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Chapter 21: Problem 9

Write the formulas of the following compounds. (a) ammonia (b) laughing gas (c) hydrogen peroxide (d) sulfur trioxide

Short Answer

Expert verified
Answer: The chemical formulas for the given compounds are: (a) Ammonia - NH_3, (b) Laughing gas - N_2O, (c) Hydrogen peroxide - H_2O_2, and (d) Sulfur trioxide - SO_3.

Step by step solution

01

(a) Ammonia Formula

Ammonia is a compound made up of nitrogen and hydrogen. The formula for ammonia can be found by recognizing that it has one nitrogen atom and three hydrogen atoms. The chemical symbol for nitrogen is N and for hydrogen is H. Therefore, the formula for ammonia is NH_3.
02

(b) Laughing Gas Formula

Laughing gas, also known as nitrous oxide, is a compound made up of nitrogen and oxygen. It contains two nitrogen atoms and one oxygen atom. The chemical symbol for nitrogen is N and for oxygen is O. Thus, the formula for laughing gas is N_2O.
03

(c) Hydrogen Peroxide Formula

Hydrogen peroxide is a compound composed of hydrogen and oxygen. It has two hydrogen atoms and two oxygen atoms. The chemical symbol for hydrogen is H, and for oxygen, it is O. Consequently, the formula for hydrogen peroxide is H_2O_2.
04

(d) Sulfur Trioxide Formula

Sulfur trioxide is a compound made up of sulfur and oxygen. It contains one sulfur atom and three oxygen atoms. The chemical symbol for sulfur is S, and for oxygen, it is O. As a result, the formula for sulfur trioxide is SO_3.

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Most popular questions from this chapter

The average concentration of bromine (as bromide) in seawater is \(65 \mathrm{ppm} .\) Calculate (a) the volume of seawater \(\left(d=64.0 \mathrm{lb} / \mathrm{ft}^{3}\right)\) in cubic feet required to produce one kilogram of liquid bromine. (b) the volume of chlorine gas in liters, measured at \(20^{\circ} \mathrm{C}\) and \(762 \mathrm{~mm}\) \(\mathrm{Hg}\), required to react with this volume of sea water.

Write the formula of the acid formed when each of these acidic oxides reacts with water. (a) \(\mathrm{SO}_{2}\) (b) \(\mathrm{Cl}_{2} \mathrm{O}\) (c) \(\mathrm{P}_{4} \mathrm{O}_{6}\)

At equilibrium, a gas mixture has a partial pressure of \(0.7324\) atm for \(\mathrm{HBr}\) and \(2.80 \times 10^{-3}\) atm for both hydrogen and bromine gases. What is \(K\) for the formation of two moles of HBr from \(\mathrm{H}_{2}\) and \(\mathrm{Br}_{2} ?\)

If an electrolytic cell producing fluorine uses a current of \(7.00 \times 10^{3} \mathrm{~A}\) (at \(10.0 \mathrm{~V})\), how many grams of fluorine gas can be produced in two days (assuming that the cell operates continuously at \(95 \%\) efficiency)?

Write a balanced equation for the reaction of ammonia with (a) \(\mathrm{Cu}^{2+}\) (b) \(\mathrm{H}^{+}\) (c) \(\mathrm{Al}^{3+}\)
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