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Reptile [31]
3 years ago
7

*CHEMISTRY*

Chemistry
1 answer:
Troyanec [42]3 years ago
8 0

Answer:

1.54 liters.

Explanation:

If the liters increases by .27 for every 100ºC, then just multiply .27 by 2.

You'd then get 1.54, which is your answer.

Hope this helps!

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What is the predominant intermolecular force in the liquid state of each of these compounds: ammonia (NH3), methane (CH4), and n
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Answer:

The  predominant intermolecular force in the liquid state of each of these compounds:

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methane (CH4)

and nitrogen trifluoride (NF3)

Explanation:

The types of intermolecular forces:

1.Hydrogen bonding: It is a weak electrostatic force of attraction that exists between the hydrogen atom and a highly electronegative atom like N,O,F.

2.Dipole-dipole interactions: They exist between the oppositely charged dipoles in a polar covalent molecule.

3. London dispersion forces exist between all the atoms and molecules.

NH3 ammonia consists of intermolecular H-bonding.

Methane has London dispersion forces.

Because both carbon and hydrogen has almost similar electronegativity values.

NF3 has dipole-dipole interactions due to the electronegativity variations between nitrogen and fluorine.

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Physisorption is reversible in nature and occurs at low temperatures.

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Thus, we can conclude that on increasing temperature at which adsorption is carried out decreases the extent of physisorption.

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