Answer : Carbon tetrachloride,
will show the greatest freezing point lowering.
Explanation :
For non-electrolyte solution, the formula used for lowering in freezing point is,
![\Delta T_f=k_f\times m](https://tex.z-dn.net/?f=%5CDelta%20T_f%3Dk_f%5Ctimes%20m)
where,
= lowering in freezing point
= molal depression constant
m = molality
As per question, the molality is same for all the non-electrolyte solution. So, the lowering in freezing point is depend on the
only.
That means the higher the value of
, the higher will be the freezing point lowering.
From the given non-electrolyte solutions, the value of
of carbon tetrachloride is higher than the other solutions.
Therefore, Carbon tetrachloride,
will show the greatest freezing point lowering.
Answer:
0.400 M
Explanation:
The reaction given is
H₂(g) + Br₂(g) ⇄ 2HBr(g)
So, the stoichiometry is 1 mol of H₂ for 1 mol of Br₂ to form 2 moles of HBr.
By the molas masses given, the number of moles of each compound is (mass/molar mass):
nH₂ = 1.374/2.0159 = 0.681581427 mol
nBr₂ = 70.31/159.81 = 0.439959952 mol
The number of moles of H₂ in the equilibrium will be:
nH₂e = 0.566/2.0159 = 0.280767895 mol
So the number of moles that reacts is the initial less the equilibrium:
n = 0.400813531 mol
For the stoichiometry, the number of moles that is formed of HBr must be double, which will be the number of moles in equilibrium:
nHBr = 0.801627063
The molar concentration is the number of moles divided by the volume:
0.801627063/2.00
0.400 M
Answer:
The precautionary principle would prevent the implementation of technologies that possess a risk to humans, animals, and the environment. The strengths are that it will definately save the population and planet from a new technology that could cause long-term harm.
The weakness is that this principle may inhibit new technologies that are needed to help under-developed countries from preventing diseases. The precautionary principle states that technologies should entirely risk-free.
Explanation:
Both of you are overlooking a pretty big component of the question...the Group I cation isn't being dissociated into water. We're testing the solubility of the cation when mixed with HCl. And this IS a legitimate question, seeing as our lab manual is the one asking.
<span>By the way, the answer you're looking for is "Because Group I cations have insoluble chlorides". </span>
<span>"In order...to distinguish cation Group I, one adds HCl to a sample. If a Group I cation is present in the sample, a precipitate will form." </span>
Answer: Your answer is, <u>close to the freezing point, the water molecules start to arrange locally into ice-like structures. This creates some "openness" in the liquid water, which tends to decrease its density.</u>
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Hope this helps!