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Chapter 3: Problem 127

In using a mass spectrometer, a chemist sees a peak at a mass of \(30.0106 .\) Of the choices \({ }^{12} \mathrm{C}_{2}{ }^{1} \mathrm{H}_{6}{ }_{6}{ }^{12} \mathrm{C}^{1} \mathrm{H}_{2}{ }^{16} \mathrm{O}\), and \({ }^{14} \mathrm{~N}^{16} \mathrm{O}\), which is responsible for this peak? Pertinent masses are \({ }^{1} \mathrm{H}\), \(1.007825 ;{ }^{16} \mathrm{O}, 15.994915 ;\) and \({ }^{14} \mathrm{~N}, 14.003074 .\)

Short Answer

Expert verified
The molecule responsible for the mass spectrometer peak at 30.0106 is \({ }^{14}\mathrm{N}^{16}\mathrm{O}\), as its molecular mass (30.008) is closest to the observed mass peak.

Step by step solution

01

Identify the given information

The mass spectrometer peak is at a mass of 30.0106. Possible choices are: 1. \({ }^{12}C_{2}{ }^{1}H_{6}{ }_{6}{ }^{12}C^{1}H_{2}{ }^{16}O\) 2. \({ }^{14}\mathrm{N}^{16}\mathrm{O}\) Pertinent masses are: - \({ }^{1}\mathrm{H}\): 1.007825 - \({ }^{16}\mathrm{O}\): 15.994915 - \({ }^{14}\mathrm{N}\): 14.003074
02

Calculate the molecular mass of each choice

We need to find the molecular mass of each choice by adding up the atomic masses present in the molecule. This can be calculated as follows: For choice 1: \({ }^{12}C_{2}{ }^{1}H_{6}{ }_{6}{ }^{12}C^{1}H_{2}{ }^{16}O\) Molecular mass = (2 × (12.0000)) + (6 × 1.007825) + (6 × 12.0000)+ (2 × 1.007825) + (1 × 15.994915) For choice 2: \({ }^{14}\mathrm{N}^{16}\mathrm{O}\) Molecular mass = (1 × 14.003074) + (1 × 15.994915)
03

Compare calculated molecular mass with the observed mass peak

Now we need to compare the calculated molecular mass for each choice with the observed mass peak from the mass spectrometer to determine which molecule is responsible for the mass peak. For choice 1: Calculated molecular mass = (2 × (12.0000)) + (6 × 1.007825) + (6 × 12.0000)+ (2 × 1.007825) + (1 × 15.994915) ≈ 30.016 For choice 2: Calculated molecular mass = (1 × 14.003074) + (1 × 15.994915) ≈ 30.008
04

Identify the molecule responsible for the peak

Upon comparing the calculated molecular masses with the observed mass peak (30.0106), we can conclude that choice 2, i.e., \({ }^{14}\mathrm{N}^{16}\mathrm{O}\), is the molecule responsible for the peak as its molecular mass (30.008) is the closest to the observed mass peak.

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Most popular questions from this chapter

Ascorbic acid, or vitamin \(\mathrm{C}\left(\mathrm{C}_{6} \mathrm{H}_{8} \mathrm{O}_{6}\right)\), is an essential vitamin. It cannot be stored by the body and must be present in the diet. What is the molar mass of ascorbic acid? Vitamin C tablets are taken as a dietary supplement. If a typical tablet contains \(500.0 \mathrm{mg}\) vitamin \(\mathrm{C}\), what amount (moles) and what number of molecules of vitamin C does it contain?

The compound adrenaline contains \(56.79 \% \mathrm{C}, 6.56 \% \mathrm{H}\), \(28.37 \% \mathrm{O}\), and \(8.28 \% \mathrm{~N}\) by mass. What is the empirical formula for adrenaline?

Coke is an impure form of carbon that is often used in the industrial production of metals from their oxides. If a sample of coke is \(95 \%\) carbon by mass, determine the mass of coke needed to react completely with \(1.0\) ton of copper(II) oxide. $$ 2 \mathrm{CuO}(s)+\mathrm{C}(s) \longrightarrow 2 \mathrm{Cu}(s)+\mathrm{CO}_{2}(g) $$

A compound contains only \(\mathrm{C}, \mathrm{H}\), and \(\mathrm{N}\). Combustion of \(35.0 \mathrm{mg}\) of the compound produces \(33.5 \mathrm{mg} \mathrm{CO}_{2}\) and \(41.1 \mathrm{mg}\) \(\mathrm{H}_{2} \mathrm{O}\). What is the empirical formula of the compound?

A compound contains \(47.08 \%\) carbon, \(6.59 \%\) hydrogen, and \(46.33 \%\) chlorine by mass; the molar mass of the compound is \(153 \mathrm{~g} / \mathrm{mol}\). What are the empirical and molecular formulas of the compound?
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