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Ierofanga [76]
3 years ago
7

What type(s) of intermolecular forces are expected between ch3ch2ch2ch2ch2oh molecules?

Chemistry
1 answer:
notka56 [123]3 years ago
5 0

Answer : Hydrogen-bonding, Dipole-dipole attraction and London-dispersion force.

Explanation :

The given molecule is, CH_3CH_2CH_2CH_2CH_2OH

Three types of inter-molecular forces are present in this molecule which are Hydrogen-bonding, Dipole-dipole attraction and London-dispersion force.

  • Hydrogen-bonding : when the partial positive end of hydrogen is bonded with the partial negative end of another molecule like, oxygen, nitrogen, etc.
  • Dipole-dipole attraction : When the partial positively charged part of the molecule is interact with the partial negatively charged part of the molecule. For example : In case of HCl.
  • London-dispersion force : This force is present in all type of molecule whether it is a polar or non-polar, ionic or covalent. For example : In case of Br-Br , F-F, etc

Hydrogen-bonding is present between the oxygen and hydrogen molecule.

Dipole-dipole forces is present between the carbon and oxygen molecule.

London-dispersion forces is present between the carbon and carbon molecule.

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Answer:

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Explanation:

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A sample of gas occupies a volume of 61.5 mL . As it expands, it does 130.1 J of work on its surroundings at a constant pressure
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Answer:

the final volume of the gas is V_2 = 1311.5 mL

Explanation:

Given that:

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Since the process does 130.1 J of work on its surroundings at a constant pressure of 783 Torr. Then, the pressure is external.

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P_{ext} = 1.03 \ atm

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The change in volume ΔV= \dfrac{W}{P_{ext}}

ΔV = \dfrac{130.1 \ J  \times \dfrac{1 \ L  \ atm}{ 101.325 \ J}  }{1.03 \ atm }

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Recall that the initial  volume = 61.5 mL

The change in volume V is \Delta V = V_2 -V_1

-  V_2= -  \Delta V  -V_1

multiply through by (-), we have:

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