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Chapter 3: Problem 37

What does the word "empirical" in empirical formula mean?

Short Answer

Expert verified
In an empirical formula, 'empirical' means that the formula is based on experimental data. It reflects the simplest, whole-number ratio of atoms in a compound. It does not provide actual number of atoms, which might be given by molecular formula, but gives the simplest, yet meaningful piece of information about the compound.

Step by step solution

01

Definition

Empirical, when referred to in an empirical formula, derives from the word 'empiricism', which is a philosophical belief that all knowledge is based on experience. Therefore, empirical suggests something based on observation or experiment, not just theoretical ideas.
02

Connection to empirical formula

\An empirical formula in chemistry is the simplest, whole-number ratio of atoms in a compound. It does not necessarily show the real number of atoms in each molecule, but the ratio derived from experimental data.
03

Importance of Empirical Formula

The use of the term 'empirical' stresses the fact that this kind of formula is based on empirical evidence - that is, formulas are determined using experimental data, including elemental analysis, which provides the ratio of atoms according to the amount of elements present. It does not provide actual number of atoms, which might be given by molecular formula, but empirical formula is critical as it gives the simplest, most reduced ratio of elements within a molecule, yet meaningful piece of information about the compound.

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Most popular questions from this chapter

If we know the empirical formula of a compound, what additional information do we need to determine its molecular formula?

The fertilizer ammonium sulfate \(\left[\left(\mathrm{NH}_{4}\right)_{2} \mathrm{SO}_{4}\right]\) is prepared by the reaction between ammonia \(\left(\mathrm{NH}_{3}\right)\) and sulfuric acid: $$ 2 \mathrm{NH}_{3}(g)+\mathrm{H}_{2} \mathrm{SO}_{4}(a q) \longrightarrow\left(\mathrm{NH}_{4}\right)_{2} \mathrm{SO}_{4}(a q) $$ How many kilograms of \(\mathrm{NH}_{3}\) are needed to produce \(1.00 \times 10^{5} \mathrm{~kg}\) of \(\left(\mathrm{NH}_{4}\right)_{2} \mathrm{SO}_{4} ?\)

Each copper(II) sulfate unit is associated with five water molecules in crystalline copper(II) sulfate pentahydrate \(\left(\mathrm{CuSO}_{4} \cdot 5 \mathrm{H}_{2} \mathrm{O}\right)\). When this compound is heated in air above \(100^{\circ} \mathrm{C},\) it loses the water molecules and also its blue color: $$ \mathrm{CuSO}_{4} \cdot 5 \mathrm{H}_{2} \mathrm{O} \longrightarrow \mathrm{CuSO}_{4}+5 \mathrm{H}_{2} \mathrm{O} $$ If \(9.60 \mathrm{~g}\) of \(\mathrm{CuSO}_{4}\) are left after heating \(15.01 \mathrm{~g}\) of the blue compound, calculate the number of moles of \(\mathrm{H}_{2} \mathrm{O}\) originally present in the compound.

Use ammonia \(\left(\mathrm{NH}_{3}\right)\) to explain what is meant by the percent composition by mass of a compound.

Nitroglycerin \(\left(\mathrm{C}_{3} \mathrm{H}_{5} \mathrm{~N}_{3} \mathrm{O}_{9}\right)\) is a powerful explosive. Its decomposition can be represented by $$ 4 \mathrm{C}_{3} \mathrm{H}_{5} \mathrm{~N}_{3} \mathrm{O}_{9} \longrightarrow 6 \mathrm{~N}_{2}+12 \mathrm{CO}_{2}+10 \mathrm{H}_{2} \mathrm{O}+\mathrm{O}_{2} $$ This reaction generates a large amount of heat and many gaseous products. It is the sudden formation of these gases, together with their rapid expansion, that produces the explosion. (a) What is the maximum amount of \(\mathrm{O}_{2}\) in grams that can be obtained from \(2.00 \times 10^{2} \mathrm{~g}\) of nitroglycerin? (b) Calculate the percent yield in this reaction if the amount of \(\mathrm{O}_{2}\) generated is found to be \(6.55 \mathrm{~g}\).
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