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3 years ago

Which of the following would have the lowest entropy?

Chemistry

2 answers:

SpyIntel [72]3 years ago

8 0

A) diamond

Because solids has the lowest microstates

sweet [91]3 years ago

5 0

Answer:

A. Diamond

Explanation:

Entropy is an important physical quantity used in statistical mechanics and thermodynamics to measure the degree of disorder of a system. We say that the greater the entropy variation of a system, the greater its clutter, the less energy will be available for use. Entropy is related to the spontaneity of some physical or chemical process. Whenever such a process happens spontaneously, the entropy of the system will increase, ie the system will be less organized or more random.

If we compare three systems with entropy: the first with something in the liquid state, the second with something in the solid state, and the third with something in the form of vapor, we will conclude that the entropy of the third system will be greater than the others, due to the greater agitation of the molecules. Already the second system, with something in the solid state will be the system with less entropy because in this case the spacing between the molecules of this "something" is smaller and consequently the agitation of them. For this reason, as diamond is something in solid state, we can say that with the exposed options, diamond is the alternative with less entropy.

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bogdanovich [222]

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2 years ago

0.10 M potassium chromate is slowly added to a solution containing 0.20 M AgNO3 and 0.20 M Ba(NO3)2. What is the Ag+ concentrati

erastova [34]

Answer:

$[Ag^{+}]=4.2\times 10^{-2}M$

Explanation:

Given:

[AgNO3] = 0.20 M

Ba(NO3)2 = 0.20 M

[K2CrO4] = 0.10 M

Ksp of Ag2CrO4 = 1.1 x 10^-12

Ksp of BaCrO4 = 1.1 x 10^-10

$BaCrO_4 (s)\leftrightharpoons Ba^{2+}(aq)\;+\;CrO_{4}^{2-}(aq)$

$Ksp=[Ba^{2+}][CrO_{4}^{2-}]$

$1.2\times 10^{-10}=(0.20)[CrO_{4}^{2-}]$

$[CrO_{4}^{2-}]=\frac{1.2\times 10^{-10}}{(0.20)}= 6.0\times 10^{-10}$

Now,

$Ag_{2}CrO_4(s) \leftrightharpoons 2Ag^{+}(aq)\;+\;CrO_{4}^{2-}(aq)$

$Ksp=[Ag^{+}]^{2}[CrO_{4}^{2-}]$

$1.1\times 10^{-12}=[Ag^{+}]^{2}](6.0\times 10^{-10})$

$[Ag^{+}]^{2}]=\frac{1.1\times 10^{-12}}{(6.0\times 10^{-10})}= 1.8\times 10^{-3}$

$[Ag^{+}]=\sqrt{1.8\times 10^{-3}}=4.2\times 10^{-2}M$

So, BaCrO4 will start precipitating when [Ag+] is 4.2 x 1.2^-2 M

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3 years ago

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3 years ago

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3 years ago

Based on the ideal gas law, there is a simple equivalency that exists between the amount of gas and the volume it occupies. at s

nordsb [41]

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3 years ago