text{l})$$ (b) Hydrogen peroxide reacts with an aqueous solution of sodium hypochlorite to form oxygen and chlorine gases.
06

Write the unbalanced equation

The unbalanced equation for the reaction is: $$\text{H}_2\text{O}_2(\text{aq}) + \text{NaOCl}(\text{aq}) \rightarrow \text{O}_2(\text{g}) + \text{Cl}_2(\text{g}) + \text{Na}^{+}(\text{aq}) + \text{H}^{+}(\text{aq})$$
07

Determine oxidation states of elements

Assign oxidation states to all the elements in the unbalanced equation: O: -1 (in H2O2), -2 (in NaOCl), 0 (in O2), Cl: +1 (in NaOCl), 0 (in Cl2), Na: +1 (in NaOCl), H: +1 (in H2O2 and H+).
08

Identify the redox half-reactions

The oxidation half-reaction is H2O2(aq) -> O2(g). The reduction half-reaction is NaOCl(aq) -> Cl2(g).
09

Balance atoms and charges in half-reactions

Balance the two half-reactions, separately: Oxidation half-reaction: $$2\,\text{H}_2\text{O}_2(aq) \rightarrow 2\,\text{O}_2(\text{g}) + 4\text{ H}^{+}(aq) + 4\text{ e}^{-}$$ Reduction half-reaction: $$2\,\text{OCl}^{-}(aq) + 2\,H^{+}(aq) + 2\,\text{e}^{-} \rightarrow \text{Cl}_2(\text{g}) + 2\,H_2\text{O}(l)$$
10

Combine the balanced half-reactions and cancel spectator ions

Combine the balanced half-reactions to obtain the balanced net ionic equation: $$2\,\text{H}_2\text{O}_2(aq) + 2\,\text{OCl}^{-}(aq) + 2\,\text{H}^{+}(aq) \rightarrow 2\,\text{O}_2(\text{g}) + 4\text{ H}^{+}(aq) + \text{Cl}_2(\text{g}) + 2\,H_2\text{O}(l)$$ Cancel out the spectator ions (2H+) to get the final balanced net ionic equation: $$2\,\text{H}_2\text{O}_2(aq) + 2\,\text{OCl}^{-}(aq) \rightarrow 2\,\text{O}_2(\text{g}) + 2\text{H}^{+}(aq) + \text{Cl}_2(\text{g}) + 2\,H_2\text{O}(l)$$ (c) Zinc metal reduces the vanadyl ion (\(\text{VO}^{2+}\)) to vanadium(III) ions. Zinc ions are also formed.
11

Write the unbalanced equation

The unbalanced equation for the reaction is: $$\text{Zn}(s) + \text{VO}^{2+}(aq) \rightarrow \text{V}^{3+}(aq) + \text{Zn}^{2+}(aq)$$
12

Determine oxidation states of elements

Assign oxidation states to all the elements in the unbalanced equation: Zn: 0 (in Zn), +2 (in Zn2+), V: +5 (in VO2+), +3 (in V3+), O: -2 (in VO2+).
13

Identify the redox half-reactions

The oxidation half-reaction is Zn(s) -> Zn2+(aq). The reduction half-reaction is VO2+(aq) -> V3+(aq).
14

Balance atoms and charges in half-reactions

Balance the two half-reactions, separately: Oxidation half-reaction: $$\text{Zn}(s) \rightarrow \text{Zn}^{2+}(aq) + 2\text{ e}^{-}$$ Reduction half-reaction: $$2\,\text{VO}^{2+}(aq) + 6\,\text{H}^{+}(aq) + 2\,\text{e}^{-} \rightarrow 2\,\text{V}^{3+}(aq) + \text{H}_2\text{O}(l)$$
15

Combine the balanced half-reactions and cancel spectator ions

Combine the balanced half-reactions to obtain the balanced net ionic equation: $$\text{Zn}(s) + 2\,\text{VO}^{2+}(aq) + 6\,\text{H}^{+}(aq) \rightarrow \text{Zn}^{2+}(aq) + 2\,\text{V}^{3+}(aq) + \text{H}_2\text{O}(l)$$ There are no spectator ions to cancel in this case. The final balanced net ionic equation is: $$\text{Zn}(s) + 2\,\text{VO}^{2+}(aq) + 6\,\text{H}^{+}(aq) \rightarrow \text{Zn}^{2+}(aq) + 2\,\text{V}^{3+}(aq) + \text{H}_2\text{O}(l)$$

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Most popular questions from this chapter

Write balanced net ionic equations for the following reactions in acid solution. (a) Liquid hydrazine reacts with an aqueous solution of sodium bromate. Nitrogen gas and bromide ions are formed. (b) Solid phosphorus \(\left(P_{4}\right)\) reacts with an aqueous solution of nitrate to form nitrogen oxide gas and dihydrogen phosphate \(\left(\mathrm{H}_{2} \mathrm{PO}_{4}^{-}\right)\) ions. (c) Aqueous solutions of potassium sulfite and potassium permanganate react. Sulfate and manganese(II) ions are formed.

Calcium in blood or urine can be determined by precipitation as call cium oxalate, \(\mathrm{CaC}_{2} \mathrm{O}_{4}\). The precipitate is dissolved in strong acid and titrated with potassium permanganate. The products of the reaction are carbon dioxide and manganese(II) ion. A 24-hour urine sample is collected from an adult patient, reduced to a small volume, and titrated with \(26.2 \mathrm{~mL}\) of \(0.0946 \mathrm{M} \mathrm{KMnO}_{4}\). How many grams of calcium oxalate are in the sample? Normal range for \(\mathrm{Ca}^{2+}\) output for an adult is 100 to \(300 \mathrm{mg}\) per 24 hour. Is the sample within the normal range?

Copper metal can reduce silver ions to metallic silver. The copper is oxidized to copper ions according to the reaction $$ 2 \mathrm{Ag}^{+}(a q)+\mathrm{Cu}(s) \longrightarrow \mathrm{Cu}^{2+}(a q)+2 \mathrm{Ag}(s) $$ A copper strip with a mass of \(2.00 \mathrm{~g}\) is dipped into a solution of \(\mathrm{AgNO}_{3}\). After some time has elapsed, the copper strip is coated with silver. The strip is removed from the solution, dried, and weighed. The coated strip has a mass of \(4.18 \mathrm{~g}\). What are the masses of copper and silver metals in the strip? (Hint: Remember that the copper metal is being used up as silver metal forms.)

Classify each of the following half-equations as oxidation or reduction and balance. (a) (basic) \(\quad \mathrm{ClO}^{-}(a q) \longrightarrow \mathrm{Cl}^{-}(a q)\) (b) (acidic) \(\quad \mathrm{NO}_{3}^{-}(a q) \longrightarrow \mathrm{NO}(g)\) (c) (basic) \(\quad \mathrm{Ni}^{2+}(a q) \longrightarrow \mathrm{Ni}_{2} \mathrm{O}_{3}(s)\) (d) (acidic) \(\quad \mathrm{Mn}^{2+}(a q) \longrightarrow \mathrm{MnO}_{2}(s)\)

Mssign oxidation numbers to each element in (a) \(\mathrm{HIO}_{3}\) (b) \(\mathrm{NaMnO}_{4}\) (c) \(\mathrm{SnO}_{2}\) (d) NOF (e) \(\mathrm{NaO}_{2}\)
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