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Chapter 3: 3.112_CP (page 136)

The study of sulfur-nitrogen compounds is an active area of chemical research, made more so by the discovery in the early 1980s of one such compound that conducts electricity like a metal. The first sulfur-nitrogen compound was prepared in 1835 and serves today as a reactant for preparing many of the others. Mass spectrometry of the compound shows a molar mass of 184.27 g/mol, and analysis shows it to contain 2.288 g of S for every 1.000 g of N. What is its molecular formula?

Short Answer

Expert verified

The molecular formula is S4N4.

Step by step solution

01

Finding the moles of S and N

On converting the mass of S & N into moles by multiplication for molar mass reciprocal.

Moles鈥�of鈥�S=2.288鈥�g鈥�S脳1鈥�molS32.07鈥�g鈥�S=0.0713鈥�mol鈥�SMoles鈥�of鈥�N=1鈥�g鈥�N脳1鈥�mol鈥�N14.01鈥�g鈥�N=0.0714鈥�molN

02

Finding the molecular formula

The whole number multiple can be derived as,

=184.27鈥�g/mol46.08鈥�g/molWhole鈥�number鈥�multiple=4

On multiplying the subscript of S1N1 by 4. The molecular formula can be found as S4N4.

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Most popular questions from this chapter

Hemoglobin is 6.0% heme (C34H32FeN4O4) by mass. To remove the heme, hemoglobin is treated with acetic acid and NaCl to form hemin (C34H32N4O4FeCl). At a crime scene, a blood sample contains 0.65 g of hemoglobin. (a) How many grams of heme are in the sample? (b) How many moles of heme? (c) How many grams of Fe? (d) How many grams of hemin could be formed for a forensic chemist to measure?

Aspirin (acetylsalicylic acid, C9H8O4) is made by reacting salicylic acid (C7H6O3) with acetic anhydride [(CH3CO)2O]:

C7H6O3(S)+(CH3CO)2O(I)鈫�C9H8O4(S)+CH3COOH(I)

In one reaction, 3.077 g of salicylic acid and 5.50 mL of acetic anhydride react to form 3.281 g of aspirin. (a) Which is the limiting reactant (d of acetic anhydride = 1.080 g/mL)? (b) What is the percent yield of this reaction? (c) What is the percent atom economy of this reaction?

Find the empirical formula of the following compounds:

(a) 0.063 mol of chlorine atoms combined with 0.22 mol of oxygen atoms

(b) 2.45 g of silicon combined with 12.4 g of chlorine

(c) 27.3 mass % carbon and 72.7 mass % oxygen

Ethanol (CH3CH2OH), the intoxicant in alcoholic beverages, is also used to make other organic compounds. In concentrated sulfuric acid, ethanol forms diethyl ether and water:

2CH3CH2OH(I)鈫�CH3CH2OCH3CH2(I)+H2O(g)

In a side reaction, some ethanol forms ethylene and water:

CH3CH2OH(I)鈫�CH2=CH2(g)+H2O(g)

(a) If 50.0 g of ethanol yields 35.9 g of diethyl ether, what is the percent yield of diethyl ether? (b) During the process, 45.0% of the ethanol that did not produce diethyl ether reacts by the side reaction. What mass of ethylene is produced?

The following circles represent a chemical reaction between AB2 and B2:

(a) Write a balanced equation for the reaction. (b) What is the limiting reactant? (c) How many moles of product can be made from 3.0 mol of B2 and 5.0 mol of AB2? (d) How many moles of excess reactant remain after the reaction in part (c)?
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