UNIT 6: Gaseous State - Online Test
Q1. Gases
deviate from ideal behavior at high pressure. Which of the following
statement(s) is correct for non-ideality?
Answer : Option D
Explaination / Solution:
No Explaination.
Q2. Rate
of diffusion of a gas is
Answer : Option D
Explaination / Solution:
No Explaination.
Q3. Which
of the following is the correct expression for the equation of state of van der
Waals gas?
Answer : Option C
Explaination / Solution:
No Explaination.
Q4. When
an ideal gas undergoes unrestrained expansion, no cooling occurs because the
molecules
Answer : Option B
Explaination / Solution:
No Explaination.
Q5. Equal
weights of methane and oxygen are mixed in an empty container at 298 K. The
fraction of total pressure exerted by oxygen is
Answer : Option A
Explaination / Solution:
mass of methane
= mass of oxygen = a
number of moles of methane = a/16
number of moles of Oxygen = a/32
mole fraction of Oxygen =
=[a/32] / [{a/16} + {a/32{ ]
= [a/32] / [3a/32]
=1/32
Partial pressure of oxygen
= mole fraction Total Pressure
=1/3 P
Q6. The
temperatures at which real gases obey the ideal gas laws over a wide range of
pres-sure is called
Answer : Option B
Explaination / Solution:
The
temperature at which real gases obey the ideal gas laws over a wide range of pressure
is called Boyle temperature
Q7. In
a closed room of 1000 m3 a perfume bottle is opened up. The room develops a
smell. This is due to which property of gases?
Answer : Option C
Explaination / Solution:
No Explaination.
Q8. A
bottle of ammonia and a bottle of HCl connected through a long tube are opened
simultaneously at both ends. The white ammonium chloride ring first formed will
be
Answer : Option B
Explaination / Solution:
Rate of diffusion α 1/√m
mNH3 = 17 ; mHCl = 36.5
γNH3 > γHCl
Hence white fumes first formed near hydrogen
chloride
Q9. The
value of universal gas constant depends upon
Answer : Option D
Explaination / Solution:
No Explaination.
Q10. The
value of the gas constant R is
Answer : Option C
Explaination / Solution:
No Explaination.
