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geniusboy [140]
2 years ago
8

What kind(s) of intermolecular forces exist in the compounds given below? (a) CH3CH2CH2CH2CH3(l) dispersion forces dipole-dipole

forces hydrogen bonding (c) H2CO(l) dispersion forces dipole-dipole forces hydrogen bonding (b) CH3CH2OH(l) dispersion forces dipole-dipole forces hydrogen bonding (d) O2(l) dispersion forces dipole-dipole forces hydrogen bonding
Chemistry
1 answer:
Ira Lisetskai [31]2 years ago
7 0

Answer:

(a) CH3CH2CH2CH2CH3(l)

  • dispersion

(b) CH3CH2OH(l)

  • Dipole-dipole interaction
  • Dispersion forces
  • Hydrogen bonding

(c) H2CO(l)

  • Dipole-dipole
  • Dispersion

(d) O2(l)

  • Dispersion

Explanation:

Dispersion forces are those forces that occur between two non polar molecules.They form the weakest bonds.Here electrons of one molecule is attracted to the nucleus of the other molecule. Example are;

  • Interaction of two methyl (-CH₃) group
  • Interaction between nitrogen gas , N₂ molecules
  • Interaction between oxygen gas ,O₂ molecules

Dipole-Dipole interaction happens when two polar molecules interact.Positive charges in one molecule is attracted to negative charge of another molecule.Examples

  • Chloroform (CHCl₃)
  • Ammonia (NH₃)

Hydrogen bonding are created when an hydrogen atom bonded to an electronegative atom is attracted to a another electronegative atom.Example is the hydrogen bond between oxygen atom and hydrogen is water (H₂O).

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Design an invitation you could use to calculate the density of a penny
Nataliya [291]
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7 0
3 years ago
A certain gas at 2oC and 1.00 atm pressure fills a 4.0 container. What volume will the gas occupy at 100oC and 780 torr pressure
artcher [175]

The final volume V₂=4.962 L

<h3>Further explanation</h3>

Given

T₁=20 + 273 = 293 K

P₁= 1 atm

V₁ = 4 L

T₂=100+273 = 373 K

P₂=780 torr=1,02632 atm

Required

The final volume

Solution

Combined gas law :

P₁V₁/T₁=P₂V₂/T₂

Input the value :

V₂=(P₁V₁T₂)/(P₂T₁)

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6 0
3 years ago
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Yuki888 [10]

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Explanation:

5 0
2 years ago
A compound is composed of 13% carbon, 4.3% hydrogen, 30.4% nitrogen, and 52.2% oxygen. The mystery compound has a molar mass of
vredina [299]

Answer:

C₂H₈N₄O₆ is the molecular formula for the compound

Explanation:

Data from the problem:

13 g of C in 100 g of compound

4.3 g of H in 100 g of compound

30.4 g of N in 100 g of compound

52.2 g of O in 100 g of compound

Firstly we determine, the mass of each in 184 g of compound, which is 1 mol

(13 g / 100 g) . 184 g  = 24 g C

(4.3 g  / 100 g) . 184 g  = 7.91 g H ≅ 8 g H

(30.4 g / 100 g) . 184 g  = 56 g N

(52.2 g  / 100 g) . 184 g  = 96 g O

And now, we divide the mass by the molar mass of each to determine the moles:

24 g C / 12 g/mol = 2 mol C

8g H / 1 g/mol = 8 mol H

56 g N / 14 g/mol = 4 mol N

96 g O / 16 g/mol = 6 mol O

So the molecular formula of the compound is C₂H₈N₄O₆

8 0
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Strong electrolytes  are completely ionised in solution.
Weak ones are only partially ionised.
Non electrolytes do not  form ions
3 0
3 years ago
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