1. Identify the Possible Elements:
* You're given that the compound contains hydrogen (H), oxygen (O), and nitrogen (N).
2. Determine the Atomic Masses:
* H: 1.008 amu
* O: 15.999 amu
* N: 14.007 amu
3. Use Trial and Error (with a bit of logic):
* Start with Nitrogen: Since the molecular mass is 63.008 amu, the compound could have one nitrogen atom (14.007 amu).
* Subtract Nitrogen: This leaves 63.008 - 14.007 = 49.001 amu to account for hydrogen and oxygen.
* Oxygen: The closest we can get to 49.001 amu with oxygen is using three oxygen atoms (3 x 15.999 = 47.997 amu).
* Hydrogen: To make up the difference, we need two hydrogen atoms (2 x 1.008 = 2.016 amu).
4. The Formula:
* The formula is HNO3 (Nitric Acid)
Verification:
* 1 (N) + 1 (H) + 3 (O) = 63.008 amu (close enough to our given molecular mass)
