Answer:
CH₄
Explanation:
CH₃OH has hydrogen bonding due to the OH group present
NH₃ also has hydrogen bonding due to the NH bonds
H₂S has dipole-dipole forces present due to the polar SH bonds
HCl also has dipole-dipole forces due to the polar HCl bond
Empirical formula is the simplest ratio of components making up a compound.
The percentage composition of each element has been given
therefore the mass present of each element in 100 g of compound is
B N H
mass 40.28 g 52.20 g 7.53 g
number of moles
40.28 g / 11 g/mol 52.20 g / 14 g/mol 7.53 g / 1 g/mol
= 3.662 mol = 3.729 mol = 7.53 mol
divide the number of moles by the least number of moles, that is 3.662
3.662 / 3.662 3.729 / 3.662 7.53 / 3.662
= 1.000 = 1.018 = 2.056
the ratio of the elements after rounding off to the nearest whole number is
B : N : H = 1 : 1 : 2
therefore empirical formula for the compound is B₁N₁H₂
that can be written as BNH₂
Answer:
0.1 mole of CH₄
Explanation:
From the question given above, the following data were obtained:
Volume of CH₄ = 2.24 L
Number of mole of CH₄ =?
The number of mole of CH₄ can be obtained as follow:
Recall:
1 mole of a gas occupy 22.4 L at stp. This implies that 1 mole of CH₄ occupies 22.4 L at stp.
22.4 L = 1 mole of CH₄
Therefore,
2.24 L = 2.24 × 1 mole of CH₄ / 22.4
2.24 L = 0.1 mole of CH₄.
Answer: The electronic configuration of nitrogen is 1s2 2s2 2p3. Thus nitrogen has a half-filled p orbital, which is comparatively more stable. Thus the p orbital is the outermost orbital. To achieve a stable gas configuration, nitrogen needs to have a fulfilled p orbital.
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