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Chapter 22: Problem 26

Write balanced equations for each of the following reactions (some of these are analogous to reactions shown in the chapter). (a) Aluminum metal reacts with acids to form hydrogen gas. (b) Steam reacts with magnesium metal to give magnesium oxide and hydrogen. (c) Manganese(IV) oxide is reduced to manganese(II) oxide by hydrogen gas. (d) Calcium hydride reacts with water to generate hydrogen gas.

Short Answer

Expert verified
The balanced equations for the given reactions are: a) \(2 Al (s) + 6 HCl (aq) \rightarrow 2 AlCl_3 (aq) + 3 H_2 (g)\) b) \(Mg (s) + H_2O (g) \rightarrow MgO (s) + H_2 (g)\) c) \(MnO_2 (s) + 2 H_2 (g) \rightarrow MnO (s) + 2 H_2O (g)\) d) \(CaH_2 (s) + 2 H_2O (l) \rightarrow Ca(OH)_2 (aq) + 2 H_2 (g)\)

Step by step solution

01

Reaction a: Aluminum metal reacts with acids to form hydrogen gas

In this case, we consider hydrochloric acid as a representative for acids. The reaction can be written as: Al (s) + HCl (aq) -> AlCl3 (aq) + H2 (g) Now we need to balance the equation: 2 Al (s) + 6 HCl (aq) -> 2 AlCl3 (aq) + 3 H2 (g)
02

Reaction b: Steam reacts with magnesium metal to give magnesium oxide and hydrogen

Write the reaction: Mg (s) + H2O (g) -> MgO (s) + H2 (g) Balance the equation: Mg (s) + H2O (g) -> MgO (s) + H2 (g) In this case, the equation is already balanced.
03

Reaction c: Manganese(IV) oxide is reduced to manganese(II) oxide by hydrogen gas

Write the reaction: MnO2 (s) + H2 (g) -> MnO (s) + H2O (g) Balance the equation: MnO2 (s) + 2 H2 (g) -> MnO (s) + 2 H2O (g)
04

Reaction d: Calcium hydride reacts with water to generate hydrogen gas

Write the reaction: CaH2 (s) + H2O (l) -> Ca(OH)2 (aq) + H2 (g) Now we need to balance the equation: CaH2 (s) + 2 H2O (l) -> Ca(OH)2 (aq) + 2 H2 (g)

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Most popular questions from this chapter

Write the chemical formula for each of the following, and indicate the oxidation state of the halogen or noble-gas atom in each, (a) calcium hypobromite, (b) bromic acid, (c) xenon trioxide, (d) perchlorate ion, (e) iodous acid, (f) iodine pentafluoride.

The solubility of \(\mathrm{Cl}_{2}\) in \(100 \mathrm{~g}\) of water at \(\mathrm{STP}\) is \(310 \mathrm{~cm}^{3}\). Assume that this quantity of \(\mathrm{Cl}_{2}\) is dissolved and equilibrated as follows: $$ \mathrm{Cl}_{2}(a q)+\mathrm{H}_{2} \mathrm{O} \rightleftharpoons \mathrm{Cl}^{-}(a q)+\mathrm{HClO}(a q)+\mathrm{H}^{+}(a q) $$ If the equilibrium constant for this reaction is \(4.7 \times 10^{-4}\), calculate the equilibrium concentration of \(\mathrm{HClO}\) formed.

Silicon has a limited capacity to form linear, \(\mathrm{Si}-\mathrm{Si}\) bonded structures similar to those formed by carbon. (a) Predict the molecular formula of a hydride of silicon that contains a chain of three silicon atoms. (b) Write a balanced equation for the reaction between oxygen and the compound you predicted in part (a).

(a) What is the oxidation state of \(\mathrm{P}\) in \(\mathrm{PO}_{4}^{3-}\) and of \(\mathrm{N}\) in \(\mathrm{NO}_{3}^{-}\) ? (b) Why doesn't \(\mathrm{N}\) form a stable \(\mathrm{NO}_{4}{ }^{3-}\) ion analogous to \(\mathrm{P}\) ?

An aqueous solution of \(\mathrm{SO}_{2}\) reduces (a) aqueous \(\mathrm{KMnO}_{4}\) to \(\mathrm{MnSO}_{4}(a q)\), (b) acidic aqueous \(\mathrm{K}_{2} \mathrm{Cr}_{2} \mathrm{O}_{7}\) to aqueous \(\mathrm{Cr}^{3+}\), (c) aqueous \(\mathrm{Hg}_{2}\left(\mathrm{NO}_{3}\right)_{2}\) to mercury metal. Write balanced equations for these reactions.
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