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Chapter 3: Problem 36

Describe how the knowledge of the percent composition by mass of an unknown compound can help us identify the compound.

Short Answer

Expert verified
The knowledge of the percent composition by mass of an unknown compound can help us identify the compound by providing details about the proportion of elements in it. This leads us to the empirical formula and thus, the identity of the compound.

Step by step solution

01

Definition of Percent Composition

Percent Composition is a calculation of how much of each element constitutes a compound, expressed in terms of percentages. This information can be derived from the compound's molecular or empirical formula.
02

Role of Percent Composition in Compound Identification

Knowing the percent composition by mass of an unknown compound helps us identify the compound because it provides us with specific details about the proportion in which the elements combine to form the compound. This information can draw us closer to the empirical formula and eventually to the identity of the compound.
03

Application in Chemistry

Percent Composition is used in chemistry to determine the amount of specific elements present in chemical compounds. This knowledge is useful when experimenting, analysing substances or when trying to recreate a particular compound in the lab.

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Most popular questions from this chapter

Industrially, nitric acid is produced by the Ostwald process represented by the following equations: \(\begin{aligned} 4 \mathrm{NH}_{3}(g)+5 \mathrm{O}_{2}(g) & \longrightarrow 4 \mathrm{NO}(g)+6 \mathrm{H}_{2} \mathrm{O}(l) \\ 2 \mathrm{NO}(g)+\mathrm{O}_{2}(g) & \longrightarrow 2 \mathrm{NO}_{2}(g) \\ 2 \mathrm{NO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow & \mathrm{HNO}_{3}(a q)+\mathrm{HNO}_{2}(a q) \end{aligned}\) What mass of \(\mathrm{NH}_{3}\) (in g) must be used to produce 1.00 ton of \(\mathrm{HNO}_{3}\) by the above procedure, assuming an 80 percent yield in each step? \((1\) ton \(=2000 \mathrm{lb}\); \(1 \mathrm{lb}=453.6 \mathrm{~g} .)\)

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A compound X contains 63.3 percent manganese (Mn) and 36.7 percent O by mass. When \(X\) is heated, oxygen gas is evolved and a new compound \(\mathrm{Y}\) containing 72.0 percent \(\mathrm{Mn}\) and 28.0 percent \(\mathrm{O}\) is formed. (a) Determine the empirical formulas of \(X\) and Y. (b) Write a balanced equation for the conversion of \(X\) to \(Y\).
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