---
title: "A volatile chlorinated hydrocarbon compound with the molecular formula \\(\\text{C}_x\\text{H}_y\\text{Cl}_z\\) is analyzed using a mass spectrometer. The mass spectrum displays a cluster of three molecular ion peaks corresponding to the intact cation \\([\\text{C}_x\\text{H}_y\\text{Cl}_z]^+\\) as shown in the table below.  | \\(m/z\\) | Relative Intensity | |:——-:|:——————:| | 112     | 90                 | | 114     | 60                 | | 116     | 10                 |  Naturally occurring chlorine consists of two major isotopes, \\(^{35}\\text{Cl}\\) (nominal mass \\(35\\text{ amu}\\), relative abundance \\(\\approx 75\\%\\)) and \\(^{37}\\text{Cl}\\) (nominal mass \\(37\\text{ amu}\\), relative abundance \\(\\approx 25\\%\\)). Assume that carbon and hydrogen consist exclusively of \\(^{12}\\text{C}\\) (nominal mass \\(12\\text{ amu}\\)) and \\(^{1}\\text{H}\\) (nominal mass \\(1\\text{ amu}\\)). Based on these data, what is the value of \\(y\\), the number of hydrogen atoms in one molecule of the compound?"
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url: "https://nerd-notes.com/ubq/120130/"
date_modified: "2026-08-21T09:21:43+00:00"
---

# A volatile chlorinated hydrocarbon compound with the molecular formula \(\text{C}_x\text{H}_y\text{Cl}_z\) is analyzed using a mass spectrometer. The mass spectrum displays a cluster of three molecular ion peaks corresponding to the intact cation \([\text{C}_x\text{H}_y\text{Cl}_z]^+\) as shown in the table below.

| \(m/z\) | Relative Intensity |
|:——-:|:——————:|
| 112     | 90                 |
| 114     | 60                 |
| 116     | 10                 |

Naturally occurring chlorine consists of two major isotopes, \(^{35}\text{Cl}\) (nominal mass \(35\text{ amu}\), relative abundance \(\approx 75\%\)) and \(^{37}\text{Cl}\) (nominal mass \(37\text{ amu}\), relative abundance \(\approx 25\%\)). Assume that carbon and hydrogen consist exclusively of \(^{12}\text{C}\) (nominal mass \(12\text{ amu}\)) and \(^{1}\text{H}\) (nominal mass \(1\text{ amu}\)). Based on these data, what is the value of \(y\), the number of hydrogen atoms in one molecule of the compound?

A volatile chlorinated hydrocarbon compound with the molecular formula \(\text{C}_x\text{H}_y\text{Cl}_z\) is analyzed using a mass spectrometer. The mass spectrum displays a cluster of three molecular ion peaks corresponding to the intact cation \([\text{C}_x\text{H}_y\text{Cl}_z]^+\) as shown in the table below.

| \(m/z\) | Relative Intensity |
|:-------:|:------------------:|
| 112     | 90                 |
| 114     | 60                 |
| 116     | 10                 |

Naturally occurring chlorine consists of two major isotopes, \(^{35}\text{Cl}\) (nominal mass \(35\text{ amu}\), relative abundance \(\approx 75\%\)) and \(^{37}\text{Cl}\) (nominal mass \(37\text{ amu}\), relative abundance \(\approx 25\%\)). Assume that carbon and hydrogen consist exclusively of \(^{12}\text{C}\) (nominal mass \(12\text{ amu}\)) and \(^{1}\text{H}\) (nominal mass \(1\text{ amu}\)). Based on these data, what is the value of \(y\), the number of hydrogen atoms in one molecule of the compound?

- **A.** \(2\)
- **B.** \(4\)
- **C.** \(6\)
- **D.** \(8\)

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/120130/*