Free Objective Test 02 Practice Test - 11th and 12th
Question 1
If C1,C2,C3.........represent the speeds of n1,n2,n3......... molecules, then the root mean square speed is _____.
√n1C12+n2C22+n3C32+...n1+n2+n3+...
⟮n1C12+n2C22+n3C32+..⟯12n1+n2+n3+.....
⟮n1C12⟯12n1+⟮n2C22⟯12n2+⟮n3C32⟯12n3+.....
⟮⟮n1C1+n2C2+n3C3+...⟯2⟮n1+n2+n3+.....⟯⟯12
SOLUTION
Solution : A
Root mean square speed = √n1C12+n2C22+n3C32+...n1+n2+n3+...
Question 2
The ratio of the rate of diffusion of helium and methane under identical condition of pressure and temperature will be___.
4
2
1
0.5
SOLUTION
Solution : B
rHerCH4=√MCH4MHe⇒√(164)⇒2
Question 3
In which of the gases given below, the average speed of the molecule is the least at 1000K?
CO2
SO2
O2
CH4
SOLUTION
Solution : B
Speed is inversely proportional to molecular weight. Molecular weight of SO2 is highest among the four. Hence its speed is least.
Question 4
The temperature and pressure at which ice, liquid water and water vapour can exist together are
0∘ C, 1atm
2∘C, 4.7atm
SOLUTION
Solution : C
All the three phases of water can coexist at 0∘ C & 4.7 mm pressure.
Question 5
Helium atom is two times heavier than a hydrogen molecule at 298 K, the average kinetic energy of helium is
Two times that of a hydrogen molecule
Same as that of a hydrogen molecule
Four times that of a hydrogen molecule
Half that of a hydrogen molecule
SOLUTION
Solution : B
EHeEH2=√THeTH2 so energies will be same for
He & H2 at same temperature.
Question 6
The temperature at which RMS velocity of SO2 molecules is half that of He molecules at 300 K is
150 K
600 K
900 K
1200 K
SOLUTION
Solution : D
USO2UHe=12=√MHeMSO2TSO2THe=√464TSO2300
=464TSO2300=14;TSO2=1200∘K
Question 7
The compressibility factor of a gas is less than 1 at STP. Its molar volume Vm will be
Vm > 22.42
Vm < 22.42
Vm = 22.42
None
SOLUTION
Solution : B
If Z<1 then molar volume is less than 22.4 L
Question 8
n1 and n2 moles of two ideal gases (mol. wt. M1 and M2) respectively at temperature T1K and T2K are mixed. Assuming that no loss of energy, the temperature of mixture becomes -
n1T1+n2T2
n1T1+n2T2T1+T2
n1T1+n2T2n1+n2
n1×T2n1×n2
SOLUTION
Solution : C
Let the final temperature be T , then K E1 + K Emixture
32 n1RT1 + 32 n2RT2 = 32 (n1+n2) RT
T = n1T1+n2T2n1+n2
Question 9
A cubical vessel has a side with 'I' cm lenth contained a gas at a pressure of 'p'. when the side of the vessel is made 12 cm, the pressure of gas becomes?
P
P8
2P
8P
SOLUTION
Solution : D
P1V1 = P2V2
P. l3 = p2 (12)3
P2 = 8P
Question 10
At what temperature, the volume of 'V' of a certain mass of a gas at 37o C will be doubled, keeping the pressure constant?
327o C
347o C
527o C
54o C
SOLUTION
Solution : B
V1T1=V2T2
V1=V, T1=37+273=310 k
V2=2V,T2=?
V310=2VT2
T2=620 K=347o C
Question 11
Pressure of a mixture of 4 g of O2 and 2 g of H2 confined in a bulb of 1 litre at 0°C is___.
25.215 atm
31.205 atm
45.215 atm
15.210 atm
SOLUTION
Solution : A
No. of moles of O2=432=0.125
No.of moles of H2=22=1
Total no. of moles = 1+0.125 = 1.125
P=nRTV=1.125×0.082×2731=25.215 atm
Question 12
For one mole of a van der Waal's gas when b =o and T = 300 K, the PV vs 1V plot is shown below. The value of the Van der Waal's constant "a" (atmL2mol−2) is
1.0
4.5
1.5
3.0
SOLUTION
Solution : C
⟮P+aV2⟯⟮V⟯=RT
PV + aV = RT
y = RT –a(V)
y = RT –a(x)
So, slope = a = 21.6–20.13−2=1.51=1.5
Question 13
The density of vapour of a substance (X) at 1 atm pressure and 500 K is 0.8 kgm3. The vapour effuses through a small hole at a rate of 45 times slower than oxygen under the same condition. What is the compressibility factor (Z) of the vapour?
0.974
1.35
1.52
1.22
SOLUTION
Solution : C
rxrO2=√MO2Mx=⟮45⟯2=32Mx⇒Mx = 50
dx = 0.80 kg m−3
Vm=1000800×50=62.5L
Z = PVmRT= 1×62.50.0821×500=1.52
Question 14
The temperature above which gas cannot be liquefied by application of pressure alone is
Boyle temperature
Curie temperature
Critical temperature
None of the above
SOLUTION
Solution : C
This is the definition of critical temperature.
Question 15
The density of Ne is maximum at
STP
0∘C, 2atm
273∘C, 1 atm
273∘C, 2 atm
SOLUTION
Solution : B
For an ideal gas, density(d) will be the maximum when Pressure is high and the temperature is low.
d=PMRT (or) d∝PT
Therefore option B is correct as it satisfies these conditions.