If a sample of gas has a volume of
100.ome when the pressure is 50.ok pa,
What is the volume when the pressure
is increased to 400.0 kpa, assuroing
temperature and number of moles is held
constant
Answers
Answer:
Hi friend how are you hope u are doing well and taking good care of yourself and your family and friends. Be happy forever in your life. Have a good day. Keep smiling. May God fill your life with happiness. God bless you.
Explanation:
Please mark me as the brainliest
Answer:
One of the most amazing things about gases is that, despite wide differences in chemical properties, all the gases more or less obey the gas laws. The gas laws deal with how gases behave with respect to pressure, volume, temperature, and amount.
Pressure
Gases are the only state of matter that can be compressed very tightly or expanded to fill a very large space. Pressure is force per unit area, calculated by dividing the force by the area on which the force acts. The earth's gravity acts on air molecules to create a force, that of the air pushing on the earth. This is called atmospheric pressure.
The units of pressure that are used are pascal (Pa), standard atmosphere (atm), and torr. 1 atm is the average pressure at sea level. It is normally used as a standard unit of pressure. The SI unit though, is the pascal. 101,325 pascals equals 1 atm.
For laboratory work the atmosphere is very large. A more convient unit is the torr. 760 torr equals 1 atm. A torr is the same unit as the mmHg (millimeter of mercury). It is the pressure that is needed to raise a tube of mercury 1 millimeter.
The Gas Laws: Pressure Volume Temperature Relationships
Boyle's Law: The Pressure-Volume Law
Robert Boyle (1627-1691)
Boyle's law or the pressure-volume law states that the volume of a given amount of gas held at constant temperature varies inversely with the applied pressure when the temperature and mass are constant.
V is proportional to the inverse of P
Another way to describing it is saying that their products are constant.
PV = C
When pressure goes up, volume goes down. When volume goes up, pressure goes down.
From the equation above, this can be derived:
P1V1 = P2V2 = P3V3 etc.
This equation states that the product of the initial volume and pressure is equal to the product of the volume and pressure after a change in one of them under constant temperature. For example, if the initial volume was 500 mL at a pressure of 760 torr, when the volume is compressed to 450 mL, what is the pressure?
Plug in the values:
P1V1 = P2V2
(760 torr)(500 mL) = P2(450 mL)
760 torr x 500 mL/450 mL = P2 844 torr = P2
The pressure is 844 torr after compression.
Charles' Law: The Temperature-Volume Law