Question

The molecular mass of a compound is 92 g/mol. Analysis of the compound shows that it consists of 0.608 g of N and 1.388 g of O. What is its empirical and molecular formula?
pls help and show work

Answer 1

The empirical and molecular formula would be  $NO_2$ and  $N_2O_4$ respectively.

Empirical formula

The compound contains N and O.

N                                                        O

0.608/14 = 0.0434                        1.388/16 = 0.0867

Divide by the smallest.

N = 1                                             O = 2

Thus, the empirical formula would be $NO_2$

To get the molecular formula:

Empirical formula mass = 14 + (16x2) = 46

n = molar mass/empirical formula mass

          = 92/46 = 2

Thus, the molecular formula would be $N_2O_4$

More on empirical formulas can be found here: brainly.com/question/14044066

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