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?