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Chapter 22: Problem 74

Write equations to show how to prepare \(\mathrm{H}_{2}(\mathrm{g})\) from each of the following substances: \((a) \mathrm{H}_{2} \mathrm{O} ;\) (b) \(\mathrm{HI}(\mathrm{aq})\) (c) \(\mathrm{Mg}(\mathrm{s}) ;\) (d) \(\mathrm{CO}(\mathrm{g})\). Use other common laboratory reactants as necessary, that is, water, acids or bases, metals, and so on.

Short Answer

Expert verified
The formulae show the preparation of Hydrogen gas are: \(2H_{2}O(l) \rightarrow 2H_{2}(g) + O_{2}(g)\) for water, \(2HI(aq) + Zn(s) \rightarrow H_{2}(g) + ZnI_{2}(s)\) for Hydroiodic acid, \(Mg(s) + 2HCl(aq) \rightarrow H_{2}(g) + MgCl_{2}(aq)\) for Magnesium and \(CO(g) + H_{2}O(g) \rightarrow H_{2}(g) + CO_{2}(g)\) for Carbon monoxide.

Step by step solution

01

Formula for H2O

To prepare hydrogen gas from water, a common method is to use electrolysis. The reaction equation is as follows: \(2H_{2}O(l) \rightarrow 2H_{2}(g) + O_{2}(g)\). Here, electricity is used to break the water molecules into hydrogen and oxygen gases.
02

Formula for HI(aq)

Hydroiodic acid (HI) can be reduced to produce hydrogen gas. This can be done using a metal such as zinc. The reaction equation is: \(2HI(aq) + Zn(s) \rightarrow H_{2}(g) + ZnI_{2}(s)\). Here, Zinc combines with Iodide and Hydrogen gas is released.
03

Formula for Mg

Magnesium can produce hydrogen gas when it reacts with an acid. In this case, hydrochloric acid (HCl) can be used. The reaction equation is: \(Mg(s) + 2HCl(aq) \rightarrow H_{2}(g) + MgCl_{2}(aq)\). Here, Magnesium chloride is formed and Hydrogen gas is released.
04

Formula for CO(g)

Carbon Monoxide can form hydrogen gas when it is mixed with steam in the presence of a catalyst like iron. The reaction equation is: \(CO(g) + H_{2}O(g) \rightarrow H_{2}(g) + CO_{2}(g)\). Here, Carbon dioxide is formed and Hydrogen gas is released.

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Most popular questions from this chapter

Figure \(15-1\) (page 656 ) shows that \(I_{2}\) is considerably more soluble in \(\mathrm{CCl}_{4}(1)\) than it is in \(\mathrm{H}_{2} \mathrm{O}(1) .\) The concentration of \(I_{2}\) in its saturated aqueous solution is \(1.33 \times 10^{-3} \mathrm{M},\) and the equilibrium achieved when \(\bar{I}_{2}\) distributes itself between \(\mathrm{H}_{2} \mathrm{O}\) and \(\mathrm{CCl}_{4}\) is $$\mathrm{I}_{2}(\mathrm{aq}) \rightleftharpoons \mathrm{I}_{2}\left(\mathrm{CCl}_{4}\right) \quad K_{\mathrm{c}}=85.5$$ (a) \(\mathrm{A} 10.0 \mathrm{mL}\) sample of saturated \(\mathrm{I}_{2}(\mathrm{aq})\) is shaken with \(10.0 \mathrm{mL} \mathrm{CCl}_{4} .\) After equilibrium is established, the two liquid layers are separated. How many milligrams of \(I_{2}\) will be in the aqueous layer? (b) If the \(10.0 \mathrm{mL}\) of aqueous layer from part (a) is extracted with a second \(10.0 \mathrm{mL}\) portion of \(\mathrm{CCl}_{4}\) how many milligrams of \(\mathrm{I}_{2}\) will remain in the aqueous layer when equilibrium is reestablished? (c) If the 10.0 mL sample of saturated \(I_{2}(\) aq) in part (a) had originally been extracted with \(20.0 \mathrm{mL} \mathrm{CCl}_{4}\) would the mass of \(I_{2}\) remaining in the aqueous layer have been less than, equal to, or greater than that in part (b)? Explain.

In \(1988,\) G. J. Schrobilgen, professor of chemistry at McMaster University in Canada, reported the synthesis of an ionic compound, \([\mathrm{HCNKrF}]\left[\mathrm{AsF}_{6}\right],\) which consists of \(\mathrm{HCNKr} \mathrm{F}^{+}\) and \(\mathrm{AsF}_{6}^{-}\) ions. In the \(\mathrm{HCNKr} \mathrm{F}^{+}\) ion, the krypton is covalently bonded to both fluorine and nitrogen. Draw Lewis structures for these ions, and estimate the bond angles.

Both nitramide and hyponitrous acid have the formula \(\mathrm{H}_{2} \mathrm{N}_{2} \mathrm{O}_{2} .\) Hyponitrous acid is a weak diprotic acid; nitramide contains the amide group \(\left(-\mathrm{NH}_{2}\right) .\) Draw plausible Lewis structures for these two substances.

The structure of \(\mathrm{N}\left(\mathrm{SiH}_{3}\right)_{3}\) involves a planar arrangement of \(\mathrm{N}\) and \(\mathrm{Si}\) atoms, whereas that of the related compound \(\mathrm{N}\left(\mathrm{CH}_{3}\right)_{3}\) has a pyramidal arrangement of N and \(\mathrm{C}\) atoms. Propose bonding schemes for these molecules that are consistent with this observation.

Provide an explanation for the observation that helium, neon, and argon do not react directly with fluorine.
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