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The first experimental evidence needed is to identify the elements present in the new compound. This can be done using several methods, such as mass spectrometry, X-ray diffraction, and chemical tests. Once you know the elements in the compound, you can start investigating the ratios of these elements to each other.

The next important experimental evidence is the ratio of the elements within the compound. This can be determined through various methods such as combustion analysis, gravimetric analysis, and titration. In combustion analysis, the compound is burned in an excess of oxygen, and the amounts of products formed (such as water and carbon dioxide) are weighed. These weights can then be used to find the ratio of the elements in the compound. Gravimetric analysis relies on the precipitation of an insoluble species from the compound, which can then be used to deduce the elemental composition. Titration can involve adding a known concentration of a reactant to a sample until a reaction is completed. The amount of reactant used can provide valuable information about the compound's elemental composition.

Knowing the compound's molecular mass is another essential piece of experimental evidence. This information can be found using mass spectrometry or other techniques such as vapor density determination or freezing point depression measurements. The molecular mass will help in establishing the compound's empirical and molecular formulas.

With the elements present in the compound and their ratios known, you can now determine the empirical formula, which represents the simplest whole-number ratio of the elements in the compound. To do this, divide the ratio of the elements by their respective molar masses, then normalize them to the smallest whole number ratio. This will give you the empirical formula of the new compound.

Finally, if you have the molecular mass of the compound, you can determine its molecular formula. The molecular formula is a multiple of the empirical formula. To find the molecular formula, divide the compound's molecular mass by the empirical formula's mass. The result is the multiple you need to multiply the empirical formula to get the molecular formula of the new compound.