Consider 100.0-g samples of two different compounds consisting only of carbon and oxygen. one compound contains 27.2 g of carbon and the other has 42.9 g of carbon. how can these data support the law of multiple proportions if 42.9 is not a multiple of 27.2? show that these data support the law of multiple proportions.

Explanation:

It is known that a mole of carbon atom contains a mass of 12 g and a mole of oxygen atom contains a mass of 16 g.

As it is given that first compound has 27.2 g C. So, amount of oxygen present in this compound will be as follows.

                         (100 - 27.2) g

                        = 72.8 g of O

Hence, calculate the moles of C and O as follows.

       No. of moles of C =

                                    =

                                    = 2.26 mol

        No. of moles of O =

                                    =

                                    = 4.55 mol

Therefore, mole ratios of both C and O will be calculated as follows.

               C =

                   = 1

                O =

                   = 2

Hence, empirical formula of the first compound is .

Since, it is also given that mass of carbin in another compound is 42.9 g. So, mass of oxygen present will be as follows.

                           (100 - 42.9) g

                          = 57.1 g

Hence, calculate the moles of C and O as follows.

      No. of moles of C =

                                    =

                                    = 3.57 mol

      No. of moles of O =

                                    =

                                    = 3.57 mol    

Therefore, mole ratios of both C and O will be calculated as follows.

               C =

                   = 1

                O =

                   = 1

Hence, empirical formula of the second compound is CO.

Therefore, carbon and oxygen combine to form 2 different compounds in small whole numbers.

2b2t

explanation:

2b2t