What is the empirical formula of a compound that contains 43.38% sodium, 11.33% carbon, and 45.29% oxygen

Let the total weight of compound is 100 grams

the mass of sodium = 43.38 grams

moles of sodium = mass /  atomic mass = 43.38/ 23 = 1.88

mass of carbon = 11.33 grams

moles of carbon = mass / atomic mass = 11.33/12 = 0.944

mass of oxygen = 45.29

moles of oxygen = mass / atomic mass = 45.29 / 16 = 2.83

Let us divide each moles with the lowest moles to get a ratio of whole number

moles of sodium = 1.88/0.944 = 2

moles of carbon = 0.944/0.944 = 1

moles of oxygen = 2.83/0.944 = 3

so the empirical formula is Na₂CO₃

explanation:

two years ago, when picking flowers in the mountains back of yosemite valley, i found a book. it was blotted and storm-beaten; all of its outer pages were mealy and crumbly. the paper seemed to dissolve like the snow beneath which it had been buried, however; many of the inner pages were well preserved. and although all were more or less stained and torn, whole chapters were easily readable. this is the condition of the great open book of yosemite glaciers today; its granite pages have been torn and blurred by the same storms that wasted the castaway book.

two years ago, when picking flowers in the mountains back of yosemite valley; i found a book. it was blotted and storm-beaten, all of its outer pages were mealy and crumbly. the paper seemed to dissolve like the snow beneath which it had been buried, however, many of the inner pages were well preserved. and although all were more or less stained and torn; whole chapters were easily readable. this is the condition of the great open book of yosemite glaciers today, its granite pages have been torn and blurred by the same storms that wasted the castaway book.