F.SC CHEMISTRY MCQS


1. The pH of 0.001 M HCl is

(2, 4, 3)

2. K ( rate constant) is dependent on

(temperature, concentration, volume)

3. The universal indicator in water shows the colour

(red, green, blue)

4. The pH of blood is

(7.3, 8.4, 5.6)

 
5. Absolute Zero is equal to

(273.16°C, -273.16°C)

6. The compounds having hydrogen bond generally have __________ boiling points.

(High, Low)

7. Surface tension __________ with the rise of temperature.

(Increases, Decreases)

8. Mercury forms __________ meniscus in a glass tube.

(concave, convex)

 
9. Two moles of water contains __________ molecules.

(6.02 x 1023, 1.204 x 1024, 3.01 x 1023)

10. One mole of Cl- ions contains __________ ions.

(6.02 x 1023, 1.204 x 1024, 3.01 x 1023)

11. 220 gms of CO2 contains __________ moles of CO2.

(One, Five, Ten)

12. In rounding off __________ figure is dropped.

(First, Last, No)

 
13. 3.7 x 104 contains __________ significant figures.

(2, 3, 5)

14. 9.40 x 10-19 contains __________ significant figures.

(2, 3, 5)

 
15. The S.I unit of mass is

(kilogram, gram, pound)

16. One mole of glucose contains __________ gms.

(100, 180, 342)

 
17. The freezing point of water in Fahrenheit scale is

(0°F, 32°F, 212°F)

18. All gases change to solid before reaching to

(-100°C, 0°C, -273°C)

19. Pressure of the gas is due __________ of the molecules on the wall of the vessel.

(Collisionns, Attraction, Repulsion)

20. Boiling point of water in absolute scale is __________.

(212°K, 100°K, 373°K)

21. Boyle’s Law relates __________.

(Pressure and volume, Temperature and volume, Pressure and temperature)

 
22. Anode rays consists of __________ particles.

(Negative, Positive, Neutral)

23. Atomic mass of an element is equal to the sum of

(electrons and protons, protons and neutrons, electrons and neutrons)

24. Neutrons were discovered by

(Faraday, Dalton, Chadwick)

25. The value of Plank’s constant is

(6.626 x 10-34, 6.023 x 1024, 1.667 x 10-28)

 
26. The sigma bond is __________ than pi bond.

(Weaker, Stronger, Unstable)

27. The sp3 orbitals are __________ in shape.

(Tetrahedral, Trigonal, Diagonal)

28. The shape of CH4 molecule is

(Tetrahedral, Trigonal, Diagonal)

29. The bond in Cl2 is

(Non polar, Polar, Electrovalent)

 
30. Ionic reactions of inorganic compounds are

(very slow, moderately slow, very fast)

31. The rate of __________ reactions can be determined.

(Very Slow, Moderately Slow, Very fast)

 
32. __________ is an example of weak acid.

(Hydrochloric Acid, Acetic Acid, Sulphuric Acid)

33. When NH4Cl is hydrolyzed, the solution will be

(Acidic, Basic, Neutral)

34. When Na2CO3 is hydrolyzed, the solution will be.

(Acidic, Basic, Neutral)

 
35. Chemical Equilibrium is __________ equilibrium.

(Dunamic, Static, Heterogeneous)

 

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