Mock Test

Exam: BPSC Subject: General Science Topic: Chemistry

Total Questions: 20

Q1. The rate-determining step in a multi-step reaction is the step that:

Is the fastest Is the slowest Produces the most product Requires the least activation energy
Q2. The relationship between the standard free energy change (ΔG°) and the standard cell potential (E°cell) is given by:

ΔG° = -nFE°cell ΔG° = nFE°cell ΔG° = FE°cell/n ΔG° = nE°cell/F
Q3. Which of the following is an example of heterogeneous catalysis?

Enzyme catalysis Acid-base catalysis Contact process for sulfuric acid Hydrolysis of ester
Q4. Which of the following molecules is likely to have the strongest dipole-dipole interactions?

CH4 CO2 HCl N2
Q5. What is the SI unit for absorbed dose of radiation?

Roentgen Rad Gray Curie
Q6. Which technique is used to detect and quantify analytes based on their interaction with specific antibodies or antigens?

Spectroscopy Chromatography Immunoassays Titration
Q7. The lanthanides and actinides are collectively known as:

Transition metals Halogens Inner transition metals Noble gases
Q8. What is a common application of complexometric titrations?

Determining the concentration of acids and bases Determining the concentration of metal ions Determining the amount of precipitate formed Determining the redox potential of a solution
Q9. The formation of allotropes of carbon like fullerenes is a testament to the versatility of carbon bonding. Which of the following fullerene structures is known as buckyball?

C70 C84 C60 C120
Q10. Which of the following indicators would be most suitable for the titration of a weak acid with a strong base?

Methyl orange Bromothymol blue Phenolphthalein Methyl red
Q11. The van der Waals equation is a modification of the ideal gas law that accounts for:

The volume of gas molecules and intermolecular attractive forces The number of moles and temperature Pressure and volume changes only The constant 'R'
Q12. What is the relationship between the change in Gibbs Free Energy (ΔG) and spontaneity?

ΔG > 0 indicates a spontaneous reaction. ΔG < 0 indicates a spontaneous reaction. ΔG = 0 indicates a spontaneous reaction. The sign of ΔG does not determine spontaneity.
Q13. The regulation of amino acid metabolism is crucial. Which enzyme is primarily responsible for the transamination of amino acids, transferring an amino group from an amino acid to an alpha-keto acid?

Glutamate dehydrogenase Aspartate aminotransferase (AST) Alanine transaminase (ALT) Glutamine synthetase
Q14. The change of a substance from the gaseous state directly to the solid state is known as:

Melting Vaporization Condensation Deposition
Q15. What is the effect of increasing temperature on the equilibrium constant (K) for an endothermic reaction?

K increases. K decreases. K remains unchanged. The effect depends on the concentration of reactants.
Q16. Which element is the most electronegative?

Carbon Nitrogen Oxygen Fluorine
Q17. What is the enthalpy change for the reverse reaction if the forward reaction is exothermic?

Same as forward Opposite sign Zero Double the value
Q18. For a reaction at equilibrium, the standard Gibbs free energy change (ΔG°) is related to the equilibrium constant (K) by:

ΔG° = -RT ln K ΔG° = RT ln K ΔG° = RT K ΔG° = -RT / K
Q19. Consider the electrolysis of aqueous CuSO4 using a copper anode and a platinum cathode. What are the reactions occurring at the anode and cathode?

Anode: Cu(s) -> Cu²⁺(aq) + 2e⁻; Cathode: Cu²⁺(aq) + 2e⁻ -> Cu(s) Anode: 2H₂O(l) -> O₂(g) + 4H⁺(aq) + 4e⁻; Cathode: Cu²⁺(aq) + 2e⁻ -> Cu(s) Anode: Cu(s) -> Cu²⁺(aq) + 2e⁻; Cathode: 2H₂O(l) + 2e⁻ -> H₂(g) + 2OH⁻(aq) Anode: 2H₂O(l) -> O₂(g) + 4H⁺(aq) + 4e⁻; Cathode: 2H₂O(l) + 2e⁻ -> H₂(g) + 2OH⁻(aq)
Q20. Which of the following has the least kinetic energy among the given states of matter at the same temperature?

Gas Liquid Solid Plasma

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