The empirical and molecular formula would be 
and 
respectively.
<h3>Empirical formula</h3>
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
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
More on empirical formulas can be found here: brainly.com/question/14044066
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Answer:
Please did you ever get an answer??
Explanation:
Im doing usa test prep too and its really late
It varies with container, temperature, pressure and amount of gas. But, the volume occupied by a gas at a fixed temperature and pressure remains constant which is 22.4 L for 1 mole at STP.
Answer:
Mass of oxygen required = 19.5 moles × 16 g/mol = 312 g.
Explanation:
Answer & Explanation:
D orbitals begin filling with electrons after the orbital found in the 4s sublevel is filled. This occurs because the d sublevel is first found in the.
