Q.1
Which of the following is closed system? [ KCET 1995]
  • a) Jet engine
  • b) Tea placed in steel kettle
  • c) Pressure cooker
  • d) Rocket engine during propulsion
Q.2
For the reaction C + O2 → CO2 ..[ BHU 1995]
  • a) ΔH > ΔE
  • b) ΔH < ΔE
  • c) ΔH=ΔE
  • d) none of these
Q.3
Enthalpy of a reaction ΔH is expressed as ... [ AIIMS 1996]
  • a) ΔH=∑ΔHp - ∑ΔHR
  • b) ΔH=dHp + dHR
  • c) ΔH=dHp / dHR
  • d) ΔH=∑Hp / dHR
Q.4
Given thatC + O2 → CO2 ; ΔH=-x kJ2CO + O2 → 2CO2; ΔH=-y kJthe enthalpy of formation of carbon monoxide will be .. [ CBSE PMT 1997]
  • a) (2x - y) / 2
  • b) (y - 2x) / 2
  • c) 2x - y
  • d) y=2x
Q.5
Enthalpy change (ΔH) of system depends on its ... [ Pb CET 1997]
  • a) Initial state
  • b) Final state
  • c) Both initial and final state
  • d) None of these
Q.6
Energy required to dissociate 4 g of gaseous hydrogen into free gaseous atoms is 208 kcal at 25°C. The bond energy H-H bond will be .... [ CPMT 1989]
  • a) 104 kcal
  • b) 10.4 kcal
  • c) 1040 kcal
  • d) 104 kcal
Q.7
The relation between enthalpy (H), pressure (P), volume (V) and internal energy (E) is given by .. [ MP PMT 1998]
  • a) E=H + PV
  • b) H=E + PV
  • c) H=E - PV
  • d) H=E + P + V
Q.8
Based on the following thermo chemical equationsH2O(g) + C(s) → CO(g) + H2(g); ΔH=131 kJCO(g) + ½O2(g) → CO2(g); ΔH=-282 kJH2(g) + ½O2(g) → H2O; ΔH=-242 kJC(s) + O2(g) → CO2(g); ΔH=X kJthe value of X will be .... [ CBSE PMT 1992]
  • a) -393 kJ
  • b) -655 kJ
  • c) +393 kJ
  • d) +655 kJ
Q.9
Identify the correct statement regarding entropy .. [ BHU 1998]
  • a) At absolute zero of temperature, entropy of a perfectly crystalline substance is taken to be zero
  • b) At absolute zero of temperature, the entropy of a perfectly crystalline substance is positive
  • c) Absolute entropy of a substance cannot be determined
  • d) At 0°C , the entropy of a perfectly crystalline substance is taken to be zero
Q.10
Equal volumes of methanoic acid and sodium hydroxide are mixed. If x is the heat of formation of water, then heat evolved on neutralization is ... [ BHU 1998]
  • a) more than x
  • b) equal to x
  • c) less than x
  • d) twice x
Q.11
The energy change of reaction C2H6(g) → 2C (g) + 6H(g) is X kJ The bond energy of C - H bond is ..[ Haryana CEET 1998]
  • a) X/6 kJ
  • b) X/3 kJ
  • c) X kJ
  • d) indeterminate
Q.12
For the process Dry ice → CO2(g) .. [ KCET 2000]
  • a) ΔH is positive and ΔS is negative
  • b) Both ΔH and ΔS are negative
  • c) Both ΔH and ΔS are positive
  • d) ΔH is negative where as ΔS is positive
Q.13
The enthalpy of neutralization of weak acid by a strong base is ... [ Tamil nadu CET 2001]
  • a) -57.32 kJ
  • b) +57.2 kJ
  • c) equal to -57.32 kJ + enthalpy of ionization of weak acid
  • d) more than -57.32 kJ
Q.14
Mechanical work is specially important in systems that contain
  • a) solid - liquid
  • b) liquid -liquid
  • c) solid - solid
  • d) gases
Q.15
If an endothermic reaction is non-spontaneous at freezing point of water and becomes feasible at its boiling point of water , then ... [ AIEEE 2002]
  • a) ΔH is -ve, ΔS is +ve
  • b) ΔH and ΔS both are +ve
  • c) ΔH and ΔS both are -ve
  • d) ΔH is +ve, ΔS is -ve
Q.16
The bond energy of O-H bond is 109 kcal/mol. When a mole of water is formed.. [ CBSE PMT 1990]
  • a) 218 kcal is released
  • b) 109 kcal is released
  • c) 218 kcal is absorbed
  • d) 109 kcal is absorbed
Q.17
If a reaction involves only solids and liquids, which of the following is true .. [ Tamilnadu CET 2002]
  • a) ΔH < ΔE
  • b) ΔH=ΔE
  • c) ΔH > ΔE
  • d) ΔH=ΔE + RTΔn
Q.18
Which of the following statements is true? ..[ KCE 2002]
  • a) ΔG may be lesser or greater or equal to ΔH
  • b) ΔG is always proportional o ΔH
  • c) ΔG is always greater than ΔH
  • d) ΔG is always less than ΔH
Q.19
Compounds with high heat of formation are less stable because .. [ KCET 2002]
  • a) It is difficult to synthesize them
  • b) energy rich state leads to instability
  • c) higher temperature is required to synthesize them
  • d) molecules of such compounds are distorted
Q.20
The law formulated by Nernst is ... [ kerala CET 2002
  • a) first law of thermodynamics
  • b) second law of thermodynamics
  • c) third law of thermodynamics
  • d) both a and b
Q.21
In a closed insulated container a liquid is stirred with a paddle to increase the temperature. Which of the following is true
  • a) ΔE=W ≠ 0, q=0
  • b) ΔE=W=q ≠ 0
  • c) ΔE=0, W=q ≠ 0
  • d) W=0, ΔE=q ≠ 0
Q.22
An adiabatic expansion of an ideal gas always has ... [ MP PMT 2002]
  • a) q=0
  • b) w=0
  • c) ΔH=0
  • d) decrease temperature
Q.23
The favorable conditions for a spontaneous reaction are .. [ MP PET 2002]
  • a) TΔS > ΔH, ΔH=+ve, ΔS=+ve
  • b) TΔS > ΔH, ΔH=+ve, ΔS=-ve
  • c) TΔS=ΔH, ΔH=-ve, ΔS=-ve
  • d) TΔS=ΔH, ΔH=+ve, ΔS=+ve
Q.24
H2(g) + Cl2(g) → 2HCl(g) ; ΔH=-44 kcal2Na(s) + 2HCl(g) → 2NaCl(s) + H2(g); ΔH=-152 kcalFor reactionNa(s) + ½Cl2(g) → NaCl(s); ΔH=?
  • a) -180 kcal
  • b) -196 kcal
  • c) -98 kcal
  • d) 54 kcal
Q.25
Heat exchanged in chemical reaction at constant temperature and pressure is called .. [ AFMC 1998]
  • a) entropy
  • b) enthalpy
  • c) internal energy
  • d) free energy
Q.26
According to second law of thermodynamics, a process ( reaction) is spontaneous, if during the process .. [ kerala MEE 2001]
  • a) ΔS universe > 0
  • b) ΔSuniverse=0
  • c) ΔHsystem > 0
  • d) ΔSuniverse < 0
Q.27
S + (3/2)O2 → SO3 + 2x calSO2 + ½O3 + y calFind out the heat of formation of SO2
  • a) ( y -2x)
  • b) ( 2x - y )
  • c) ( x + y)
  • d) 2x/y
Q.28
One mole of an ideal gas is allowed to expand freely and adiabatically into vacuum until its volume has doubled. The expression which is not true concerning statement is .. [ PB. PMT 1998]
  • a) ΔH=0
  • b) ΔS=0
  • c) ΔE=0
  • d) W=0
Q.29
The neutralization of strong acid by a strong base liberates an amount of energy per mole of H+ ... [ BHU 1998]
  • a) depends upon which acid and base are involved
  • b) depends upon the temperature at which the reaction takes place
  • c) depends upon which catalyst is used
  • d) is always same
Q.30
The enthalpy and entropy change for a chemical reaction are -2.5×103 cal and 7.4 cal/deg respectively. The reaction will be .. [ AFMC 1998]
  • a) spontaneous
  • b) reversible
  • c) irreversible
  • d) non - spontaneous
0 h : 0 m : 1 s