Question

A 3.80-g sample of an unknown compound containing only C, H, and O combusts in an oxygen rich environment. When the products have cooled to 20.0 degree C at 1 bar, there are 4.96 L of CO_2 and 2.45 mL of H_2O. The density of water at 20.0 degree C is 0.998 g/mL. What is the empirical formula of the unknown compound? If the molar mass is 168.2 g/mol, what is the molecular formula of the compound?

Answer 1

O: 20.0°C = 273+20 = 293 K Pal bar v=4.962. R=0008314 L-Bay/kmal PVzRT n= (1 bar) (4:962) (0.08814 l-bar/ K-mad) (29314) males of corn = 0.2036 mal) 2.45mL of water contains no. of groms = valeme) (density) = (2.45 m2) (0.098g/mL) a 24451 g males of H2o=2.4451g s C 1891 mal = 10.13584 mail Males of C in con = 1x males of con = 0.2036 map nales of Hin H₂O = 28 males of H₂O = 2X0.135842 0.27 16 h weight of c = (0.2036 mal X 12 g/mad) = 2.4432g coeight of H = (0.27167 mal xiglmal) = 0.27167 g careight of o = (3.80g) - (2.4432 +0. 271167) g = 3.8 - 2.714872 10 08513 g males of o= 1085139 16 zimãe 2 000678 map mals Of CIHLO :0.2036 : 0.27167: 010678 3:4:1 empirical formula C 3 H40] empin' cal formula ceight = 12x3+4x1 +16 = 56 emoleculor formula weight) 168.2... 50"? 3 ( empirical formula wreigen) Malecedor tormula = (Chao), = Catig og