Chapter Wise IIT JAM Chemistry questions and solution
Chapter Wise IIT JAM Chemistry: Questions and Solutions 2005 - onwards
Previous Years IIT JAM Chemistry Questions and solutions:
We are here to help you with previous year question papers and solutions of IIT JAM Chemistry arranged chapter wise from 2005 to the recent one. Some expected important questions can also be found.
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IIT JAM Physical Chemistry:
Atomic Structure and Quantum Chemistry for IIT JAM
1. For H - like atoms,
the ground state energy is proportional to (IIT JAM 2005):
A.µ /z2 B.z2/µ
C.µ z2 D.1/
µ z2
2a.The electronic wave
function for hydrogen atom in the 2s state is given as:
Ψ ∝ (2-r/a0) exp (-r/2a0). Determine the
most probable radial distance for the electron in this state and also the
position of the node in terms of a0. (IIT JAM
2006):
2b. Calculate the
wavelength corresponding to the lower energy excitation of an electron
confined to a one dimensional box of length 1 nm. (IIT JAM 2006):
3. Which of the
following shows the kinetic energy of the ejected electron
versus frequency of the incident photons? (IIT JAM 2007)
4. The normalisation
constant A for the wave function,
Ψ(Φ) = A exp (imΦ) where
0 ≤ Φ ≤ 2π is: (IIT JAM 2007)
5. (IIT
JAM 2007)
6. a. (IIT JAM CHEM 2009)
In Bohr's model of hydrogen like atom with atomic number Z.
the angular momentum of an electron (Mass m and charge e) is a non zero
integral (n) multiple of h/2π.
The electrostatic attraction exerted by the
nucleus on the electron is balanced by the centrifugal force of the electron.
Write the mathematical expression for the
above statements. Hence obtain the expression for the radius of r of the
electron in terms of e, n and z.
6b.
7. IIT JAM CHEM 2009: The acceptable valence shell electronic arrangement is: the
8. An electron is found in an orbital
with one radial node and two angular nodes. Which orbital the electron is in?
a. 1s b. 2p.
c. 3d. d. 4d (IIT JAM Chem 2009)
9. An atomic orbital is described by
the wave function, (IIT JAM 2010)
a. identify the atomic orbital and calculate the mean or the
average radius of this orbital in terms of a0.
b.
Calculate the most probable radius (in terms of a0.) at
which an electron will be found when it occupies this orbital?
10. IIT JAM 2011
In the following equation, X is:
Am(95, 241) + α ----> Bk (97, 243) + X
11. IIT JAM 2011
i. U (92,235)+ n (0,1) -----> A(52,137) + B (40,97) + ______
ii. Se (34,82) ------>
2e(-1,0)+______
12. IIT JAM CHEMISTRY
2012 Q 42.
13. IIT JAM 2013 : For unnormalised wave function,
Ψ (r, θ, φ) = sinθ cosφ ((2r/a0) - (r/a0)2)
exp (-r/a0), the number of radial node is ___________.
14. IIT JAM 2014 : The energy of an electron in a hydrogenic atom with nuclear charge z varies as:
A. Z B. Z2
C. 1/Z D. 1/Z2
15. IIT JAM 2015
Click here get QnA of IIT JAM 2015
16. IIT JAM 2016 The effective nuclear charge of helium
atom is 1.7. The first ionization energy
of helium atom is _________.
A. 13.6 B.
23.1 C. 39.3 D. 27.2
17. IIT JAM 2016 (MSQ): 3pz orbital has:
A. one radial node B. Two radial nodes
C. one angular node D. two angular nodes
18. IIT JAM 2016 (Numerical answer type, NAT) The isotope 84 Po 214 undergoes one alpha and one beta particle emission sequentially to form an isotope X. The number of neutrons in X is __________.
19. 19. IIT JAM 2016 (NAT) Effective nuclear charge for 3d electron of vanadium according to Slater’s rule is ________.
=> Zeff = z – σ = 23 – 19.7 = 3.3
=> Zeff = z – σ = 23 – 19.7 = 3.3
20. IIT JAM 2017: For a particle in one
dimensional box of length L with potential energy V(x) = 0 for L > x
> 0 and V(x) = infinity for x ≥ L
and x ≤ 0, an acceptable function consistent with the boundary conditions
is _______. (A and B are constants)
a. A cos (nπx/L) b. B(x+X2)
c. Cx3
(x-L)
d. D/ Sin (nπx/L)
21.
IIT JAM 2018: Which of the following set(s) of
quantum numbers is (are) not allowed?
A. n =3, l=2, m
= -1
B. n =4, l=0, m
= -1
C.
n =3, l=3, m = -3
D.
n =5, l=3, m = +2
22. III
JAM Chem 2018 NAT: The electron of a hydrogen atom is in its nth Bohr orbit
having de-broglie wavelength of 13.4 angstrom. The value of n is _____. (radius
of nth orbit = 0.53 n^2 Angstrom)
23. III JAM Chem 2019 NAT: Ionisation energy of hydrogen atom is 13.6 ev and the first ionization energy of sodium atom is 5.1ev. The effective nuclear charge experienced by the valence electron of sodium atom is _____.
24. The Bohr’s first orbit radius of hydrogen is 53 pm. Radius
of third Bohr’s Orbit radius is ___.
25. III JAM Chem 2020 (NAT): The longest wavelength of light absorbed by hydrogen like atom is 2.48 nm. The z = ____. (Rydberg constant = 109700 cm^-1)
Ans. 1. The formula for energy of electron in an orbit is
En = -
me4 z2/8ε02 n2 h2
replacing mass by reduced mass the formula becomes
En= - µe4 z2/8ε02 n2 h2.
Thus the answer is C. µ z2
2a and 2b. Click here to get
the answer of 2a. And 2b.
If you want to test yourself whether you are for IIT JAM Chemistry,
then appear in these Online Mock Test.
3. The incident photon
should have some energy called work function below which no electrons can be
ejected. The energy with which electron is bound to the surface is called the
work function and the corresponding frequency is called threshold frequency (𝜈0). According to Einstein's Photoelectric effect,
K.E = h𝜈 - h𝜈0
This equation is
equivalent to: y=mx-C. Hence the correct option should be: A
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4. Click here to get
the answer.
5. According to the
question, overlap between dzx and pz orbital is positive as both have the same
sign (+ and -) to the same side. Hence they are ready for the bond formation.
Thus the answer should be A.
6. Click here to get
the answer
6.b. Two answers respectively are 8 O 17 and 4 Be 8
7. The answer should be
c. as all unpaired electron are having similar spin.
According to Hund's rule, no two electrons can occupy same spin direction
in same orbital. Orbitals of a subshell are filled up first with similar spin
then filled up with opposite direction during pairing.
Also maximum spin multiplicity and Large L value is stable configuration.
8. The formula of angular
node = l That means the angular nodes of an orbital is equal to it's Azimuthal
Quantum Number.
Since s orbitals have l =
0, they have no angular nodes. p and d orbitals have 1 and 2 angular nodes
respectively.
Thus the answer should either be 3d or 4d.
Now the formula of radial nodes = n-l-1. Since 4-2-1=1 and
according to the question, the radial nodes = 1, the orbital should be 4d. Thus
the answer should be d.
9. -Since the wave function only depends on r, it can be
represented as:
Ψ(r, θ,Φ) = Ψ(r, 0, 0) . Thus it has no angular nodes (as it is independent of θ and Φ ). Hence it is an s-orbital.
Thus
the given orbital is 1s (n,l,m = 1,0,0). The average radius of the orbital can
be found as follows
b. The most probable radius of the electron in 1s orbital
can be found as follows:
Thus
the given orbital is 1s (n,l,m = 1,0,0). The average radius of the orbital can
be found as follows
Thus
the average distance is 50% greater than the most probable distance of the
electron.
10. In
the given reaction, Am stands for Americium having atomic number 95 and mass
number 241, alpha particle has a charge of +2 and mass of 4. It means when Am
is bombarded with alpha particle the total nuclear charge becomes 97 and mass
becomes 245 on the left. Since Bk stands for Berkelium, the particles emitted
should be two neutrons 2n. Thus X stands for 2n (0,1).
11.
Similar as above
13. According quantum mechanics, the atomic orbitals can be written by the wave function Ψ (r, θ, φ) which is obtained by solving Schrodinger wave equation. That means a function of three polar coordinates r, θ and φ can be represented as a product of three independent wave function which depend separately on r, θ and φ respectively.
Ψ (r, θ, φ) = R(r) . Θ (θ) . Φ (φ)
Radial function R(r) gives the distribution of the electron as a function of the distance r from the nucleus. The R(r) part of the complete wave function can be isolated looking into the r realated part. in this case,
R(r) = ((2r/a0) - (r/a0)2) exp (-r/a0)
All points for which r = 0 gives the radial nodes.
When R(r) = 0,
((2r/a0) - (r/a0)2) exp
(-r/a0) = 0
=> r/a0 (2- (r/a0)) = 0
=> r =0 and r = 2a0
=> number of radial nodes = 2
14. Energy of an electron in Bohr's orbit = -kZ2/n2,
thus the answer should be B.
16.
Energy of an electron = -kZ2/n2
=
- 13.6 Z2/n2
Here
effective nuclear charge (Z*) is given that can be put into the above formula
for Z as because only two electrons are present in helium atom.
This
energy as calculated by the formula should be equal to the ionization energy as
this energy when given to the electron it is ejected.
Ionisation
Energy of an electron = -13.6 (1.7)2/ 12 = 39.3
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17. The number of radial nodes of an orbital = n - l - 1 and the number of angular nodes = l, where n and l are the principal and azimuthal quantum numbers respectively.
3pz orbital has n = 3 and l = 1, hence it should have one radial nodes and one angular nodes. hence the answer should be A and C.
18. On emission of one alpha particle (2 He 4)
atomic number reduced by 2 and mass by 4. Similarly on the emission of a beta particle
(-1 e 0) only the atomic number is increased by 1.
Thus the mass number of X = 214 – 1x 4 = 210
And the atomic number of X = 84 – 1 x 2 + 1 = 83
Thus the number of neutrons = 210 – 83 = 12719. V has z = 23
23 V = 1s2, 2s2, 2p6, 3s2, 3p6, 3d3, 4s2
According to Slater’s rule (find it along with periodic classification of elements), the electronic configuration
should be written as:
23 V = (1s)2, (2s 2p)8, (3s, 3p)8, (3d)3, (4s)2
σ = Shielding constant for s orbital = number
of n shell electrons x 0.35 + number of n -1 shell electrons x 0.85 + number of
all other electrons [(n-2) (n-3) or lower shells] x 1 = 1 x 0.35 + 11 x 0.85 =
10 x 1 = 19.70
=> Zeff = z – σ = 23 – 19.7 = 3.3
20. The function is continuous between X = 0 to
L and hence the function should be zero at x = 0 and x = L.
Both these conditions are satisfied by the
function C. Cx^3 (x-L)
21. B. and C.
are not possible as in B. when l = 0, m must be zero but given m = -1 which is
not possible. In C. n and l can’t be same as per quantum numbers.
22. 2πr = nλ
=> 2 x 3.14 x 0.53 n2 / n.13.4
=> n = 13.4 / 2 x 3.14 x 0.53
=> n = 4.03 = 4
23. Na = (1s)2, (2s,2p)8, (3s)1
Zeff for s electron = z – σ = 11 – (8 x 0.85 + 2 x 1) = 2.2
24.
Radius of nth orbit = ao (n2/z)
For
hydrogen atom, r = ao (n2/1)
= 53 x (32)
R = 53 x 9 = 477 pm
25. For longest wavelength, the energy absorbed for the transitiuon should be lowest. Thus the transition referes to 1st to 2nd orbit.
IIT JAM Questions on Gaseous State:
(JAM 2005) : Justify the following:
Considering CO2 as an ideal gas, equipartition theorem
predicts its total energy as 6.5 kT.
Justification: It’s a linear molecule
having 3 numbers (N) of atoms. It has 3 modes of translational, two modes of
rotational and 3N-5 modes of vibrational degrees of freedom. Thus according to
equipartition principle (each mode contributes ½ kT per molecule or ½ RT per
mole), Total energy E(total) = 3/2RT + RT + (3N-5)RT = 6.5 RT per mole or 6.5kT
per molecule. Click here to find details about degrees of freedom and
equipartition principle.
(JAM 2005): For the distribution of
molecular velocities of gases, what is the correct order most probable (m.p),
root mean square (rms) and average velocity (avg)?
Ans: mp : avg : rms = (2RT/M)1/2 : (8RT/πM)1/2 : (3RT/M)1/2.
= 1 : 1.128 : 1.224. Thus the order should
be: mp < avg < rms
Jam (2006): In the Maxwell distribution of molecular velocity given below as a graph, H is the height of the peak, L is the location of maximum and W is the width at half height.
What happens to these H, L and W as temperature
is decreased:
Ans:
Jam (2007): The Maxwell distribution function for the distribution of
speeds of molecules in gaseous system is,
f(c) = 4π(m/2πkT)3/2 C2 exp
(-mC2/2kT)
Show that the most probable speed is (2kT/m)1/2
Proof: The following proof is from the equation,
f(c)
= dNc/N
= 4π (m/2πkT)3/2 C2 exp
(-mC2/2kT)
The velocity with which most of the molecules move in a container at a particular temperature is called the most probable velocity.
We can see from the Maxwell
distribution curve that the most probable velocity is the peak of the curve
where the value of the derivative must be zero. Accordingly the derivative
of dNc with respect to dc must be equal to zero.
(JAM 2008): Given that the most probable speed of oxygen
gas is 1000 m/s, the average speed under the same conditions will
be ______?
Ans:
Cmp = (2RT/M)1/2 = 1000 ms-1
Cavg = (8RT/πM)1/2
= (4x2RT/πM)1/2
=> Cavg = (4/π) ½ x (2RT/M)1/2
=> Cavg = 2000/1.772 = 1128.6 ms-1
(JAM 2009): Write the expression for the vibrational contribution
to the total energy of CH4 (g) at 500k. All the vibrational modes
are active at this temperature. Also calculate the total internal energy of 1
mole of the gas at this temperature. Click here if want to know details about degreesof freedom and equipartition principle.
Ans: Vibrational degrees of freedom are
active at high temperature. CH4 (N = 5, as it has 5 atoms) is a non
linear molecule. Thus the number of vibrational modes = 3N-6 =9.
According to equipartition principle each mode (degrees
of freedom) contributes 1/2RT to the total energy but since vibrational mode
includes both potential and kinetic contributions, each vibrational mode
contribute 2x(1/2RT) or simply RT.
Thus vibrational contribution to the total energy = 9 RT
= 9x8.314x500 =37400 J/mole = 37.4kJ/mol
Total internal energy = translational contribution +
rotational contribution + vibrational contribution
Any molecule has 3 translational degrees freedom. CH4
being a non linear molecule has 3 rotational degrees of freedom and as
calculated it has 9 vibrational degrees of freedom.
=> I.E = 3x(1/2RT) + 3x(1/2RT) + 9RT = 48.88kJ/mol
(JAM 2010): The molar internal energy
of a gas at temperature is Um(T). The molar internal energy at T = 0
is Um(0). The correct expression that relates these two with
appropriate contributions is:
a) Um(T) = Um(0) +3RT (Linear molecule;
translation only)
b) Um(T) = Um(0) +(5/2)RT (Linear molecule;
translation and rotation only)
c) Um(T) = Um(0) +(3/2)RT (Non-linear
molecule; translation and rotation only)
d) Um(T) = Um(0) + RT (Non-linear molecule;
translation only)
Ans:
Molar heat capacity, CV = (∂U/ ∂T)
=>∂U = CV ∂T
=> ΔUm = CV ΔT
=> Um(T) - Um(0)
= CV (T – 0)
=> Um(T) - Um(0)
= CV T
For linear molecule, CV = (5/2)R
=> Um(T) - Um(0)
= (5/2)RT
Also, a linear molecule has 3 translational and 2
rotational degrees of freedom (if temperature not very high, where vibrational
mode is not active, as per the options/choices of answer available). Each mode
contributes (½)RT. Thus the option b is correct.
(JAM 2011): (a)Same as (JAM 2007)
(b) Calculate most probable velocity of CH4
at 1270c. (R = 8 J K-1mol-1)
Ans: M = 16 = 16X10-3 kg/mol
T = 1270c = 400k
Vmp = (2RT/M)1/2
= [(2x8x400)/ 16X10-3]1/2
= 632.45m/s
(JAM 2012)(i) Show that for n moles of a
van der Waal’s gas:
(∂U/∂V)T
=n2a/V2
(JAM 2013): No questions particularly on
gaseous state.
(JAM 2014): According to equipartition principle
of energy the molar heat capacity at constant volume for CO2 , SO2
and H2O gas follows the trend:
Ans: CO2 is a linear molecule where as the rest
two are nonlinear molecules.
For linear molecules, and according to equipartition
principle of energy,
Internal energy (U) = Contribution from Translational +
Rotational + Vibrational DOF
Linear molecules with two atoms (N=2) follow,
U = 3X(1/2)RT + 2 X(1/2)RT +
(3N-5)RT
=6.5RT
Thus Cv = (∂U/∂T)v = (∂/∂T) 6.5RT = 6.5R
Non-linear molecules with three atoms (N=3) follow,
U = 3X(1/2)RT + 3 X(1/2)RT +
(3N-6)RT
=6RT
Thus Cv = (∂U/∂T)v = (∂/∂T) 6RT = 6R
Hence order of molar heat capacity at constant volume
will be:
CO2 > SO2 = H2O
(JAM 2015): In an ideal monoatomic gas,
the speed of sound is given by (5RT/3M)1/2. If the speed of sound in
argon at 250c is 1245 km hr-1, the root mean square
velocity in ms-1 is __________.
Ans: RMS = (3RT/M)1/2
1245 km/hr = 1245 X 1000 m/hr
= (1245 X 1000) m/3600 sec
= 345.833 m/s
Given , speed of sound = (5RT/3M)1/2
= 345.833 m/s
= (5) ½ . 3 (3RT/M)1/2 = 345.833
m/s
RMS = (3RT/M)1/2
= 463 m/s
(JAM 2016): A 10 ltr flask containing
10.8 g of N2O5 is heated to 373 k, which leads to its
decomposition according to the equation
2 N2O5 -------> 4NO2 +
O2. If the final pressure in the flask is 0.5atm, then the partial
pressure of O2 in atm is _______.
Ans:
(JAM 2016): The relationship between the
van der Waals b coefficient of N2 and O2 is ______.
Ans: The van der Waals constant b represents excluded
volume (from the total volume of the vessel) of a gas. The greater the size of
the molecule greater is the excluded volume.
The size of N2 is 300 pm compared to 292 pm in
O2. Thus b(N2) > b(O2)
(JAM 2016): From the kinetic theory of
gases, the ratio of most probable speed to root mean square speed is _______.
Ans: Cmp/Crms = (2RT/M)1/2
/ (3RT/M)1/2 = 21/2/31/2
(JAM 2017): A vessel contains a mixture
of H2 and N2 gas. Density of the mixture is 0.2g L-1
at 300k and 1 atm pressure. Assuming that both the gases behave ideally, the
mole fraction of N2 in the vessel is ______.
(JAM 2017): The number of normal modes
of vibrations in naphthalene is _______.
Ans: Naphthalene is a non-linear molecule
with 18 number (N) of atoms.
Normal modes of vibrations = 3N -6
=3x18 – 6 = 48
(JAM 2018): The value of Cv
for 1 mole of N2 gas predicted from equipartition principle,
ignoring vibrational contribution is ________.
Ans: N2 is linear diatomic (N = 2)
molecule.
Cv = 3X(1/2)R + 2X(1/2)R
=(5/2)R = (5/2)x8.3
=20.75Jk-1mol-1
(JAM 2018): Assuming ideal gas behavior,
the density of O2 gas at 300
k and 1 atm is ______.
Ans: We know PV = nRT
=> P = (n/V)RT
=> P = (w/mV) RT
=> Pm = dRT
=> d = Pm/RT
Putting the values,
Density = 1.30gL-1
(JAM 2018): The behavior of Cl2
is closest to ideal gas at ______ temperature and ______ pressure.
Ans: high temperature and low pressure
(JAM 2019): The total number of degrees
of freedom of HBr molecule that is constrained to move in a straight line but
does not have any constraints on rotational and vibrational degrees of freedom
is ______.
Ans: Linear diatomic (N =2) molecule. One translational + 2
rotational + 1 vivrational DOF. In total 4.
(JAM 2019): The ratio of RMS velocity
for molecular oxygen and hydrogen is ________.
Ans: RMS velocity = (3RT/M)1/2
RMS of O2 / RMS of H2
= (MH2/MH2)1/2
= 1:4
(JAM 2020): The Boyle’s temperature (Tb)
is the temperature at which the properties of a real gas coincide with those of
an ideal gas in the low pressure limit. What should be the graph for Z (compressibility
factor) versus pressure at Tb?
(JAM 2021): If the root mean square
velocity of hydrogen at a particular temperature is 1900 ms-1, then
the rms speed for nitrogen at the same temperature should be ____.
Ans: Apply the formula RMS velocity = (3RT/M)1/2
for both the gases and take the ratio to cancel out similar terms. Find answer
next.
IIT JAM Questions on Liquid State:
(JAM 2005): At 20 0c the
vapour pressure of two pure liquids X and Y which form an ideal solution are 70
torr and 20 torr respectively. If the mole fraction of X in solution is 0.5,
find the mole fractions of X and Y in the vapour state.
Solution: Applying Raoult’s law of
vapour pressure,
PX = P0X . XX
= 70 X 0.5 = 35torr ----------eq. 1
[XX = molefraction of X in the liquid state]
Py = P0y . Xy
= 20 X 0.5 =10 torr ----------2
PT = 35 + 10 = 45 torr --------------3
Applying Dalton’s law of partial pressure,
PX = PT . yX ------------4
[yX = molefraction of X in the vapour state]
Py = PT . yy ---------------5
Using eq. 1, 3 and 4, we get,
And yy =
1 – 0.77 = 0.22
No particular question in IIT JAM Chemistry 2006 from Liquid state.
JAM (2007):
No
particular question in IIT JAM Chemistry 2008 and 2009 from Liquid state.
(JAM 2010): At room temperature, HCl is
a gas but HF is liquid, because:
Ans: Due to intermolecular H-Bonding in HF
(JAM 2010): Addition
of 1 g of a compound to 10 g water increases the boiling point by 0.3 0
c. The amount of compound needed to prepare 500 ml of 0.1M solution is: (given
that no dissociation or association of solute takes place, Kb of water = 0.513
k kg mol-1)
(JAM 2011): The
most viscous liquid among water, methanol, ethylene glycol and glycerol is:
Ans: Glycerol having 3 –OH
groups makes maximum intermolecular hydrogen bonding. It is the most viscous
among given liquids.
(JAM 2011): If 4
moles of MX2 salt in 1 kg water raises boiling point of water by 3.2
k, calculate the degree of dissociation of MX2 in the solution. (Kb
= 0.5 K Kg mol-1)
Solution: if
association or dissociation of solute particles take place then we have
the formula, ΔTb = i Kb m, where i = van’t Hoff factor.
Thus, 3.2 = i X 0.5 X 4
=> i =1.6
The relation between i and α in case of dissociation of solute is :
i = 1 + α (n-1) and MX2
gives one M 2+ and two X- ions number of particles after
dissociation, n = 3. Putting the value of n and i in the equation we get α =
0.3
(JAM 2012): An
aqueous solution containing 1g L-1 of a polymer exerts osmotic
pressure of 4 torr at 300 K. The molar mass of the polymer is:
Ans: Osomotic pressure = π =
4 torr = 4 / 760 atm
Corresponding R = 0.082 L atm K-1
mol-1
Π = wRT/mV
=> m = wRT/ Π V
= (1 X 0.082 X 300) / (4/760) X 1
= 4674g/mol
(JAM 2012): The
molality of (NH4)2SO4 solution that has same
ionic strength as 1 mol kg-1 of KCl is:
Solution:
(JAM 2012): Consider
ideal mixing of 2 moles of toluene and 2 moles of benzene at 1 atm and 300 K. Calculate
the values of ΔVmix , ΔUmix , ΔHmix , ΔGmix
, ΔSmix for the process. (ln 2 = 0.69).
Solution: An
ideal solution can be considered as a mixture of two ideal gasses.
Also for ideal solution, each of
ΔVmix , ΔUmix , ΔHmix isequal to 0
The initial pressure of each gas
= 1 atm and temperature = 300K
Each of the gas is of 1 mole. Hence the mole fraction (χ) of each component = χ = 2/ (2+2) = 0.5
The Gibb’s energy of mixing,
ΔGmix = nRT (χ1 ln χ1 +
χ2 ln χ2)
=
4 X 8.314 X 300 [0.5 ln(1/2) + 0.5 ln(1/2)}
=
4 X 8.314 X 300 [ ln(1/2)]
=
- 6.916 KJ
The
negative value of free energy of mixing indicates the spontaneous process while
two liquids are added.
ΔSmix = ( - ΔGmix)
/ T
= - (- 6.916) /
T
= + 6.916 / 300 = 23.05 j/K
(JAM 2013): No
particular question from liquid state.
(JAM 2014): Mixed question (Change in enthalpy, free energy, osmotic pressure rate, constant, heat capacity versus temperature)
(II - D) Osmotic
Pressure of ideal solution (π),
is directly proportional to the temperature. Hence Curve D is the right
choice.
π V = nRT
(III - B) Standard free energy of
formation (ΔfG0) of elements is taken as zero. ΔfG0 versus temperature is constant. Hence Curve B fits into it.
(IV - C) The
molar heat capacity at constant volume for an ideal gas as predicted by
equipartition of energy is given by, Cv.m = (∂ Um / ∂ T). Thus molar heat capacity
is inversely proportional to the temperature. Curve C fits into it.
(V - A) Arrehenius
equation,
K = A Exp (-Ea/RT)
Thus k ∝ Exp (-1/T) and the
Exponential Curve A fits to it.
(JAM 2014): The ionic
strength of 0.1M aqueous solution of Fe2(SO4)3is
______.
Soution: Refer
corresponding JAM 2012 Q and A.
(JAM 2016):
Cu(s) + 4H+(aq) +2NO3- (aq) -----------> 2NO2 (g) + Cu2+(aq) +2H2O
In the above reaction, at 1 atm and 298 K, if 6.36g of Cu is used. Assuming ideal gas behavior, the volume of NO2 produced in litre is __________.
Solution: Number of moles of Cu = 6.36/63.6 = 0.1
from the equation,
0.1 mole Cu equivalent to 0.2 mole of NO2
V = nRT/P = (0.2X0.0821X298)/1 = 4.89 L
(JAM 2017): No particular question from liquid state.
(JAM 2018): The volume of 0.3M ferrous ammonium sulphate solution required for the completion of redox titration with 20 ml of 0.1M potassium dichromate solution is _______.
Solution: In the redox reaction Cr2O72- oxidises ferrous (Fe2+) ion, by the following reaction,
Cr2O72- + 6Fe2+ + 14H+ ----> 2Cr3++ 6Fe3+ + 7H2O
Fom the equation,
1 mole of Cr2O72- requirres 6 moles of Fe2+
Number of moles of Cr2O72- (as per the question) = 20 X 0.1 = 2 moles
Number of moles of Mohr’s salt (Fe2+) ions needed = 6X2 = 12 moles
Volume of Mohr’s salt required = 12/0.3 = 40 ml
Alternatively,
One mole (n1) of Cr2O72- requirres 6 moles (n2) of Fe2+
n1M1V1 = n2M2V2
=> 1 X 0.3 X V1 = 6 X 0.1 X 20
=> V1 = 40 ml
(JAM 2019): Assume that the reaction of MeMgBr with ethylacetate proceeds with 100% conversion to give tert-butanol. The volume of 0.2M solution of MeMgBr required to covert 10 ml of a 0.025 M solution of ethylacetate to tert-butanol is ____ ml.
Solution: This question can be solved according to the milimoles of reactant species.
Milimoles = Molarity X Volume in ml
Also Volume in ml = Milimoles / molarity
In a balanced equation moles of reaction can be replaced by milimoles.
(JAM 2020): The mean ionic activity coefficient for a 0.01 M aqueous solution of Ca3(PO4) 2 is __________.
[log Y± = -0.059 z+ I Z-I (I1/2 ) ]
Solution: See IIT JAM 2012 in liquid section.
IIT JAM Questions on Solid State
(JAM 2005): No questions from solid state.
(JAM 2006): No questions from solid state.
(JAM 2007): No questions from solid state.
(JAM 2008): No questions from solid state.
(JAM 2009): No questions from solid state.
(JAM 2010): The structure of rock salt is_________.
Ans:
Vectorization: GKFX, CC BY-SA 3.0 <http://creativecommons.org/licenses/by-sa/3.0/>, via Wikimedia Commons
https://commons.wikimedia.org/wiki/File:NaCl-Ionengitter.svg
In most of ionic crystal the anions take the
lattice point positions and the cations occupy the voids formed by the
anions.
The ionic radius ratio (ratio of radius of
cation to the anion is 0.52 which is in between 0.414 and 0.732 suggests an
octahedral void)
In NaCl crystal Cl- ions at
lattice points (corner + face centres in FCC or ABCABC arrangement) form the
octahedral voids which are occupied by Na+ ions. Thus
Coordination number of both the ions are =6:6 or 1:1
(JAM 2010): Draw
a properly labeled unit cell diagram of CsCl. Show through calculations that
there is only one CsCl per unit cell.
Ans:
Chegg Study, CC BY-SA 4.0 <https://creativecommons.org/licenses/by-sa/4.0>, via Wikimedia Commons, https://commons.wikimedia.org/wiki/File:Struktura_cezijevega_klorida.png
The radius ratio of CsCl is 0.93
suggesting a cubical void or BCC packing and thus ration of coordination number
is 8:8 or 1:1.
Number of Cs+ ion per unit
cell = 1 (at the body centre cubic unit cell)
Number of Cl- ions present at
all corner of Body centre cubic = 8X1/8 =1
Thus there is only one CsCl per unit
cell.
(JAM 2011): The
oxide that has inverse spinel structure is:
i.FeCr2O4 ii.MnCr2O4
iii. CoAl2O4
iv. Fe2CoO4
Solution: Class of minerals of
general formula AB2X4, having cubic (isometric) crystal
system with X anions arranged in cubic close packed lattice and cations A and B
occupying some or all of the tetrahedral and octahedral voids are called
spinels. Oxide spinels have general formula AB2O4, for example, MgAl2O4. In the close pack
array of anions (e.g., oxide ions), A site cations fill the 1/8 part of the
tetrahedral voids and B site cations fill ½ of the octahedral voids.
Its very clear that in a unit cell of FCC the
number of atoms at all lattice points = 8X1/8(from corner) + 6X1/2(from face
centres) = 4
Hence number of Oxide ions = n = 4
Number of tetrahedral holes = 2n = 8
1/8 th of 8 = 1 = A
Number of octahedral holes = n = 4
½ of octahedral holes = 2 = B
½ of octahedral holes = 2 = B
Hence AB2O4 is the
formula of normal spinels. For more clarity A can be understood as divalent
cations and B can be understood as trivalent cations.
Inverse spinels are closely related to spinels,
where the close pack array of anions remain the same but A site ions and ½ of B
site ions switch their positions, giving a formula B(AB)O4. For more
clarity, in an inverse spinel the A2+ ions occupy ¼ th of octahedral
voids along with ½ of B3+ ions whereas the other half of the B3+
ions occupy 1/8th of the tetrahedral voids.
In the given question, FeIII(CoIIFeIII)O4
is the inverse spinel because the Co2+ ion is octahedrally surrounded.
CFSE of Co2+ = d7 = t2g5eg2
= (-0.4X5 + 0.6x2) Δo = -0.8 Δo. This is highest compared to FeIII having CFSE 0. Thus Co2+ will be stabilized
in octahedral voids. This should be the answer.
JAM 2011: The
transition metal monoxide that shows metallic conductivity is: i.NiO
ii.MnO iii.TiO iv.CoO
Solution: NiO, becaude Nickel can exists both in +2 and +3 oxidation states. The +3 state of Nickel act as a hole and accept electrons from nearby +2 oxidation state to conduct the electricity.
JAM 2012: Draw the unit cell
structure of NaCl. Calculate the limiting radius ratio of any ionic solid
having NaCl like structure.
Solution: See JAM 2010 for the structure of NaCl
JAM 2013: A hypothetical element
(atomic weight 300) crystalises in simple cubic lattice. The first order X-ray
diffraction with wavelength 5 A0 appears at an angle 300.
The density of the crystal is _______ g cm-3.
Solution: From Bragg’s equation,
2dsin θ
= nλ , for first order n=1, Thus 2dsin300=1X5
2d(1/2)=5
d=5 A0 = 5X10-8
cm
d=a (for simple cubic lattice)
density = ZM/a3Na
For simple cubic lattice the number atoms per
unit cell z = 1
Na = 6.02X1023 and M = atomic mass =
300
We got density = 3.985 g cm-3
For limiting radius Click here.
To be continued.....