Determine the empirical,molecular formula ?Arenes are a special type of compound consisting of only carbon and hydrogen.If 5.000g of a specific arene with a molar mass approximately 155g/mol yields 17.123g of CO2.Upon combustion in a purely oxygen atmosphere.determine the a) empirical, and b) molecular formulas, for the compound. ### Understanding Arenes: Empirical and Molecular Formulas**Concept Overview:**Arenes are a unique type of compound made solely of carbon and hydrogen atoms. These compounds are significant in organic chemistry due to their aromatic properties.**Problem Statement:**Consider a specific arene with a molar mass of approximately 155 g/mol. When 5.000 g of this arene undergoes combustion in an oxygen-rich environment, it produces 17.123 g of carbon dioxide (CO₂). Your task is to determine the:a) **Empirical formula** b) **Molecular formula** **Instructions for Finding Formulas:**- **Empirical Formula:** The simplest whole-number ratio of atoms in the compound.- **Molecular Formula:** The actual number of atoms of each element in a molecule of the compound.**Important Note:**Chemical notation is case sensitive. Ensure correct format in your solutions.**Input Fields:**a) Enter your empirical formula hereb) Enter your molecular formula hereBy completing this exercise, you will deepen your understanding of combustion analysis and the determination of chemical formulas.

Given : Grams of arene = 5.00 g Molar mass of arene =155 g/mol Mass of CO2 =17.123 g(a) From the given grams of CO2, we can find the mass of C in the given sample of arene. Convert the grams of CO2 into moles as shown below, 17.123g CO2×1 mol CO2 44.01 g CO2=0.3891 mol CO2 Convert the moles of CO2 into grams of C as shown below, 0.3891 mol CO2×1 mol C1 mol CO2×12.011 g C1 mol C=4.6735 g C From the grams of C and mass of arene sample we can calculate grams of H as shown below, mass of H = 5.00 g- 4.6735g=0.3265 g HConvert grams of H into moles as shown below. 0.3265 g H×1 mol H1.008 gH=0.3239 mol H We have moles of C = 0.3891 mol To get number of atoms in empirical formula, divide moles of C and H with lease number of moles as shown below, For H = 0.3239mol0.3239mol=1For C =0.3891mol0.3239 mol=1.2 To get the whole number, multiply each above number with 5, For H =1×5 =5For C =1.2×5=6 Thus, the empirical formula of the arene is C6H5. (b) Given molar mass of arene = 155 g/mol Empirical formula mass = C6H5 = 77.106 g/mol From the above values we can calculate the number by which we can find the molecular formula of the compound, n = Molar massempirical formula mass=155g/mol77.106g/mol=2.0 Multiply empirical formula by 2 as (2 x C6H5) = C12H10 Thus, molecular formula of the compound is, C12H10.