AIPMT 2015 Chemistry Model Test Paper - 1
Q.1. Which amongst the following is the most stable carbocation ?
Q.2. Products of the following reaction :
1) CH3CHO + CH3CH2CHO
2) CH3COOH + CH3COCH3
3) CH3COOH + HOOC . CH2CH3
4) CH3COOH + CO2
2) CH3COOH + CH3COCH3
3) CH3COOH + HOOC . CH2CH3
4) CH3COOH + CO2
Q.3. At 25°C, the dissociation constant of a base, BOH, is 1.0 x 10-12. The concentration of hydroxyl ions in 0.01 M aqueous solution of the base would be :
1) 1.0 x 10-6 mol L-1
2) 1.0 x 10-5 mol L-1
3) 1.0 x 10-8 mol L-1
4) 1.0 x 10-7 mol L-1
2) 1.0 x 10-5 mol L-1
3) 1.0 x 10-8 mol L-1
4) 1.0 x 10-7 mol L-1
Q.4. Which one of the following pairs represents stereoisomerism ?
1) Chain isomerism and rotational isomerism
2) Structural isomerism and geometric isomerism
3) Linkage isomerism and geometric isomerism
4) Optical isomerism and geomertric isomerism
2) Structural isomerism and geometric isomerism
3) Linkage isomerism and geometric isomerism
4) Optical isomerism and geomertric isomerism
The structure of the product D would be :
1) C6H5CH2NH2
2) C6H5NHCH2CH3
3) C6H5NHOH
4) C6H5CH2OH
2) C6H5NHCH2CH3
3) C6H5NHOH
4) C6H5CH2OH
Q.6. Identify the correct statement for change of Gibbs energy for a system (ΔGsystem) at constant temperature and pressure :
1) If ΔGsystem> 0, the process is spontaneous
2) If ΔGsystem= 0, the system has attained equilibrium
3) If ΔGsystem= 0, the system is still moving in a particular direction
4) If ΔGsystem< 0, the process is not spontaneous
2) If ΔGsystem= 0, the system has attained equilibrium
3) If ΔGsystem= 0, the system is still moving in a particular direction
4) If ΔGsystem< 0, the process is not spontaneous
Q.7. A solution containing 10g per dm 3 of urea (molecular mass = 60g mol-1) is isotonic with a 5% solution of a non-volatile solute. The molecular mass of this non-volatile solute is :
1) 200 g mol-1
2) 300 g mol-1
3) 400 g mol-1
4) 500 g mol-1
2) 300 g mol-1
3) 400 g mol-1
4) 500 g mol-1
Q.8. A plot of log x/m versus log p for the adsorption of a gas on a solid gives a straight line with slope equal to :
1) - log k
2) n
3) 1/n
4) log k
2) n
3) 1/n
4) log k
Q.9. Assume each reaction is carried out in an open container. For which reaction will ΔH = ΔE ?
1) H2(g) + Br2(g) → 2HBr(g)
2) C(s) + 2H2O(g) → 2H2(g) + CO2(g)
3) PCl5(g) → PCl3(g) + Cl2(g)
4) 2CO(g) + O2(g) → 2CO2(g)
2) C(s) + 2H2O(g) → 2H2(g) + CO2(g)
3) PCl5(g) → PCl3(g) + Cl2(g)
4) 2CO(g) + O2(g) → 2CO2(g)
Q.10. In a set of reactions propionic acid yielded a compound D.
CH3CH2COOH
The structure of D would be :
1) CH3CH2CH2NH2
2) CH3CH2CONH2
3) CH3CH2NHCH3
4) CH3CH2NH2
2) CH3CH2CONH2
3) CH3CH2NHCH3
4) CH3CH2NH2
Q.11. With which of the following configuration an atom has the lowest ionization enthalpy?
1)
2)
3)
4)
Q.12. An element, X has the following isotopic composition; 200X:90% ; 199X:8.0% ; 202X:2.0%
The weighted average atomic mass of the naturally occurring element X is closest to :
Q.13. Concentrated aqueous sulphuric acid is 98% H 2SO 4 by mass and has a density of 1.80 g. mL-1 . Volume of acid required to make one litre of 0.1 M H2SO4 is,
Q.14. Consider the following sets of quantum numbers:
Which of the following sets of quantum number is not possible
Q.15. The number of moles of KMnO4 that will be needed to react with one mole of sulphite ion in acidic solution is:
Q.16. If uncertainty in position and momentum are equal, then uncertainty in velocity is
Q.17. If a gas expands at constant temperature, it indicates that
Q.18. The value of equilibrium constant of the reaction
The equilibrium constant of the reaction
will be
Q.19. If 'a' stands for the edge length of the cubic systems : simple cubic, body centred cubic and face centred cubic, then the ratio of radii of the spheres in these systems will be respectively
Q.20. Kohlrausch's law states that at
Answer Key:
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2)
3)
4)
Q.12. An element, X has the following isotopic composition; 200X:90% ; 199X:8.0% ; 202X:2.0%
The weighted average atomic mass of the naturally occurring element X is closest to :
1) 199 amu
2) 200 amu
3) 201 amu
4) 202 amu
2) 200 amu
3) 201 amu
4) 202 amu
Q.13. Concentrated aqueous sulphuric acid is 98% H 2SO 4 by mass and has a density of 1.80 g. mL-1 . Volume of acid required to make one litre of 0.1 M H2SO4 is,
1) 5.55 mL
2) 11.10 mL
3) 16.65 mL
4) 22.20 mL
2) 11.10 mL
3) 16.65 mL
4) 22.20 mL
Q.14. Consider the following sets of quantum numbers:
| n | I | M | s | |
|---|---|---|---|---|
| a |
3
|
0
|
0
|
+1/2
|
| b |
2
|
2
|
1
|
+1/2
|
| c |
4
|
3
|
-2
|
-1/2
|
| d |
1
|
0
|
-1
|
-1/2
|
| e |
3
|
2
|
3
|
+1/2
|
1) a and c
2) b, c and d
3) a, b, c and d
4) b, d and e
2) b, c and d
3) a, b, c and d
4) b, d and e
Q.15. The number of moles of KMnO4 that will be needed to react with one mole of sulphite ion in acidic solution is:
1) 1
2) 3/5
3) 4/5
4) 2/5
2) 3/5
3) 4/5
4) 2/5
Q.16. If uncertainty in position and momentum are equal, then uncertainty in velocity is
1)
2)
3)
4)
2)
3)
4)
Q.17. If a gas expands at constant temperature, it indicates that
1) Number of the molecules of gas increases
2) Kinetic energy of molecules decreases
3) Pressure of the gas increases
4) Kinetic energy of molecules remains the same
2) Kinetic energy of molecules decreases
3) Pressure of the gas increases
4) Kinetic energy of molecules remains the same
Q.18. The value of equilibrium constant of the reaction
The equilibrium constant of the reaction
will be
A) 1/8
B) 1/16
C) 1/64
D) 16
B) 1/16
C) 1/64
D) 16
Q.19. If 'a' stands for the edge length of the cubic systems : simple cubic, body centred cubic and face centred cubic, then the ratio of radii of the spheres in these systems will be respectively
Q.20. Kohlrausch's law states that at
1) Infinite dilution, each ion makes definite contribution to equivalent conductance of an electrolyte, whatever be the nature of the other ion of the electrolyte
2) Finite dilution, each ion makes definite contribution to equivalent conductance of an electrolyte, whatever be the nature of the other ion of the electrolyte
3) Infinite dilution each ion makes definite contribution to equivalent conductance of an electrolyte depending on the nature of the other ion of the electrolyte
4) Infinite dilution, each ion makes definite contribution to conductance of an electrolyte whatever be the nature of the other ion of the electrolyte
2) Finite dilution, each ion makes definite contribution to equivalent conductance of an electrolyte, whatever be the nature of the other ion of the electrolyte
3) Infinite dilution each ion makes definite contribution to equivalent conductance of an electrolyte depending on the nature of the other ion of the electrolyte
4) Infinite dilution, each ion makes definite contribution to conductance of an electrolyte whatever be the nature of the other ion of the electrolyte
Answer Key:
Q.1-
|
2
|
Q.2-
|
3
|
Q.3-
|
4
|
Q.4-
|
4
|
Q.5-
|
4
|
|---|---|---|---|---|---|---|---|---|---|
Q.6-
|
2
|
Q.7-
|
2
|
Q.8-
|
3
|
Q.9-
|
1
|
Q.10-
|
4 |
| Q.11- | 4 | Q.12- | 2 | Q.13- | 1 | Q.14- | 4 | Q.15- | 4 |
Q.16-
|
2
|
Q.17-
|
4
|
Q.18-
|
3
|
Q.19-
|
2 |
Q.20-
|
1
|
We have tried our best to present important questions with correct answer key. Any suggestion or update about any erroneous entry or answer is always appreciable. Please comment your score or any suggestion in comment section below.
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