2007
NEET
MCQ
AIPMT 2007
Consider the following reactions :
(i) H+(aq) + OH$-$(aq) = H2O(l), $\Delta $H = $-$ X1 kJ mol$-$1
(ii) H2(g) + 1/2O2(g) = H2O(l), $\Delta $H = $-$ X2 kJ mol$-$1
(iii) CO2(g) + H2(g) = CO(g) + H2O(l), $\Delta $H = $-$ X3 kJ mol$-$1
(iv) C2H2(g) + 5/2O2(g) = 2CO2(g) + H2O(l), $\Delta $H = +X4 kJ mol$-$1
Enthalpy of formation of H2O(l) is
(i) H+(aq) + OH$-$(aq) = H2O(l), $\Delta $H = $-$ X1 kJ mol$-$1
(ii) H2(g) + 1/2O2(g) = H2O(l), $\Delta $H = $-$ X2 kJ mol$-$1
(iii) CO2(g) + H2(g) = CO(g) + H2O(l), $\Delta $H = $-$ X3 kJ mol$-$1
(iv) C2H2(g) + 5/2O2(g) = 2CO2(g) + H2O(l), $\Delta $H = +X4 kJ mol$-$1
Enthalpy of formation of H2O(l) is
A.
+X3 kJ mol$-$1
B.
$-$X4 kJ mol$-$1
C.
+X1 kJ mol$-$1
D.
$-$X2 kJ mol$-$1
2006
NEET
MCQ
AIPMT 2006
Assume each reaction is carried out in an open container. For which reaction will $\Delta $H = $\Delta $E ?
A.
2CO(g) + O2(g) $ \to $ 2CO2(g)
B.
H2(g) + Br2(g) $ \to $ 2HBr(g)
C.
C(s) + 2H2O(g) $ \to $ 2H2(g) + CO2(g)
D.
PCl5(g) $ \to $ PCl3(g) + Cl2(g)
2006
NEET
MCQ
AIPMT 2006
The enthalpy of hydrogenation of cyclohexene is is $-$ 119.5 kJ mol$-$1. If resonance energy of benzene is $-$ 150.4 kJ mol$-$1, its enthalpy of hydrogenation would be
A.
$-$ 358.5 kJ mol$-$1
B.
$-$ 508.9 kJ mol$-$1
C.
$-$ 208.1 kJ mol$-$1
D.
$-$ 269.9 kJ mol$-$1
2006
NEET
MCQ
AIPMT 2006
The enthalpy and entropy change for the reaction:
Br2(l) + Cl2(g) $ \to $ 2BrCl(g)
are 30 kJ mol$-$1 and 105 J K$-$1 mol$-$1 respectively.
The temperature at which the reaction will be in equilibrium is
Br2(l) + Cl2(g) $ \to $ 2BrCl(g)
are 30 kJ mol$-$1 and 105 J K$-$1 mol$-$1 respectively.
The temperature at which the reaction will be in equilibrium is
A.
300 K
B.
285.7 K
C.
273 K
D.
450 K
2006
NEET
MCQ
AIPMT 2006
Identify the correct statement for change of Gibb's energy for a system ($\Delta $Gsystem) at constant temperature and pressure.
A.
If $\Delta $Gsystem < 0, the process is not spontaneous.
B.
If $\Delta $Gsystem > 0, the process is spontaneous.
C.
If $\Delta $Gsystem = 0, the system has attained equilibrium.
D.
If $\Delta $Gsystem = 0, the system is till moving in a particular direction.
2005
NEET
MCQ
AIPMT 2005
Which of the following pairs of a chemical reaction is certain to result in a spontaneous reaction ?
A.
Exothermic and increasing disorder
B.
Exothermic and decreasing disorder
C.
Endothermic and increasing disorder
D.
Endothermic and decreasing disorder
2005
NEET
MCQ
AIPMT 2005
A reaction occurs spontaneously if
A.
T$\Delta $S < $\Delta $H and both $\Delta $H and $\Delta $S are +ve
B.
T$\Delta $S > $\Delta $H and $\Delta $H is +ve and $\Delta $S are $-$ve
C.
T$\Delta $S > $\Delta $H and both $\Delta $H and $\Delta $S are +ve
D.
T$\Delta $S = $\Delta $H and both $\Delta $H and $\Delta $S are +ve
2005
NEET
MCQ
AIPMT 2005
The absolute enthalpy of neutralisation of the reaction :
Mg(O)(s) + 2HCl(aq) $ \to $ MgCl2(aq) + H2O(l) will be
Mg(O)(s) + 2HCl(aq) $ \to $ MgCl2(aq) + H2O(l) will be
A.
$-$57.33 kJ mol$-$1
B.
greater than $-$ 57.33 kJ mol$-$1
C.
less than $-$ 57.33 kJ mol$-$1
D.
57.33 kJ mol$-$1
2004
NEET
MCQ
AIPMT 2004
Standard enthalpy and standard entropy changes for the oxidation of ammonia at 298 K are $-$ 382.64 kJ mol$-$1 and $-$ 145.6 kJ mol$-$1, respectively. Standard Gibb's energy change for the same reaction at 298 K is
A.
$-$ 221.1 kJ mol$-$1
B.
$-$339.3 kJ mol$-$1
C.
$-$ 439.3 kJ mol$-$1
D.
$-$ 523.2 kJ mol$-$1
2004
NEET
MCQ
AIPMT 2004
The work done during the expansion of a gas from a volume of 4 dm3 to 6 dm3 against a constant external pressure of 3 atm is (1 L atm = 101.32 J)
A.
$-$ 6 J
B.
$-$ 608 J
C.
+ 304 J
D.
$-$ 304 J
2004
NEET
MCQ
AIPMT 2004
If the bond energies of H $-$ H, Br $-$ Br, and H $-$ Br are 433, 192 and 364 kJ mol$-$1 respectively, the $\Delta $Ho for the reaction
H2(g) + Br2(g) $ \to $ 2HBr(g) is
H2(g) + Br2(g) $ \to $ 2HBr(g) is
A.
$-$ 261 kJ
B.
+103 kJ
C.
+261 kJ
D.
$-$103 kJ
2004
NEET
MCQ
AIPMT 2004
Considering entropy (S) as a thermodynamic parameter, the criterion for the spontaneity of any process is
A.
$\Delta {S_{system}} + \Delta {S_{surroundings}} > 0$
B.
$\Delta {S_{system}} - \Delta {S_{surroundings}} > 0$
C.
$\Delta {S_{system}} > 0\,\,\,$only
D.
$\Delta {S_{surroundings}} > 0$ only
2003
NEET
MCQ
AIPMT 2003
Formation of solution from two components can be considered as
(i) Pure solvent $ \to $ separated solvent molecules, $\Delta $H1
(ii) Pure solute $ \to $ separated solute molecules, $\Delta $H2
(iii) Separated solvent and solute molecules $ \to $ solution, $\Delta $H3
Solution so formed will be ideal if
(i) Pure solvent $ \to $ separated solvent molecules, $\Delta $H1
(ii) Pure solute $ \to $ separated solute molecules, $\Delta $H2
(iii) Separated solvent and solute molecules $ \to $ solution, $\Delta $H3
Solution so formed will be ideal if
A.
$\Delta $Hsoln = $\Delta $H1 + $\Delta $H2 + $\Delta $H3
B.
$\Delta $Hsoln = $\Delta $H1 + $\Delta $H2 $-$ $\Delta $H3
C.
$\Delta $Hsoln = $\Delta $H1 $-$ $\Delta $H2 $-$ $\Delta $H3
D.
$\Delta $Hsoln = $\Delta $H3 $-$ $\Delta $H1 $-$ $\Delta $H2
2003
NEET
MCQ
AIPMT 2003
The molar heat capacity of water at constant pressure, C, is 75 J K$-$1 mol$-$1. When 1.0 kJ of heat is supplied to 100 g of water which is free to expand, the increase in temperature of water is
A.
1.2 K
B.
2.4 K
C.
4.8 K
D.
6.6 K
2003
NEET
MCQ
AIPMT 2003
What is the entropy change (in J K$-$1 mol$-$1) when one mole of ice is converted into water at 0oC? (The enthalpy change for the conversion of ice to liquid water is 6.0 kJ mol$-$1 at 0oC).
A.
20.13
B.
2.013
C.
2.198
D.
21.98
2003
NEET
MCQ
AIPMT 2003
For the reaction,
C3H8(g) + 5O2(g) $ \to $ 3CO2(g) + 4H2O(l)
at constant temperature, $\Delta $H $-$ $\Delta $E is
C3H8(g) + 5O2(g) $ \to $ 3CO2(g) + 4H2O(l)
at constant temperature, $\Delta $H $-$ $\Delta $E is
A.
+ RT
B.
$-$3RT
C.
+ 3RT
D.
$-$ RT
2003
NEET
MCQ
AIPMT 2003
The densities of graphite and diamond at 298 K are 2.25 and 3.31 g cm$-$3, respectively. If the standard free energy difference $\left( {\Delta {G^o}} \right)$ is equal to 1895 J mol$-$1, the pressure at which graphite will be transformed into diamond at 298 K is
A.
11.14 $ \times $ 108 Pa
B.
11.14 $ \times $ 107 Pa
C.
11.14 $ \times $ 106 Pa
D.
11.14 $ \times $ 105 Pa
2003
NEET
MCQ
AIPMT 2003
For which one of the following equations is $\Delta $Horeact equal to $\Delta $Hof for the product ?
A.
Xe(g) + 2F2(g) $ \to $ XeF4(g)
B.
2CO(g) + O2(g) $ \to $ 2CO2(g)
C.
N2(g) + O3(g) $ \to $ N2O3(g)
D.
CH4(g) + 2Cl2(g) $ \to $ CH2Cl2(l) + 2HCl(g)
2002
NEET
MCQ
AIPMT 2002
2 mole of ideal gas at 27oC temperature is expanded reversibly from 2 lit. to 20 lit. Find entropy change. (R = 2 cal/mol K)
A.
92.1
B.
0
C.
4
D.
9.2
2002
NEET
MCQ
AIPMT 2002
Which reaction is not feasible?
A.
2KI + Br2 $ \to $ 2KBr + I2
B.
2KBr + I2 $ \to $ 2KI + Br2
C.
2KBr + Cl2 $ \to $ 2KCl + Br2
D.
2H2O + 2F2 $ \to $ 4HF + O2
2002
NEET
MCQ
AIPMT 2002
Unit of entropy is
A.
J K$-$1 mol$-$1
B.
J mol$-$1
C.
J$-$1 K$-$1 mol$-$1
D.
J K mol$-$1
2002
NEET
MCQ
AIPMT 2002
In a closed insulated container a liquid is stirred with a paddle to increase the temperature which of the following is true ?
A.
$\Delta $E = W $ \ne $ 0, q = 0
B.
$\Delta $E = w = q $ \ne $ 0
C.
$\Delta $E = 0, W = q $ \ne $ 0
D.
W = 0, $\Delta $E = q $ \ne $ 0.
2002
NEET
MCQ
AIPMT 2002
Heat of combustion $\Delta $Ho for C(s), H2(g) and CH4(g) are $-$ 94, $-$ 68 and $-$213 kcal/mol, then $\Delta $Ho for C(s) + 2H2(g) $ \to $ CH4(g) is
A.
$-$17 kcal
B.
$-$111 kcal
C.
$-$170 kcal
D.
$-$85 kcal
2001
NEET
MCQ
AIPMT 2001
Change in enthalpy for reaction,
2H2O2(l) $ \to $ 2H2O(l) + O2(g)
if heat of formation of H2O2(l) and H2O(l) are $-$188 and - 286 kJ/mol respectively, is
2H2O2(l) $ \to $ 2H2O(l) + O2(g)
if heat of formation of H2O2(l) and H2O(l) are $-$188 and - 286 kJ/mol respectively, is
A.
$-$ 196 kJ/mol
B.
+ 196 kJ/mol
C.
+948 kJ/mol
D.
$-$ 948 kJ/mol
2001
NEET
MCQ
AIPMT 2001
When 1 mol of gas is heated at constant volume temperature is raised from 298 to 308 K. Heat supplied to the gas is 500 J. Then which statement is correct ?
A.
q = w = 500 J, $\Delta $E = 0
B.
q = $\Delta $E = 500 J, w = 0
C.
q = w = 500 J, $\Delta $E = 0
D.
$\Delta $E = 0, q = w = $-$ 500 J
2001
NEET
MCQ
AIPMT 2001
PbO2 $ \to $ PbO; $\Delta $G298 < 0
SnO2 $ \to $ SnO; $\Delta $G298 > 0
Most probable oxidation state of Pb and Sn will be
SnO2 $ \to $ SnO; $\Delta $G298 > 0
Most probable oxidation state of Pb and Sn will be
A.
Pb4+, Sn4+
B.
Pb4+, Sn2+
C.
Pb2+, Sn2+
D.
Pb2+, Sn4+
2001
NEET
MCQ
AIPMT 2001
Enthalpy of CH4 + ${1 \over 2}$ O2 $ \to $ CH3OH is negative. If enthalpy of combustion of CH4 and CH3OH are x and y respectively. Then which relation is correct?
A.
x > y
B.
x < y
C.
x = y
D.
x3 y
2000
NEET
MCQ
AIPMT 2000
The entropy change in the fusion of one mole of a
solid melting at 27oC (latent heat of fusion is 2930 J
mol–1) is :
A.
9.77 J/mol-K
B.
10.77 J/mol-K
C.
9.07 J/mol-K
D.
0.977 J/mol-K
2000
NEET
MCQ
AIPMT 2000
2Zn + O2 $ \to $ 2ZnO; $\Delta $Go = $-$ 616 J
2Zn + S2 $ \to $ 2ZnS; $\Delta $Go = $-$ 293 J
S2 + 2O2 $ \to $ 2SO2; $\Delta $Go = $-$408 J
$\Delta $Go for the following reaction
2ZnS + 3O2 $ \to $ 2ZnO + 2SO2 is
2Zn + S2 $ \to $ 2ZnS; $\Delta $Go = $-$ 293 J
S2 + 2O2 $ \to $ 2SO2; $\Delta $Go = $-$408 J
$\Delta $Go for the following reaction
2ZnS + 3O2 $ \to $ 2ZnO + 2SO2 is
A.
$-$ 731 J
B.
$-$ 1317 J
C.
$-$ 501 J
D.
+ 731 J
2000
NEET
MCQ
AIPMT 2000
For the reaction,
C2H5OH(l) + 3O2(g) $ \to $ 2CO2(g) + 3H2O(l)
which one is true
C2H5OH(l) + 3O2(g) $ \to $ 2CO2(g) + 3H2O(l)
which one is true
A.
$\Delta $H = $\Delta $E $-$RT
B.
$\Delta $H = $\Delta $E + RT
C.
$\Delta $H = $\Delta $E + 2RT
D.
$\Delta $H = $\Delta $E $-$ 2RT
2016
NEET
MSQ
NEET 2016 Phase 1
The correct thermodynamic conditions for the spontaneous reaction at all temperatures is
A.
$\Delta $H < 0 and $\Delta $S > 0
B.
$\Delta $H < 0 and $\Delta $S < 0
C.
$\Delta $H < 0 and $\Delta $S = 0
D.
$\Delta $H > 0 and $\Delta $S < 0
2019
AIIMS
MCQ
AIIMS 2019
The correct relation is
A.
$\Delta G=-R T \ln K / Q$
B.
$\Delta G=+R T \ln K$
C.
$\Delta G=-R T \ln Q / K$
D.
$\Delta G=+R T \ln Q$
2019
AIIMS
MCQ
AIIMS 2019
At $25^{\circ} \mathrm{C}, 1$ mole of butane is heated then $\mathrm{CO}_2$ and $\mathrm{H}_2 \mathrm{O}$ liquid is formed work done is
A.
$75.6 \mathrm{~L} \mathrm{~atm}$
B.
$85.6 \mathrm{~L} \mathrm{~atm}$
C.
$50.3 \mathrm{~L} \mathrm{~atm}$
D.
None of these
2019
AIIMS
MCQ
AIIMS 2019
Assertion : $U$ is state function.
Reason : $T$ is an intensive property.
A.
If both assertion and reason are true and reason is the correct explanation of assertion.
B.
If both assertion and reason are true, but reason is not the correct explanation of assertion.
C.
If assertion is true, but reason is false.
D.
If both assertion and reason are false.
2018
AIIMS
MCQ
AIIMS 2018
In an adiabatic process, no transfer of heat takes place between system and surroundings. Choose the correct option for free expansion of an ideal gas under adiabatic condition from the following
A.
$q=0, \Delta T \neq 0, W=0$
B.
$q \neq 0, \Delta T=0, W=0$
C.
$q=0, \Delta T=0, W=0$
D.
$q=0, \Delta T<0, W \neq 0$
2018
AIIMS
MCQ
AIIMS 2018
$\Delta H$ and $\Delta E$ for the reaction,
$\mathrm{Fe}_2 \mathrm{O}_3(s)+3 \mathrm{H}_2(g) \longrightarrow 2 \mathrm{Fe}(s)+\mathrm{H}_2 \mathrm{O}(l)$
at constant temperature are related as
A.
$\Delta H=\Delta E$
B.
$\Delta H=\Delta E+R T$
C.
$\Delta H=\Delta E+3 R T$
D.
$\Delta H=\Delta E-3 R T$