1. Real gases behave like ideal gases except at very high temperatures. 2. The gas constant, R, is equal to 0.0821 when the pressure is expressed in kilopascals. 3. As more gas particles are added to a container, there are fewer collisions because the particles don't go as far. 4. The number of moles of a gas is inversely proportional to its volume at STP. 5. Real gases behave like ideal gases except at very high pressure. 6. At a constant temperature, the pressure exerted by one mole of a gas decreases if the volume available is increased. 7. The ideal gas equation will only give correct values if the temperature in expressed in degrees Celcius. 8. One mole of oxygen at 760. mm Hg and 0 °C occupies a volume of one L. Matching: Match each variable listed on the left with the appropriate unit of measurement listed on the right. You may write one or more letters on each line. Circle the ones used in the Ideal Gas Equation. 9. number of moles 10. volume 11. pressure 12. temperature A. °C B. kg C. mol D. mm Hg E. K F. L G. atm H. Pa 1. °F J. m' K. cm³ L. kPa M. torr

1. Real gases behave like ideal gases except at very high temperatures. 2. The gas constant, R, is equal to 0.0821 when the pressure is expressed in kilopascals. 3. As more gas particles are added to a container, there are fewer collisions because the particles don't go as far. 4. The number of moles of a gas is inversely proportional to its volume at STP. 5. Real gases behave like ideal gases except at very high pressure. 6. At a constant temperature, the pressure exerted by one mole of a gas decreases if the volume available is increased. 7. The ideal gas equation will only give correct values if the temperature in expressed in degrees Celcius. 8. One mole of oxygen at 760. mm Hg and 0 °C occupies a volume of one L. Matching: Match each variable listed on the left with the appropriate unit of measurement listed on the right. You may write one or more letters on each line. Circle the ones used in the Ideal Gas Equation. 9. number of moles 10. volume 11. pressure 12. temperature A. °C B. kg C. mol D. mm Hg E. K F. L G. atm H. Pa 1. °F J. m' K. cm³ L. kPa M. torr

College Physics

11th Edition

ISBN:9781305952300

Author:Raymond A. Serway, Chris Vuille

Publisher:Raymond A. Serway, Chris Vuille

Chapter1: Units, Trigonometry. And Vectors

Section: Chapter Questions

Problem 1CQ: Estimate the order of magnitude of the length, in meters, of each of the following; (a) a mouse, (b)...

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Concept explainers

Kinetic Theory of Gas

The Kinetic Theory of gases is a classical model of gases, according to which gases are composed of molecules/particles that are in random motion. While undergoing this random motion, kinetic energy in molecules can assume random velocity across all directions. It also says that the constituent particles/molecules undergo elastic collision, which means that the total kinetic energy remains constant before and after the collision. The average kinetic energy of the particles also determines the pressure of the gas.

P-V Diagram

A P-V diagram is a very important tool of the branch of physics known as thermodynamics, which is used to analyze the working and hence the efficiency of thermodynamic engines. As the name suggests, it is used to measure the changes in pressure (P) and volume (V) corresponding to the thermodynamic system under study. The P-V diagram is used as an indicator diagram to control the given thermodynamic system.

Question

True and False: If the statement is true, write "true." If it is false, change the underlined word or
words to make the statement true. Write your answer on the line provided.
1. Real gases behave like ideal gases except at very high temperatures.
2. The gas constant, R, is equal to 0.0821 when the pressure is expressed in
kilopascals.
3. As more gas particles are added to a container, there are fewer collisions
because the particles don't go as far.
4. The number of moles of a gas is inversely proportional to its volume at
STP.
5. Real gases behave like ideal gases except at very high pressure.
6. At a constant temperature, the pressure exerted by one mole of a gas
decreases if the volume available is increased.
7. The ideal gas equation will only give correct values if the temperature in
expressed in degrees Celcius.
8. One mole of oxygen at 760. mm Hg and 0 °C occupies a volume of one L.
Matching: Match each variable listed on the left with the appropriate unit of measurement listed on the
right. You may write one or more letters on each line. Circle the ones used in the Ideal Gas
Equation.
9. number of moles
10. volume
11. pressure
12. temperature
A. °C
B. kg
C. mol
D. mm Hg
E. K
F. L
Vo = 252ML
AT: 11
C= 190 x 10-6 /oc
AEVO XCX
G. atm
H. Pa
1. °F
J. m'
K. cm³
L. kPa
M. torr
2
(252x 190x
Av=0.555mL

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