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Masteriza [31]
3 years ago
5

Which of the following will have the slowest rate of diffusion at a given temperature?

Chemistry
1 answer:
marysya [2.9K]3 years ago
8 0
<h3>Answer:</h3>

Chlorine gas (Cl₂)

<h3>Explanation:</h3>
  • According to the Graham's law of diffusion, the diffusion rate of a gas is inversely proportional to the square root of its density or molar mass.
  • Therefore, a lighter gas will diffuse faster at a given temperature compared to a heavy gas.
  • Consequently, the heavier a gas is then the denser it is and the slower it diffuses at a given temperature and vice versa.

In this case we are given gases, CI₂

, H₂,He and Ne.

  • We are required to identify the gas that will diffuse at the slowest rate.
  • In other words we are required to determine the heaviest gas.

Looking at the molar mass of the gases given;

Cl₂- 70.91 g/mol

H₂- 2.02 g/mol

He - 4.00 g/mol

Ne- 20.18 g/mol

Therefore, chlorine gas is the heaviest and thus will diffuse at the slowest rate among the choices given.

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Classify each of these soluble solutes as a strong electrolyte, a weak electrolyte, or a nonelectrolyte. solutes formula hydroio
Andreyy89
The correct classification of the solutes are as follows:

<span>hydroiodic acid hi                           =   strong electrolyte
calcium hydroxide ca(oh)2             =   weak electrolyte 
hydrofluoric acid hf                         =   weak electrolyte
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Strong electrolytes are substances that completely ionizes in aqueous solution while weak electrolytes are those that partially ionizes. Non electrolytes are substances that cannot conduct electric charge since there are no ions in the solution.</span>
6 0
2 years ago
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How many moles of sodium bicarbonate are in 1.50 kg of the compound?
salantis [7]

Answer:

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Explanation:

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We need to find the no of moles in 1.5 kg of Sodium bicarbonate . We know that, no of moles is equal to given mass divided by molar mass.

n=\dfrac{m}{M}\\\\n=\dfrac{1500}{84.007 }\\\\n=17.85

<h2>So, there are 17.85 moles in 1.5 kg of Sodium bicarbonate.</h2>
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Answer:

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