An unopened can of soda pop explodes if left in the hot sun. Which two properties change while it is in the sun? A. Temperature B. Volume C. Pressure D. Quantity of gas molecules
Ideal and Real Gases
Ideal gases obey conditions of the general gas laws under all states of pressure and temperature. Ideal gases are also named perfect gases. The attributes of ideal gases are as follows,
Gas Laws
Gas laws describe the ways in which volume, temperature, pressure, and other conditions correlate when matter is in a gaseous state. The very first observations about the physical properties of gases was made by Robert Boyle in 1662. Later discoveries were made by Charles, Gay-Lussac, Avogadro, and others. Eventually, these observations were combined to produce the ideal gas law.
Gaseous State
It is well known that matter exists in different forms in our surroundings. There are five known states of matter, such as solids, gases, liquids, plasma and Bose-Einstein condensate. The last two are known newly in the recent days. Thus, the detailed forms of matter studied are solids, gases and liquids. The best example of a substance that is present in different states is water. It is solid ice, gaseous vapor or steam and liquid water depending on the temperature and pressure conditions. This is due to the difference in the intermolecular forces and distances. The occurrence of three different phases is due to the difference in the two major forces, the force which tends to tightly hold molecules i.e., forces of attraction and the disruptive forces obtained from the thermal energy of molecules.
![To do first experiment, pump the gas pump to put gas into the chamber. Only
use between 3 and 7 pumps. Increase the temperature to a number you
like between 100 K and 500 K, using the fire/ice bucket on bottom. Do
not change the chamber width for now, keep it at 10.0 nm (handle on left
of chamber). Do not open the chamber to let gas molecules out (handle
on top of chamber).
Calculating moles using the Ideal Gas Law: PV = nRT, where R =
0.0821
Once you have everything how you like it, you will calculate how many moles of gas are in the
chamber, by using the Ideal Gas Law. Recall the Ideal Gas Law requires specific units: atm, L,
moles, and Kelvin.
Pressure
Is indicated by the circular instrument on the top right of the
chamber. It is conveniently already in atmospheres.
Volume
- Determine the volume in nm^3 by multiplying the width, height, and depth of the
chamber. Depth is always 1.00 nm and height is always 10.0 nm. Width is adjusted by you to
10.0 nm or 15.0 nm, depending on the experiment. Volume then is: width you adjust X 10.0
nm X 1.00 nm. Simplifying, it is the width you select X 10.0, with units of nm^3. To simplify
calculations assume your volume answer in nm^3 are actually Liters (L),
when calculating the Ideal Gas Law.
Temperature - This is indicated by the thermometer, conveniently
already in units Kelvin.
Quantity – for these experiments you will be calculating the quantity, or
moles, of gas under each scenario. What is the solution when you solve
the Ideal Gas Law, PV=nRT, for n, moles? R = 0.0821.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F6f1e8666-0358-4f82-8394-bfae4d254ad0%2F5eee605c-af40-466c-901c-23baf58b089f%2Fb7vn3v_processed.jpeg&w=3840&q=75)
![QUESTION 11
An unopened can of soda pop explodes if left in the hot sun. Which two
properties change while it is in the sun?
A. Temperature
B. Volume
C. Pressure
D. Quantity of gas molecules](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F6f1e8666-0358-4f82-8394-bfae4d254ad0%2F5eee605c-af40-466c-901c-23baf58b089f%2Fucykgga_processed.jpeg&w=3840&q=75)
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