CHEMISTRY WKST: GAS LAWS: KMT / GRAHAM’S LAW
1)
a) 760 mmHg
b) 760 torr
c) 273.15 K
d) 14.7 psi
e) 1 atm
f) 101.325 kPa
g) 0°C
h) 29.92 inHg
2)
Ptotal = 725 torr
(
)
(
)
ntotal = 0.357 mol + 0.469 mol = 0.826 mol
3)
You will smell the rotten-egg smell of H2S first. H2S has a
molar mass of 34.09 g/mol and SO2 has a molar mass of 64.07
g/mol. The lighter the gas, the faster it moves. Therefore, H2S
will reach you before the SO2.
4)
Since kinetic energy depends on temperature, all gases at the
same temperature will have the same kinetic energy.
5)
Find the molar masses of each gas. The lighter the gas the
higher the diffusion rate.
C2H2 →
Cl2 →
H2S →
N2 →
NO2 →
CH4 →
Cl2 < NO2 < H2S < N2 < C2H2 < CH4
1
6)
 It is assumed that gas particles are dimensionless points
with no volume. This is not true, gas particles do have a
volume.
 It is assumed that gas particles do not exert attractive forces
on each other. This is not true. Gas particles will have
attractive forces between them when they collide or even get
close to each other.
7)
Real gases approach ideal gas behavior at high temperatures
and low pressures.
8)
√
√
√
O2 is 1.582 times faster than SO3
9)
√
√
√
√
x = 28.78 g
2