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Chapter 22: Problem 70

Give the chemical formula for (a) carbonic acid, (b) sodium cyanide, (c) potassium hydrogen carbonate, (d) acetylene.

Short Answer

Expert verified
The chemical formula for (a) carbonic acid is \(H_2CO_3\), (b) sodium cyanide is \(NaCN\), (c) potassium hydrogen carbonate is \(KHCO_3\), and (d) acetylene is \(C_2H_2\).

Step by step solution

01

(a) Carbonic acid

Carbonic acid is composed of the elements hydrogen (H), carbon (C), and oxygen (O). The chemical symbols for hydrogen, carbon, and oxygen are H, C, and O, respectively. Carbonic acid is formed when one carbon atom binds with two oxygen atoms and two hydrogen atoms. In this case, the chemical formula is H鈧侰O鈧�.
02

(b) Sodium cyanide

Sodium cyanide is composed of the elements sodium (Na) and the cyanide ion (CN). The chemical symbols for sodium and cyanide are Na and CN, respectively. Sodium cyanide is formed when one sodium atom binds with one cyanide ion. In this case, the chemical formula is NaCN.
03

(c) Potassium hydrogen carbonate

Potassium hydrogen carbonate is composed of the elements potassium (K), hydrogen (H), carbon (C), and oxygen (O). The chemical symbols for potassium, hydrogen, carbon, and oxygen are K, H, C, and O, respectively. Potassium hydrogen carbonate is formed when one potassium atom, one hydrogen atom, one carbon atom, and three oxygen atoms bind together. In this case, the chemical formula is KHCO鈧�.
04

(d) Acetylene

Acetylene is composed of the elements carbon (C) and hydrogen (H). The chemical symbols for carbon and hydrogen are C and H, respectively. Acetylene is formed when two carbon atoms bind together with a triple bond, and each carbon atom also binds to a single hydrogen atom. In this case, the chemical formula is C鈧侶鈧�.

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Most popular questions from this chapter

Write a chemical formula for each compound or ion, and indicate the oxidation state of the group 5 A element in each formula: (a) phosphate ion, (b) arsenous acid, (c) antimony(III) sulfide, (d) calcium dihydrogen phosphate, (e) potassium phosphide.

One method proposed for removing \(\mathrm{SO}_{2}\) from the flue gases of power plants involves reaction with aqueous \(\mathrm{H}_{2} \mathrm{~S}\). Elemental sulfur is the product. (a) Write a balanced chemical equation for the reaction. (b) What volume of \(\mathrm{H}_{2} \mathrm{~S}\) at \(27{ }^{\circ} \mathrm{C}\) and 740 torr would be required to remove the \(\mathrm{SO}_{2}\) formed by burning \(1.0\) ton of coal containing \(3.5 \%\) S by mass? (c) What mass of elemental sulfur is produced? Assume that all reactions are \(100 \%\) efficient.

Complete and balance the following equations: (a) \(\mathrm{Li}_{3} \mathrm{~N}(\mathrm{~s})+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow\) (b) \(\mathrm{NH}_{3}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow\) (c) \(\mathrm{NO}_{2}(\mathrm{~g})+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow\) (d) \(\mathrm{NH}_{3}(g)+\mathrm{O}_{2}(g) \stackrel{\text { catalyst }}{\longrightarrow}\) (e) \(\mathrm{H}_{2} \mathrm{CO}_{3}(a q) \stackrel{\Delta}{\longrightarrow}\) (f) \(\mathrm{Ni}(s)+\mathrm{CO}(g) \longrightarrow\) (h) \(\mathrm{CS}_{2}(g)+\mathrm{O}_{2}(g) \longrightarrow\) (i) \(\mathrm{CaO}(s)+\mathrm{SO}_{2}(g) \longrightarrow\) (j) \(\mathrm{CH}_{4}(g)+\mathrm{H}_{2} \mathrm{O}(g) \stackrel{\Delta}{\longrightarrow}\) (k) \(\mathrm{LiH}(s)+\mathrm{H}_{2} \mathrm{O}(t) \longrightarrow\) (1) \(\mathrm{Fe}_{2} \mathrm{O}_{3}(s)+3 \mathrm{H}_{2}(g) \longrightarrow\)

Both dimethylhydrazine, \(\left(\mathrm{CH}_{3}\right)_{2} \mathrm{NNH}_{2}\), and methylhydrazine, \(\mathrm{CH}_{3} \mathrm{NH} \mathrm{NH}_{2}\), have been used as rocket fuels. When dinitrogen tetroxide \(\left(\mathrm{N}_{2} \mathrm{O}_{4}\right)\) is used as the oxidizer, the products are \(\mathrm{H}_{2} \mathrm{O}, \mathrm{CO}_{2}\), and \(\mathrm{N}_{2}\). If the thrust of the rocket depends on the volume of the products produced, which of the substituted hydrazines produces a greater thrust per gram total mass of oxidizer plus fuel? (Assume that both fuels generate the same temperature and that \(\mathrm{H}_{2} \mathrm{O}(\mathrm{g})\) is formed.)

Write the Lewis structure for each of the following species, and describe its geometry: (a) \(\mathrm{NH}_{4}^{+}\), (b) \(\mathrm{NO}_{2}^{-}\), (c) \(\mathrm{N}_{2} \mathrm{O}\), (d) \(\mathrm{NO}_{2}\).
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