1 mol super cooled liquid water transformed to solid ice at -10 oC under 1 atm pressure.
1 answer:
Answer:
Explanation:
Given that:
number of moles of super cooled liquid water = 1
Melting enthalpy of ice = 6020 J/mol
Freezing point =0 °C = (0 + 273 K)= 273 K
The decrease in entropy of the system during freezing for 1 mol (i.e during transformation from liquid water to solid ice ) = - 6020 J/mol × 1 mol /273 K = -22.051 J/K
Entropy change during further cooling from 0 °C (273 K) to -10 °C (263 K)
Δ S = -1.4 J/K
Total entropy change of the system = - 22.05 J/K - 1.4 J/K = - 23.45 J/K
Entropy change of universe = entropy change of the system+ entropy change of the surrounding
According to the second law of thermodynamics
Entropy change of universe >0
SO,
Entropy change of the system + entropy change in the surrounding > 0
Entropy change in the surrounding > - entropy change of the system
Entropy change in the surrounding > - (- 23.53 J/K)
Entropy change in the surrounding > 23.53 J/K
b) Make some comments on entropy changes from the obtained data.
From the data obtained; we will realize that the entropy of the system decreases as cooling takes place when water is be convert to ice , randomness of these molecules reduces and as cooling proceeds , hence, entropy reduces more as well and the liberated heat will go into the surrounding due to this entropy of the surrounding increasing.
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27) Partial pressure of oxygen: 57.8 kPa
29) Final volume: 80 mL
30) Final volume: 8987 L
31) Due to property of water of being polar, ice floats on water
Explanation:
27)
In a mixture of gases, the total pressure of the mixture is the sum of the partial pressures:
In this problem, the mixture contains 3 gases (helium, carbon dioxide and oxygen). We know that the total pressure is
We also know the partial pressures of helium and carbon dioxide:
The total pressure can be written as
where is the partial pressure of oxygen. Therefore, we find
29)
Assuming that the pressure of the gas is constant, we can apply Charle's law, which states that:
"For an ideal gas at constant pressure, the volume of the gas is proportional to its absolute temperature"
Mathematically,
where
V is the volume of the gas
T is the Kelvin temperature
We can re-write it as
Here we have:
(initial volume)
is the initial temperature
is the final temperature
Solving for V2, we find the final volume:
30)
For this problem, we can use the equation of state for ideal gases, which can be written as
where in this problem:
is the initial pressure
is the initial volume
is the initial temperature
is the final pressure
is the final temperature
And solving for V2, we find the final volume of the balloon:
31)
A molecule of water consists of two atoms hydrogen bond with an atom of oxygen () in a covalent bond.
While the molecul of water is overall neutral, due to the higher electronegativity of the oxygen atom, electrons are slightly shifted towards the oxygen atom; as a result, there is a slightly positive charge on the hydrogen side, and a slightly negative charge on the oxygen side (so, the molecules is said to be polar).
As a consequence, molecules of water attract each other, forming the so-called "hydrogen bonds".
One direct consequence of the polarity of water is that ice floats on liquid water.
Normally, for every substance on Earth, the solid state is more dense than the liquid state. However, this is not true for water, because ice is less dense than liquid water.
This is due to the polarity of water. In fact, when the temperature of water is decreased to freezing point and water becomes ice, the hydrogen bondings "force" the molecules to arrange in a lattice structure, so that the molecules become more spaced when they turn into solid state. As a result, ice occupies more volume than water, and therefore it is less dense, being able to float on water.
Learn more about ideal gases:
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