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Chapter 22: Problem 24

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
(a) 2 Al + 6 HCl → 2 AlCl₃ + 3 H₂ (b) Mg + H₂O → MgO + H₂ (c) MnO₂ + 2 H₂ → MnO + 2 H₂O (d) CaH₂ + 2 H₂O → Ca(OH)₂ + 2 H₂

Step by step solution

01

(a) Aluminum metal reacts with acids to form hydrogen gas

First, we need to identify the reactants and products involved in the reaction. In this case, the reactants are aluminum metal (Al) and an acid (we'll use hydrochloric acid, HCl, as an example), and the products are a salt (aluminum chloride, AlCl₃) and hydrogen gas (H₂). Now we can write the unbalanced equation: Al + HCl → AlCl₃ + H₂ To balance the equation, note that there are 3 chlorine atoms in the product AlCl₃, so we need 3 HCl molecules for each Al atom. And since 3 moles of HCl will produce 3 moles of H atoms, we need to balance the H₂ gas by having 3/2 moles of H₂. The balanced equation is: 2 Al + 6 HCl → 2 AlCl₃ + 3 H₂
02

(b) Steam reacts with magnesium metal to give magnesium oxide and hydrogen

The reactants in this reaction are steam (water in its gaseous form, H₂O) and magnesium metal (Mg). The products are magnesium oxide (MgO) and hydrogen gas (H₂). We can write the unbalanced equation as: Mg + H₂O → MgO + H₂ To balance the equation, observe that there are 2 H atoms in both the reactants and products side as well as 1 O atom. So, the equation is already balanced: Mg + H₂O → MgO + H₂
03

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

In this reaction, manganese(IV) oxide (MnO₂) is reduced to manganese(II) oxide (MnO) by hydrogen gas (H₂). The other product of the reaction is water (H₂O). The unbalanced equation can be written as: MnO₂ + H₂ → MnO + H₂O To balance the equation, note that we need 2 H atoms in MnO and H₂O. However, there is only 1 O atom on the product side, so we need to also balance the O atoms by adding an extra H₂O to the product side. Thus, we have: MnO₂ + 2 H₂ → MnO + 2 H₂O
04

(d) Calcium hydride reacts with water to generate hydrogen gas

In this reaction, calcium hydride (CaH₂) reacts with water (H₂O) to generate hydrogen gas (H₂) and form calcium hydroxide (Ca(OH)₂). The unbalanced equation can be represented as: CaH₂ + H₂O → Ca(OH)₂ + H₂ To balance the equation, observe that we need two O atoms and four H atoms on the product side to balance with the reactant side. Thus, the balanced equation is: CaH₂ + 2 H₂O → Ca(OH)₂ + 2 H₂

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Most popular questions from this chapter

Write a balanced equation for the reaction of each of the following compounds with water: (a) \(\mathrm{SO}_{2}(g),(\mathbf{b}) \mathrm{Cl}_{2} \mathrm{O}_{7}(g)\) (c) \(\mathrm{Na}_{2} \mathrm{O}_{2}(s),\) (d) \(\mathrm{BaC}_{2}(s),\) (e) \(\mathrm{RbO}_{2}(s)\) (f) \(\mathrm{Mg}_{3} \mathrm{N}_{2}(s)\) , (g) \(\mathrm{NaH}(s) .\)

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

A friend tells you that the "neon" in neon signs is a compound of neon and aluminum. Can your friend be correct? Explain.

The dissolved oxygen present in any highly pressurized, high-temperature steam boiler can be extremely corrosive to its metal parts. Hydrazine, which is completely miscible with water, can be added to remove oxygen by reacting with it to form nitrogen and water. (a) Write the balanced equation for the reaction between gaseous hydrazine and oxygen.(b) Calculate the enthalpy change accompanying this reaction. (c) Oxygen in air dissolves in water to the extent of 9.1 ppm at \(20^{\circ} \mathrm{C}\) at sea level. How many grams of hydrazine are required to react with all the oxygen in 3.0 \(\times 10^{4} \mathrm{L}\) (the volume of a small swimming pool) under these conditions?

Write a balanced equation for each of the following reactions. (You may have to guess at one or more of the reaction products, but you should be able to make a reasonable guess, based on your study of this chapter.) (a) Hydrogen selenide can be prepared by reaction of an aqueous acid solution on aluminum selenide. (b) Sodium thiosulfate is used to remove excess \(\mathrm{Cl}_{2}\) from chlorine-bleached fabrics. The thiosulfate ion forms \(\mathrm{SO}_{4}^{2-}\) and elemental sulfur, while \(\mathrm{Cl}_{2}\) is reduced to \(\mathrm{Cl}^{-}\) .
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