3. (a) The nitrogen oxide (NO) molecule has a bond length of 140 pm. Calculate the dipole moment, in Debyes, that results if the
charges on N and O were 2 and 2-, respectively. (Include the formula for the calculation in your solution)(b) If the experimentally measured dipole moment is 1.85 D, what is the magnitude (in units of e') of the charges on N and O. (Include the equation in your solution)
1 answer:
Answer:
The calculations is shown in the attached file.
Explanation:
- The concept of dipole moment is applied here. the size of the dipole moment is given by multiplying the size of the charge by the distance apart.
- For simpler molecules, the sizes of the dipole moments are approximately proportional to the difference between the electronegativities of the atoms. Dipole moments are usually measured in debyes (D).
Dipole moments (μ) = q x r
The detailed calculation is shown in the attachment.
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The number of moles in each sample will be 0.391 moles, 30.7 moles, 0.456 moles, and 1350 moles
<h3>What is the number of moles?</h3>The number of moles of a substance is the ratio of the mass of the substance to the molar mass.
In other words; mole = mass/molar mass.
Thus:
- moles of 18.0 g
= 18.0/46
= 0.391 moles
- moles of 1.35 kg
= 1350/44
= 30.7 moles
- moles of 46.1 g
= 46.1/101.1
= 0.456 moles
- moles of 191.8 kg
= 191800/142
= 1350 moles
More on the number of moles of substances can be found here: brainly.com/question/1445383
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