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Chapter 3: Problem 146

When \(0.273 \mathrm{~g}\) of \(\mathrm{Mg}\) is heated strongly in a nitrogen \(\left(\mathrm{N}_{2}\right)\) atmosphere, a chemical reaction occurs. The product of the reaction weighs 0.378 g. Calculate the empirical formula of the compound containing \(\mathrm{Mg}\) and \(\mathrm{N}\). Name the compound.

Short Answer

Expert verified
The empirical formula of the compound is Mg3N, and its name is Magnesium Nitride.

Step by step solution

01

Convert Mass into Moles

We can convert mass into moles using the formula: n = m/M, where n is the number of moles, m is the mass and M is the molar mass. The molar masses of Mg and N are 24.31 \mathrm{~g/mol} and 14.01 \mathrm{~g/mol} respectively. For Mg: n = 0.273 g / 24.31 g/mol = 0.0112 mol. Since Nitrogen forms diatomic molecules, the molar mass is twice that of a single Nitrogen atom. Therefore the mass of Nitrogen that reacted can be found by subtracting the mass of the original Mg and the final compound: 0.378 g - 0.273 g = 0.105 g. The number of moles of Nitrogen are then: n = 0.105 g / (14.01 g/mol * 2) = 0.00375 mol.
02

Determine the Simplest Ratio

The ratio of the moles of Mg to the moles of N is then: 0.0112 mol / 0.00375 mol = 3. This means that there are 3 moles of Mg for every mole of N in the compound. Therefore, the empirical formula of the compound is Mg3N.
03

Name the Compound

The compound is called Magnesium Nitride. It follows the naming rules for ionic compounds, where the metal (Mg) is named first, followed by the nonmetal (N), which is modified to end with '-ide'.

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Most popular questions from this chapter

Write balanced equations for the following reactions described in words. (a) Pentane burns in oxygen to form carbon dioxide and water. (b) Sodium bicarbonate reacts with hydrochloric acid to form carbon dioxide, sodium chloride, and water. (c) When heated in an atmosphere of nitrogen, lithium forms lithium nitride. (d) Phosphorus trichloride reacts with water to form phosphorus acid and hydrogen chloride. (e) Copper(II) oxide heated with ammonia will form copper, nitrogen gas, and water.

Analysis of a metal chloride \(\mathrm{XCl}_{3}\) show that it contains 67.2 percent \(\mathrm{Cl}\) by mass. Calculate the molar mass of \(\mathrm{X}\) and identify the element.

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 grams) 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 = \(2000 \mathrm{lb} ; 1 \mathrm{lb}=453.6 \mathrm{~g} .)\)

Does \(1 \mathrm{~g}\) of hydrogen molecules contain as many \(\mathrm{H}\) atoms as \(1 \mathrm{~g}\) of hydrogen atoms?

The following is a crude but effective method for estimating the order of magnitude of Avogadro's number using stearic acid \(\left(\mathrm{C}_{18} \mathrm{H}_{36} \mathrm{O}_{2}\right)\) shown here. When stearic acid is added to water, its molecules collect at the surface and form a monolayer; that is, the layer is only one molecule thick. The crosssectional area of each stearic acid molecule has been measured to be \(0.21 \mathrm{nm}^{2}\). In one experiment it is found that \(1.4 \times 10^{-4} \mathrm{~g}\) of stearic acid is needed to form a monolayer over water in a dish of diameter \(20 \mathrm{~cm} .\) Based on these measurements, what is A vogadro's number?
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