Question

Consider this reaction involving an unknown element X. F2+2XBr⟶Br2+2XF When 1.300 g of XBr reacts, 0.7241 g of Br2 is produced. Calculate the molar mass of X, and then identify its element symbol.

Answer 1

The molar mass of X would be 63.55 g/mol and the chemical symbol of X would be Cu (copper).

From the equation of the reaction: F2+2XBr⟶Br2+2XF

The mole ratio of XBr to Br2 is 2:1

Mole of Br2 = mass/molar mass

                      = 0.7241/159.808

                       = 0.004531 mole

Mole of XBr = 2 x mole of Br2

                      = 2 x 0.004531

                        = 0.009062 mole

Molar mass of XBr = mass/mole

                            = 1.300/0.009062

                                 = 143.456 g/mol

Since the molar mass of Br is 79.904, the molar of X would be:

                             143.456 - 79.904

                                   = 63.55 g/mol

Hence, X would be Cu.

More on molar mass calculation can be found here: brainly.com/question/20691135