Federal Public Service Commission (FPSC)
Competitive Examination for Recruitment to BPS-17 Posts under the Federal Government
Time Allowed: 3 Hours
MAXIMUM MARKS: 100 Marks
CHEMISTRY, PAPER-I
Attempt FIVE questions in all, Including Questions No.1 which is COMPULSORY, All questions carry EQUAL marks.
PART-I COMPULSORY QUESTION
1. Which of the following does not have the ground-state configuration 1s²2s²2p⁶?
(A) Ne
(B) Na⁺
(C) Cl⁻
(D) None of these
2. A reaction is exothermic if:
(A) ΔH > 0
(B) ΔH < 0
(C) ΔG > 0
(D) ΔG < 0
3. In chemometrics, multivariate calibration involves:
(A) Using multiple independent variables to predict dependent variables
(B) Using regression only on X-data
(C) Performing correlation without regression
(D) None of these
4. Langmuir isotherm assumes:
(A) Multilayer adsorption
(B) Uniform surface without interactions between adsorbed molecules
(C) Gas behaves as ideal
(D) None of these
5. A zero-order reaction rate does not depend on:
(A) Temperature
(B) Pressure
(C) Reactant concentration
(DNormally I can help with things like this, but I don’t seem to have access to that content. You can try again or ask me for something else.
PART-II
NOTE: (i) Part-II is to be attempted on the separate Answer Book.
(ii) Attempt ONLY FOUR questions from PART-II by selecting TWO questions from EACH SECTION. ALL questions carry EQUAL marks.
(iii) All the parts (if any) of each Question must be attempted at one place instead of at different places.
(iv) Write Q. No. in the Answer Book in accordance with Q. No. in the Q.Paper.
(v) No Page/Space be left blank between the answers. All the blank pages of Answer Book must be crossed.
(vi) Extra attempt of any question or any part of the question will not be considered.
(vii) Use of Calculator is allowed.
Q. 2. (a) Define adsorption and explain its types. Derive an expression for the Langmuir adsorption isotherm and discuss factors influencing adsorption on solids. (08)
(b) Why are transition metal complexes often colored? Explain using crystal field theory with an example. (07)
(c) Compare and contrast the Lewis concept and the Bronsted-Lowry theory of acids and bases. Include relevant examples and limitations. (05) (20)
Q. 3. (a) What is lanthanide contraction? Analyze its impact on the atomic radii and chemical properties of lanthanides and post-lanthanides. (08)
(b) Analyze the quantum numbers associated with atomic orbitals and describe their importance in explaining electron configurations. (07)
(c) Describe the catalytic activity of transition metals with reference to their variable oxidation states. Support your explanation with one example. (05) (20)
Q. 4. (a) Derive the Gibbs free energy equation from the first and second laws of thermodynamics and discuss its importance in predicting the spontaneity of chemical reactions. (10)
(b) Explain the principle of fractional distillation. Compare it with simple distillation using a diagram and examples of their applications. (05)
(c) Adsorption isotherms fail at high pressure. Why? Explain with reference to the limitations of the Freundlich isotherm. (05) (20)
Q. 5. (a) Why are Lewis acids and bases more versatile in their applications than Bronsted-Lowry acids and bases? Provide two examples to support your answer. (10)
(b) Derive the integrated rate law for a first-order reaction and explain why the half-life of such a reaction is independent of its initial concentration. (05)
(c) State and explain the Heisenberg Uncertainty Principle. How does it limit our ability to precisely determine the position and momentum of particles? (05) (20)
Q. 6. (a) Discuss the Freundlich adsorption isotherm. Derive the equation and highlight its limitations. (07)
(b) Using a diagram, explain the principle and working of a galvanic cell. Discuss its components with the example of a Zn-Cu system. (07)
(c) Why does an exothermic reaction sometimes become non-spontaneous at high temperatures? (06) (20)
Q. 7. (a) Explain the relationship between entropy, enthalpy, and Gibbs free energy. Derive an expression for equilibrium using these thermodynamic quantities. (08)
(b) Derive the first law of thermodynamics and explain its connection with internal energy and enthalpy. (07)
(c) Define the concept of activation energy and illustrate its significance in reaction kinetics using the Arrhenius equation. (05) (20)
Q. 8. Define the following: (5 each) (20)
(a) Difference between Homogenous and Heterogenous Catalysis
(b) Define Molecular Orbital Theory (MOT)
(c) Difference between ANOVA and Gaussian Distribution
(d) Define Chromatography and write key differences between Paper Chromatography and Gas Chromatography
×