5.7 CHAPTER 5. THERMAL PROPERTIES AND IDEAL GASES
- 6 g of chlorine (Cl 2 ) occupies a volume of0.002 m^3 at a temperature of 26◦C. What is the
pressure of the gas under these conditions?
- An average pair of human lungs contains about 3.5 � of air after inhalation and about 3.0 � after
exhalation. Assuming that air in your lungs isat 37◦C and 1.0 atm, determine the number of
moles of air in a typicalbreath.
- A learner is asked tocalculate the answer tothe problem below:
Calculate the pressure exerted by 1.5 moles of nitrogen gas in a container with a volume of 20
dm^3 at a temperature of 37◦C.
The learner writes the solution as follows:
V = 20 dm^3
n = 1.5 mol
R = 8.3 J·K−^1 mol−^1
T = 37 + 273 = 310 K
pT = nRV, therefore
p =
nRV
T
=
1. 5 × 8. 3 × 20
310
= 0. 8 kPa
(a) Identify 2 mistakes the learner has made inthe calculation.
(b) Are the units of thefinal answer correct?
(c) Rewrite the solution, correcting the mistakesto arrive at the right answer.
More practice video solutions or help at http://www.everythingscience.co.za
(1.) 00xz (2.) 00y0 (3.) 00y1 (4.) 00y2
5.7 Molar volume of gases ESBBE
It is possible to calculatethe volume of a mole ofgas at STP using what we now know about gases.
- Write down the ideal gas equation
pV = nRT, therefore V =nRTp
- Record the values thatyou know, making surethat they are in SI units
You know that the gas isunder STP conditions. These are as follows:
p = 101. 3 kPa = 101300 Pa
n = 1 mol
R = 8. 3 J· K−^1 mol−^1
T = 273 K
