MCH-13 EM 2024 SOLVED ASSIGNMENT

Description

ASSIGNMENT
General Physical Chemistry
Course Code: MCH-013
Assignment Code: MCH-013/TMA/2024
Maximum Marks: 100
Note: Attempt all questions. The marks for each question are indicated against it.
1. Answer any five of the following in brief. (2×5)
(a) The entropy change is not a good criterion for spontaneity of a thermodynamic process.
Comment.
(b) Derive the relation between Gibbs energy and Helmholtz energy.
(c) Differentiate between molar and partial molar properties.
(d) Give Stirling’s approximation and outline its significance
(e) How can the diamagnetic and paramagnetic substances be distinguished using magnetic
susceptibilities?
(f) Outline the limitations of collision theory.
2. (a) (i) An isothermal and isobaric process is accompanied by changes in enthalpy and
entropy as 52 kJ mol-1 and 165 JK-1 mol-1
, respectively. Predict whether the process be
spontaneous at 400K.
(ii) If the enthalpy and entropy changes are not affected by the change in temperature
calculate the temperature at which the system will attain equilibrium (3+2)
(b) Define the term ‘chemical potential’ and discuss the effect of temperature on chemical
potential. (2+3)
3. (a) Explain the difference between permutation and configuration. Calculate the number of
permutations and configurations possible while selecting three days out of seven days in a
week. (3+2)
(b) Define molecular partition functions. Derive an expression for the translational partition
function for motion along x- direction in a system. (2+3)
4. (a) The X-ray power diffraction angles from the molybdenum crystal are observed at 20.26°,
29.30°, 36.82°, 43.82°, 50.70°, 58.80°, 66.30°. Determine the type of cubic crystal formed
by molybdenum? (5)
(b) Explain crystal symmetry elements, Screw Axis and Glide Plane using suitable
illustrations. (5)
5. (a) Describe the basic premise of transition state theory of reaction rates and derive an
expression by using this theory for the rate constant for the elementary reaction (5)
X + Y ® Products
2
(b) Discuss Lindemann-Christiansen mechanism for unimolecular reactions and derive an
expression for the rate equation for the unimolecular reaction as per LindemannChristiansen mechanism. (5)
6. Answer any five of the following in brief. 2 x 5
(a) Discuss the role of solvent in reactions in solution phase.
(b) Define fast reactions and give different strategies used for studying fast reactions.
(c) Define enzyme inhibition and state it’s different types.
(d) Define ionic strength and calculate the same for an aqueous solution of 0.1 M MgCl2.
(e) Differentiate between true and potential electrolytes.
(f) Differentiate between the phenomenon of Osmosis and Dialysis.
(g) State Fick’s second law of diffusion and give its significance.
7. (a) Describe the encounter pair description of reaction in solution and derive the expression for
the rate of a reaction in solution in terms of this description. ( 2+3)
(b) In a Temperature-jump experiment the relaxation time of an equilibrium reaction of the type
is found to be 5 µs. in a separate experiment, the equilibrium constant for the reaction is
found to be 5 x 10-4
, calculate the values of rate constants for the forward and backward
reactions. (5)
8. (a) Define homogeneous catalytic reactions and derive the expression for the initial reaction
rate of a homogeneous catalytic reaction. (2+3)
(b) Give the Michaelis–Menten mechanism of enzyme catalysed reactions and derive an
expression for the rate of enzymatic reaction using this mechanism. (2+3)
9. (a) Define mean ionic mobility and formulate the relations between mean ionic molality (m±)
and m for the following electrolytes: (2+3)
Li2SO4, MgCl2 and Na3PO4
(b) Explain the principle for the experimental determination of mean ionic activity by emf
measurement. (5)
10. (a) Define coefficient of viscosity and derive the relationship between the coefficient of
viscosity and mean free path. (2+3)
(b) Define ionic mobility and derive the relationship between the ionic mobility and molar
conductivity.