a 7.337 gram sample of chromium is heated in the presence of excess oxygen. a metal oxide is formed with a mass of 9.595 g. determine
the empirical formula of the metal oxide.

Empirical formula is CrO

We are given;

We are required to determine the empirical formula of the metal oxide.

Mass of oxygen = Mass of the metal oxide - mass of the metal

                          = 9.595 g - 7.337 g

                         = 2.258 g

Moles of chromium metal

Molar mass of chromium = 51.996 g/mol

Moles of Chromium = 7.337 g ÷ 51.996 g/mol

                                 = 0.141 moles

Moles of oxygen

Molar mass of oxygen = 16.0 g/mol

Moles of Oxygen = 2.258 g ÷ 16.0 g/mol

                            = 0.141 moles

Mole ratio of Chromium to Oxygen

          Cr : O

0.141 mol : 0.141 mol

             1 : 1

Empirical formula is the simplest whole number ratio of elements in a compound.

Thus the empirical formula of the metal oxide is CrO

i believe it is c.) 1575 j.

what does the table look like