Bond energies do not account for the energy associated with the formation of aqueous solutions. Explain what energy is not accou
1 answer:
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Answer :
The number of bonding pairs of electrons around the hydrogen atom = 2
The number of lone pairs of electrons around the hydrogen atom = 0
Explanation :
Lewis-dot structure : It shows the bonding between the atoms of a molecule and it also shows the unpaired electrons present in the molecule.
In the Lewis-dot structure the valance electrons are shown by 'dot'.
The given molecule is,
As we know that carbon has '4' valence electrons, hydrogen has '1' valence electrons and nitrogen has '5' valence electrons.
Therefore, the total number of valence electrons in = 1 + 4 + 5 = 10
According to Lewis-dot structure we conclude that, there are 8 number of bonding electrons and 2 number of non-bonding electrons.
The number of bonding pairs of electrons around the hydrogen atom = 2
The number of lone pairs of electrons around the hydrogen atom = 0
Answer:
(B) 42.1%
Explanation:
The formula for the calculation of moles is shown below:
Given: For
Given mass = 15.5 g
Molar mass of = 78.0452 g/mol
<u>Moles of = 15.5 g / 78.0452 g/mol = 0.1986 moles</u>
Given: For
Given mass = 12.1 g
Molar mass of = 159.609 g/mol
<u>Moles of = 12.1 g / 159.609 g/mol = 0.0758 moles</u>
According to the given reaction:
1 mole of react with 1 mole of
0.1986 mole of react with 0.1986 mole of
Available moles of = 0.0758 moles
Limiting reagent is the one which is present in small amount. Thus, is limiting reagent. (0.0758 < 0.1986)
The formation of the product is governed by the limiting reagent. So,
1 mole of gives 1 mole of
0.0758 mole of gives 0.0758 mole of
Molar mass of = 95.611 g/mol
Mass of = Moles × Molar mass = 0.0758 × 95.611 g = 7.2473 g
Theoretical yield = 7.2473 g
Given experimental yield = 3.05 g
% yield = (Experimental yield / Theoretical yield) × 100 = (3.05/7.2473) × 100 = 42.1 %
<u>Option B is correct.</u>