Find the molecular formula of a compound that contains 56.36 g of oxygen (o) and 43.64 g of phosphorus (p). the molar mass of the compound is 283.9 gmol. your

We have to first find the empirical formula. Empirical formula gives the simplest ratio of whole number of components in a compound.
                                    oxygen                   phosphorous 
mass                           56.36 g                         43.64 g
number of moles         56.36 g/ 16 g/mol          43.64 g/ 31 g/mol 
                                     =3.5                             = 1.4
divide by least number of moles 
                                      3.5/1.4 = 2.5                1.4/1.4 = 1
multiply by 2 to get a whole number 
O - 2.5 x 2 = 5
P - 1x2 = 2
Therefore empirical formula - P₂O₅
Mass of one empirical unit - 31x2 + 16 x 5 = 62 + 80 = 142
number of empirical units - 283.9 / 142 = 2
Therefore molecular formula - 2(P₂O₅)
molecular formula - P₄O₁₀

No table found. the question asks for covalent bond based on electronegativies

Olá. porque a reação na temperatura é muito rapida a do copo : )