Assume that you have a cylinder with a movable piston. What would happen to the gas pressure inside the cylinder if you do the f
1 answer:
Answer:
A. The pressure will increase 4 times. P₂ = 4 P₁
B. The pressure will decrease to half its value. P₂ = 0.5 P₁
C. The pressure will decrease to half its value. P₂ = 0.5 P₁
Explanation:
Initially, we have n₁ moles of a gas that occupy a volume V₁ at temperature T₁ and pressure P₁.
<em>What would happen to the gas pressure inside the cylinder if you do the following?</em>
<em />
<em>Part A: Decrease the volume to one-fourth the original volume while holding the temperature constant. Express your answer in terms of the variable P initial.</em>
V₂ = 0.25 V₁. According to Boyle's law,
P₁ . V₁ = P₂ . V₂
P₁ . V₁ = P₂ . 0.25 V₁
P₁ = P₂ . 0.25
P₂ = 4 P₁
<em>Part B: Reduce the Kelvin temperature to half its original value while holding the volume constant. Express your answer in terms of the variable P initial.</em>
T₂ = 0.5 T₁. According to Gay-Lussac's law,
<em>Part C: Reduce the amount of gas to half while keeping the volume and temperature constant. Express your answer in terms of the variable P initial.</em>
n₂ = 0.5 n₁.
P₁ in terms of the ideal gas equation is:
P₂ in terms of the ideal gas equation is:
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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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