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balu736 [363]
2 years ago
14

A hydrogen bond can occur between:

Chemistry
1 answer:
Readme [11.4K]2 years ago
5 0

A hydrogen bond occurs between a hydrogen from one molecule and an oxygen from another molecule. Option D

<h3>What is the hydrogen bond?</h3>

The hydrogen bond is one that is responsible for association in molecules. It occurs when hydrogen is covalently bonded to a highly electronegative element such as oxygen, nitrogen or Sulphur.

Thus, a hydrogen bond occurs between a hydrogen from one molecule and an oxygen from another molecule. Option D

Learn more about hydrogen bonding:brainly.com/question/10904296?

#SPJ1

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Please help me with this question please!!!
Deffense [45]

Answer:

A

Explanation:

I looked up aromatic hydrocarbon and this one looks like a replica of benzene

3 0
3 years ago
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sasho [114]

I would say it is answer choice C, Laws are based on proven hypothesis by many different scientists.

4 0
2 years ago
Calculate the volume of a 0.225M solution of KOH required to react with 0.215g of acetic acid.
Sidana [21]
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7 0
3 years ago
Read 2 more answers
If 5.100 g of c6h6 is burned and the heat produced from the burning is added to 5691 g of water at 21 °c, what is the final temp
emmasim [6.3K]
  <span>C6H12 = 6x12 + 6x1 = 78. 
The equation indicates that 2x78 = 156g benzene will produce 6542kJ. 
Using proportions you can then calculate that 
x/6542kJ = 7.9g / 156g 
x = 331.3kJ = 331300J. 

heat = mass x ΔT x 4.18J/g° 
ΔT = 331300J / (5691g x 4.18J/g°) = 13.9° 

final temp = 21 + 14° = 35°C</span>
4 0
3 years ago
A gas sample occupies 350.0 mL at 546 mm Hg. What volume does the gas occupy at 652 mm Hg?​
leva [86]

Answer:

293.1 mL.

Explanation:

  • Boyle's law states that: at a constant temperature the pressure of a given mass of an ideal gas is inversely proportional to its volume.
  • It can be expressed as: <em>P₁V₁ = P₂V₂,</em>

P₁ = 546.0 mm Hg, V₁ = 350.0 mL.

P₂ = 652.0 mm Hg, V₂ = ??? mL.

<em>∴ V₂ = (P₁V₁)/(P₂)</em> = (546.0 mm Hg)(350.0 mL) / (652.0 mm Hg) = <em>293.1 mL.</em>

8 0
3 years ago
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