12th Grade > Chemistry
STATES OF MATTER MCQs
Total Questions : 30
| Page 3 of 3 pages
Answer: Option B. -> 1.5×1014
:
B
PV=nRT
n=PVRT=3.8×10−5×112×10−362.4×273
=0.02461×10−8mol
No. of molecules = 0.02461×10−8mol
=1.5×1014
:
B
PV=nRT
n=PVRT=3.8×10−5×112×10−362.4×273
=0.02461×10−8mol
No. of molecules = 0.02461×10−8mol
=1.5×1014
Answer: Option C. -> -100∘ C and 4 atm
:
C
Gas deviate from ideal gas behaviour to real gas (according to Vander Waal's at low temperature and high pressure)
:
C
Gas deviate from ideal gas behaviour to real gas (according to Vander Waal's at low temperature and high pressure)
Answer: Option C. -> He
:
C
Noble gases have the least intermolecular forces (dipole induced dipole)
:
C
Noble gases have the least intermolecular forces (dipole induced dipole)
Answer: Option D. -> H2
:
D
Vrms=√3RTM∴Vrmsα1√M at same T
because H2 has least molecular weight so its r.m.s velocity should be maximum.
:
D
Vrms=√3RTM∴Vrmsα1√M at same T
because H2 has least molecular weight so its r.m.s velocity should be maximum.
Answer: Option D. -> 36
:
D
rH2rCl2=61=√dCl2dH2 , If density of hydrogen is 1, then density of chlorine is 36
:
D
rH2rCl2=61=√dCl2dH2 , If density of hydrogen is 1, then density of chlorine is 36
Answer: Option D. -> 4 L
:
D
Z=PVnRT⇒1.90=1×800n×R×330
n=1×8001.90×R×330
Z=1.10=V×200n×R×570
1.10=V×200×1.90×R×330800×R×570
V = 4L
:
D
Z=PVnRT⇒1.90=1×800n×R×330
n=1×8001.90×R×330
Z=1.10=V×200n×R×570
1.10=V×200×1.90×R×330800×R×570
V = 4L
Question 27. Gaseous Benzene reacts with hydrogen gas in presence of a Nickel catalyst to form gaseous cyclohexane according to the Reaction
C6H6+3H2⟶C6H12
A mixture of C6H6 and excess H2 has a pressure of 60mm of Hg in an unknown volume. After the gas had been passed over a Ni catalyst and all the benzene converted to cyclohexane, the pressure of the gas was 30mm of Hg in the same volume at the same temperature. The fraction of C6H6 (by volume) present in the original volume is
C6H6+3H2⟶C6H12
A mixture of C6H6 and excess H2 has a pressure of 60mm of Hg in an unknown volume. After the gas had been passed over a Ni catalyst and all the benzene converted to cyclohexane, the pressure of the gas was 30mm of Hg in the same volume at the same temperature. The fraction of C6H6 (by volume) present in the original volume is
Answer: Option D. -> 16
:
D
Let initial pressure of C6H6=P1mm. And that of H2=P2mm.
∴P1+P2=60mm.⟶(1)
After the Reaction, pressure of C6H6=0
(As all has reacted)
Pressure of H2=P2−3P1
Pressure of C6H16=P1
Total Pressure = P2−3P1+P1=30mm
Or, P2−2P1=30mm⟶(2)
Solving (1) and (2) we get
P1=10mm,P2=50mm
Fraction of C6H6 by volume = fraction of moles = fraction of pressure = 1060=16
:
D
Let initial pressure of C6H6=P1mm. And that of H2=P2mm.
∴P1+P2=60mm.⟶(1)
After the Reaction, pressure of C6H6=0
(As all has reacted)
Pressure of H2=P2−3P1
Pressure of C6H16=P1
Total Pressure = P2−3P1+P1=30mm
Or, P2−2P1=30mm⟶(2)
Solving (1) and (2) we get
P1=10mm,P2=50mm
Fraction of C6H6 by volume = fraction of moles = fraction of pressure = 1060=16
Answer: Option D. -> None of these
:
D
From Van der Waal's equation ,
⟮p+aV2⟯⟮V−b⟯=RT
We get ,
⟮p+1.4100(10−0.04)=0.0821×323⇒p=2.648atm
From ideal gas equation, we have
p=RTV=0.0821×32310=2.652
Pideal=2.648atmPreal=2.652atm
:
D
From Van der Waal's equation ,
⟮p+aV2⟯⟮V−b⟯=RT
We get ,
⟮p+1.4100(10−0.04)=0.0821×323⇒p=2.648atm
From ideal gas equation, we have
p=RTV=0.0821×32310=2.652
Pideal=2.648atmPreal=2.652atm
Answer: Option B. -> 26.6 lit
:
B
P1V1n1T1=P2V2n2T2
1×10n×273=1.5×V22x×546
V2=26.6lit
:
B
P1V1n1T1=P2V2n2T2
1×10n×273=1.5×V22x×546
V2=26.6lit
Answer: Option C. -> 1684K; 2143K
:
C
¯C=Cp
√8RT1Mπ=√2RTM
8T1π=T2
T1T2=π8=22718=2256
T1=1684K
T2=2143K
:
C
¯C=Cp
√8RT1Mπ=√2RTM
8T1π=T2
T1T2=π8=22718=2256
T1=1684K
T2=2143K