Draw a highly magnified view of a sealed, rigid container filled with a gas. Then draw what it would look like if you cooled the
gas significantly but kept the temperature above the boiling point of the substance in the container. Also draw what it would look like if you heated the gas significantly. Finally, draw what each situation would look like if you evacuated enough of the gas to decrease the pressure by a factor of 2.
1 answer:
Answer:
In order to fully understand the issue of the ideal gas or perfect gas, we must pay attention to the following, an ideal or perfect gas does not really exist, it is a hypothetical gas whose sharing of the variables of pressure, volume and temperature can be fully described by the ideal gas equation.
The molecules that make up an ideal gas do not usually attract or repel each other, and their volume is negligible compared to the volume of the container that contains it. Although in our nature the case of an ideal gas does not exist, the differences between the behavior of a real gas in temperature and pressure margins do not substantially alter the calculations, so we can make use of the equation with all the security, to solve various gas exercises.
Explanation:
The collisions that occur between the molecules and with the molecules and with the walls is elastic because the moment is preserved, in addition to the kinetic energy.
It can be synthesized that a gas is ideal when all collisions that occur between atoms or molecules are completely elastic and there are no attractive forces that are intermolecular.
In ideal gases the kinetic energy is proportional to its temperature. The gases approach an ideal gas if they are mono atomic gases, if it is under pressure and also at room temperature.
The amount of gas in a body is measured in moles. One mole of any type of gas reaches 22.4 liters, in normal condition, 0 ° Celsius and 1 of the pressure atmosphere. That volume is called normal molar volume.
Ideal gases have an equation called the Ideal Gas Equation and is based on three main laws that are Boyle's law, Gay-Lussac's law, Charles's law and also Avogadro's law.
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Answer:
Approximately formula units (
).
Explanation:
Refer to a modern periodic table for the relative atomic mass of magnesium () and chlorine (
):
:
.
:
.
In other words, the mass of of
atoms would be (approximately)
.
Likewise, the mass of of
atoms would be approximately
.
One formula unit of the ionic compound includes exactly as many atoms as there are in the given formula. The formula mass of a compound is the mass of
of the formula units of this compound.
The formula includes one
atom and two
atoms.
Hence, every formula unit of would include the same number of atoms: one
atom and two
atoms. There would be
of
atoms and
of
atoms in
of
formula units.
Thus, the mass of of
formula units would be equal to the mass of
of
atoms plus the mass of
of
atoms. (The mass of
of each atom could be found from the relative atomic mass of each element.)
.
In other words, the formula mass of is
.
Therefore, the number of formula units in of
would be:
.
Multiple by Avogadro's Number
to estimate the number of formula units in
:
.