How many molecules are in 25g of Na2SO4? POINTS!! Please help! Im so frustrated.

1 answer:

6 0

Hey there!

Molar mass Na2SO4 = 142.04 g/mol

Number of moles:

n = m / mm

n = 25 / 142.04

n = 0.176 moles of Na2SO4

Therefore, use the Avogadro constant

1 mole Na2SO4 ------------------- 6.02x10²³ molecules
0.176 moles Na2SO4 ------------ molecules ??

0.176 x ( 6.02x10²³ ) / 1

=> 1.059x10²³ molecules of Na2SO4

hope this helps!

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$C_{4}H_{10}$ is the molecule will undergo only London dispersion forces when interacting with other molecules of the same kind.

What are London dispersion forces?

A sort of force that interacts between atoms and molecules that is often electrically symmetric is referred to as a London dispersion force.
When viewed from the nucleus, their electron distribution is frequently symmetrical. This dispersion force, which is also known as a transient attractive force, is frequently observed when the locations of the electrons in two nearby atoms cause the atoms to temporarily form dipoles.
The bond is polar when there are significant variations between the elements' electronegativities; it is nonpolar when there are similarities. When the molecule's dipole moment is equal to O, it is nonpolar; when it differs from O, it is polar.
The force at these molecules is known as the London dispersion force. In nonpolar molecules, the forces are weak, and partial charges must be induced so that they can bond. In polar molecules, partial charges caused by polarity result in a stronger link known as a dipole-dipole. The dipole-dipole is significantly stronger and known as a hydrogen bond if it is connected to a large electronegative atom (F, O, or N). Ionic force is the name for the attraction force at ionic substances.
The intermolecular force in the letter an is the London dispersion force because the compound is nonpolar;

Reason for incorrect options:

b: the compound is ionic because Na is a metal and the other part is covalent,

c: two compounds are possible: one is nonpolar and exhibits London dispersion force; the other is polar and exhibits dipole-dipole force; and

d: both compounds exhibit hydrogen bonds (H bonded to O, and H bonded to F).

NOTE: Your question is incomplete, but most probably your full question was, which molecule will undergo only London dispersion forces when interacting with other molecules of the same kind? Which molecule will undergo only London dispersion forces when interacting with other molecules of the same kind?

A. $C_{4}H_{10}$

B. $NaC_{2}H_{3}O_{2}$