Chemistry 105A - Chapter 10 Problems - DUE IN CLASS 12/2/2009
Show your work and complete the following problems. Work independently but take advantage
of your notes and textbook as necessary just no other human help.
1. A sample of gas (24.2 g) initially at 4.00 atm was compressed from 8.00 L to 2.00 L at
constant temperature. Determine the pressure after the compression.
1 1 2 2
1 1
2
2
P V = P V
4.00 atm 8.00 L
P V
P = = 16 atm
V 2.00 L
2. A sample of H2 gas (12.28 g) occupies 100.0 L at 400.0 K and 2.00 atm. A sample
weighing 9.49 g occupies what volume at 353 K and 2.00 atm.
1 1 2 2
1 2
2 2
2 1
1 1
P nT
PV = nRT =
R V
n T n T
=
V V
1 mole
9.49 g × 353.0 K
2 g
n T
V = V = × 100.0 L
n T 1 mole
12.28 g × 400.0 K
2 g
= 68.2 L
You would not have to convert to mo
L atm
K mole
les since this cancels in the numerator and denominator.
OR with the use of the ideal gas constant:
1 mole
9.49 g × 0.08206 353.0 K
2.016 g
nRT
V = = 68.2 L
P 2 atm
3. Automobile air bags use the decomposition of sodium azide as their source of gas for
rapid inflation: 2NaN3 (s) 2Na(s) + 3N2(g)
Answers Chapter 10 problems 1
