Hello!
First, let's see what a molar mass is. A molar mass is how much a mole weighs, or how much 6.02214076×10²³ of an element weighs.
Now, let's find the molar mass of each of these three elements.
Carbon: 12.0107 g/mol
Hydrogen: 1.00784 g/mol
Nitrogen: 14.0067 g/mol
Now, see how much of the molar mass of compound x each of these contributes.
Carbon: 44.44% * 135.13 = 60.051772 g/mol
Hydrogen: 3.73% * 135.13 = 5.040349 g/mol
Nitrogen: 51.83% * 135.13 = 70.037879 g/mol
Finally, calculate how many atoms there are in the molecule. Do this my dividing the "how much they contribute to the molar mass" by the molar mass.
Carbon: 60.051772 / 12.0107 = 5
Hydrogen: 5.040349 / 1.00784 = 5
Nitrogen: 70.037879 / 14.0067 = 5
Therefore, we know that there are 5 Carbons, 5 hydrogens, and 5 nitrogens.
Put this all together to get the molecular formula: C5H5N5 (note that the numbers should be written as subscript)
Hope this helps!
The molecular formula of the compound X is C₅H₅N₅
We'll begin by listing out what was given from the question. This includes:
Molar mass of compound = 135.13
Carbon (C) = 44.44%
Hydrogen (H) = 3.73%
Nitrogen (N) = 51.83%
Next, we shall determine the empirical formula of the compound X.
Carbon (C) = 44.44%
Hydrogen (H) = 3.73%
Nitrogen (N) = 51.83%
[tex]C = \frac{44.44}{12} = 3.703\\\\H = \frac{3.73}{1} = 3.73\\\\N = \frac{51.83}{14} = 3.702\\\\[/tex]
[tex]C = \frac{3.703}{3.702} = 1\\\\H = \frac{3.73 }{3.703} = 1\\\\N = \frac{3.702}{3.702} = 1\\\\[/tex]
Thus, the empirical formula of the compound X is CHN
Finally, we shall determine the molecular formula of X. This can be obtained as follow:
Molar mass of compound = 135.13
Empirical formula = CHN
[CHN]ₙ = 135.13
[12 + 1 + 14]n = 135.13
27n = 135.13
Divide both side by 27
[tex]n = \frac{135.13}{27}\\\\[/tex]
Molecular formula = [CHN]ₙ
Molecular formula = [CHN]₅
Therefore, the molecular formula of the compound X is C₅H₅N₅
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