In a closed flask of 5 L, 1.0 g of H2 is heated from 300 to 600K. Which statement is not correct?
Pressure of the gas increases
The rate of collision increases
The number of moles of gas increases
The energy of gaseous molecules increases
Pressure remaining the same, the volume of a given mass of an ideal gas increases for every degree centigrade rise in temperature by definite fraction of its volume at
0°C
absolute zero
its critical temperature
its Boyle's temperature
Absolute zero is defined as the temperature
at which all molecular motion ceases
at which liquid helium boils
at which ether boils
All of the above
If p, V, M, T and R are pressure, volume, molar mass, temperature and gas constant respectively, then for an ideal gas, the density is given by
Correct gas equation is
The root mean square speeds at STP for the gases H2, N2, O2 and HBr are in the order
H2 < N2 < O2 < HBr
HBr < O2 < N2 < H2
H2 < N2 = O2 < HBr
HBr < O2 < H2 < N2
A gas is said to behave like an ideal gas when the relation = constant. When do you expect a real gas to behave like an ideal gas?
When the temperature is low
When both the temperature and pressuare low.
When both the temparature and pressure are high
When the temperature is high and pressure is low
Most crystals show good cleavage because the atoms, ions or molecules are
Weakly bonded together
Strongly bonded together
Spherically symmetrical
arranged in planes
In van der Waals' equation of state for a non-ideal gas, the term that accounts for inter molecular forces is
(V -b)
(RT)-1
RT
Root mean square velocity of a gas molecule is proportional to
m½
m0
m-½
m
