Question

If anyone could solve this problem and show work please? I'm a tad bit confused! Thank you! :D

"A 0.02882 g sample of gas occupies 10.0-mL at 288.5 K and 1.10 atm. Upon further analysis, the compound is found to be 38.734% C and 61.266% F. What is the molecular formula of the compound?"

A 0.02882 g sample of gas occupies 10.0-mL at 288.5 K and 1.10 atm. Upon further analysis, the compound is found to be 38.734% C and 61.266% F. What is the molecular formula of the compound? Identify the geometry around each carbon atom. Draw the Lewis structure of the compound. tetrahedral linear trigonal pyramidal trigonal planar bent Is this compound polar? The compound is polar. The compound is nonpolar.

Answer 1

Calculation of molar mass of the component pv = nRT pv = omega/m RT m = omega/pv RT omega = 0.02882 g p = 1.10 atm v = 10 mL = 0.010 L R = 0.0821 L atm/k mol T = 288.5 k M = 0.02882 g times 0.0821 L atm/k mol times 288.5 k/1.10 atm times 0.010 L = 62.06 g/mol Calculation of Empirical formula(EF) of the compound Element % Atomic mass Atomic = % ratio/Atomic mass C 38.734 12.0 38.734/12 = 3.2278 F 61.266 19.0 61.266/19 = 3.2245 C: F = 3.2278: 3.2245 = 3.2278/3.2245: 3.2245/3.2245 = 1: 1 \r\n Empirical Formula = CF To find out molecular formula: Molecular formula = (Empirical Formula)_r where r = Molecular formula mass/Empirical Formula mass molar formula mass = 62.06 g/mol Empirical Formula mass of CF = 12 + 19 = 31 g/mol therefore n = 62.06 g/mol/31 g/mol = 2 therefore molecular formula = (CF)_2 = C_2F_2