It is general principle that the less energy a system contains. It is

When 50 cm³ of a strong acid is added to 50 cm³ of an alkali, the temperature rises by 5^o If 250 cm³ of each liquid are mixed the temperature rise would be

(A)  5^oC                                     (B)  10^oC                                    (C)   25^oC                                  (D)  20^oC

A well stoppered thermos flask contains some ice cubes. This is an example of a

Which of the following is zero during adiabatic expansion of the gas

Identify the intensive quantity from the following

Identity the extensive properties in the following (I) Entropy, (II) Coulomb, (III) Specific heat, (IV) Volume

An isolated system is that system in which

Which of the following is a closed system

Leaving one system, rest solar system is known as

Point out the wrong statement in relation to enthalpy

Which of the following is zero for an isochoric process

Which one of the following statements is false

An adiabatic expansion of an ideal gas, always has  

One calorie is equal to

Joule-Thomson expansion is

Two moles of an ideal gas expand spontaneously into a vacuum. The work done is

For adiabatic process

Internal energy is an example of

The process, in which no heat enters or leaves the system, is termed as

A solution of 500 ml of 0.2 M KOH and 500 ml of 0.2 M HCl is mixed and stirred; the rise in temperature is T₁. The experiment is repeated using 250 ml. each of solution, the temperature raised is T₂ Which of the following is true

(A) T₁ = T₂                                (B)  T₁ = 2T₂                               (C)   T₁ = 4T₂                                  (D)   T₂ = 9T₁

Mechanical work is specially important in system that contain

For an adiabatic process, which of the following is correct

Which of the following is a state variable property

An irreversible process occuring isothermally in an isolated system leads to

During an isothermal expansion of an ideal gas its

In an isochoric process the increase in internal energy is

Which of the following unit represents largest amount of energy

Atomic energy is expressed in

The intensive property among these quantities is

Which of the following is a extensive properties

In thermodynamics which one of the following is not an intensive property

Assertion (A) : During an adiabatic process, heat energy is not exchanged between system and its surroundings

Reason (R) : The temperature of a gas increases when it undergoes an adiabatic expansion     

In thermodynamics, a process is called reversible when

Energy equivalent to one erg, one joule and one calorie is in the order

In an isobaric process ratio of heat supplied to the system (dQ) and work done by the system (dW) for diatomic gas is

Out of P, V and T

Zeroth law is connected with

Which is not state function

The first law of thermodynamics is only

The spontaneous flow of heat is always

The entropy of a perfectly crystalline substance at absolute zero is zero. The state corresponds to which law of thermodynamics

From Kirchhoff’s equation which factor affects the heat of reaction

The law of Lavoisier and Laplace illustrates

“The quantity of heat which must be supplied to decompose a compound into its elements is equal to the heat evolved during the formation of that compound from its elements.” This statement is known as

“The resultant heat change in a reaction is the same whether it takes place in one or several stages.” This statement is called

Hess’s law of constant heat summation is based on

Hess law is applicable for the determination of heat of

Hess law deals with

Which of the following expressions represents the first law of thermodynamics

According to Hess’s law

(A)   K_p = K_c × (RT)^∆n
(B)   ∆H is always positive
(C)   The enthalpy change of a given chemical reaction is same whether the process takes place in one or several steps
(D)  None of these

One mole of real gas at 300 K is expanded isothermally from an initial volume of 1 litre to 10 litre . The  for this process is (R = 2calmol^-1K^-1)

Carnot cycle is the application of

One mole of an ideal gas at 300 K is expanded isothermally from an initial volume of 1 litre to 10 litres. The change in energy for this process is (R = 2calmol^-1K^-1)

If a refrigerator’s door is opened, then we get

Internal energy does not include

Equal volumes of monoatomic and diatomic gases at same initial temperature and pressure are mixed. The ratio of specific heats of the mixture (C_p / C_v) will be

A gas deviates most from ideal behaviour when it is subjected to

What is true

(A) C_p – C_v = R                     (B) C_p – C_v = PΔV                     (C) R = PΔV                   (D) All are correct

Value of r for polyatomic gas is

Which of the following is the correct equation

(A) ΔU = ΔQ – W                            (B) ΔW = ΔU + ΔQ                     (C) ΔU = ΔW + ΔQ                           (D) None of these

Equation is expressed for

The relation between change in internal energy (ΔE), change in enthalpy (ΔH) and work done (W) is represented as

(A) ΔH = ΔE + W                        (B) W = ΔE – ΔH                      (C) ΔE = W – ΔH                     (D) ΔE = ΔH + W

The temperature of sink is always

Internal energy can be determined experimentally using a

Work done by an ideal gas under isothermal reversible process is

(A)                                               (B) 

(C)                                                          (D) None of these

In which of the following ΔE = ΔH

(A) N₂O₂(g) ⇌ 2NO₂(g)                                                          (B) 2SO₂(g) + O₂(g) ⇌ 2SO₃(g)
(C) H₂(g) + I₂(g) ⇌ 2HI(g)                                                       (D) H₂(g) + 1/2O₂(g) ⇌ H₂O(l)

To calculate the amount of work done in Joules during reversible isothermal expansion of an ideal gas, the volume must be expressed in

(A) m³ only                          (B) dm³ only                           (C) cm³ only                             (D) Any one of them

The work done on a system is 4 Joule when 20 Joule heat is released from it then what is the decreases in internal energy of the system

A system is changed from state A to state B by one path and from B to A another path. If E₁ and E₂ are the corresponding changes in internal energy, then

(A) E₁ + E₂ = -ve                                    (B) E₁ + E₂ = +ve                                    (C) E₁ + E₂ = 0                                   (D) None of these

Hess law is based on

Which expression is correct for the work done in adiabatic reversible expansion of an ideal gas

(A)                            (B)                                   (C)                               (D)

Mass and energy are conserved is demonstrated by

In a closed insulated container, a liquid is stirred with a paddle to increase its temperature. In this process, which of the following is true

(A) ΔE = W = Q = 0                                                     (B) ΔE ≠ 0 , Q = W = 0
(C) ΔE = W ≠ 0 , Q = 0                                                (D) ΔE = Q ≠ 0 , W = 0

A heat engine absorbs heat Q₁ at temperature T₁ and heat Q₂ at temperature T₂. Work done by the engine is (Q₁ + Q₂). This data

(A) Violates I^st law of thermodynamics                                      (B) Violates I^st law of thermodynamics if Q₁ is –ve
(C) Violates I^st law of thermodynamics if Q₂ is  –ve                  (D) Does not violate I^st law of thermodynamics

Second law of thermodynamics

The law formulated by Dr. Nernst is

Assertion (A) : Absolute value of internal energy of the substances can not be determined
Reason (R) : It is impossible to determine the exact values of the constituent energies of substance

For the reaction, CH₃COOH(l) + 2O₂(g) ⇌ 2CO₂(g) + 2H₂O(l) at 25˚C and 1 atm pressure, ΔH = -874kJ. Then the change in internal energy (ΔE) is ……..

First law of thermodynamics does not show

The work done to contract a gas in a cylinder, is 462 Joules, 128 Joule energy is evolved in the process. What will be the internal energy change in the process

According to Hess’s law, the heat of reaction depends upon

Calculate the work done during isothermal expansion of one mole of an ideal gas from 10 atm to 1 atm at 300K

Find out the energy which is supplied to Carnot cycle if it is working between 95˚C to 15˚C . Maximum work of this engine is 214 cal.

The volume of a gas decreases from 500 cc to 300 cc when a sample of gas is compressed by an average pressure of .6 atm. During this process 10 J of heat is liberated. The change in internal energy is

An exothermic reaction is one in which the reacting substances

An exothermic reaction is one which

An endothermic reaction is one in which

Which of the following is an example of endothermic reaction

(A)
(B)
(C)
(D)

The following is an endothermic reaction 

If the enthalpy of B is greater than of A, the reaction A → B  is

The heat of formation of carbon dioxide is – 90.4 kcal. This shows that

(A) CO₂   is exothermic compound                                              (B) CO₂ is endothermic compound
(C) CO₂ is isothermal compound                                                 (D) None of these

The compound with negative heat of formation are known as

All reactions with chemical dissociation are

The formation of water from H₂(g) and O₂(g) is an exothermic reaction because

(A) The chemical energy of H₂(g)  and O₂(g) is more than that of water 
(B) The chemical energy of H₂(g)  and O₂(g) is less than that of water
(C) Not dependent on energy
(D) The temperature of H₂(g)  and O₂(g) is more than that of water

In exothermic reactions

When water is added to quick lime the reaction is

Fermentation is a reaction called

In an endothermic reaction, the value of ΔH  is

Nuclear reactor is the example of

Bond formation is process of

Which of the following is endothermic exothermic reaction

Heat of formation ,  of an explosive compound like NCl₃ is 

Which of the following is not expected to be correct

(A)  = Negative
(B)  = Positive
(C)    = Negative
(D)  = Negative

Enthalpy change for a reaction does not depend upon

Dissolution of gases in water is

A reaction that takes place with the absorption of energy is

Which of the following reactions is not exothermic

(A) 
(B) 
(C) 
(D) 

Which of the following endothermic processes are spontaneous

For exothermic reaction, the equilibrium constant

O^– + e^– → O^— is the process of

The energy evolved is highest for which of the following reactions

(A)  F + e → F^–                          (B)  Cl + e → Cl^–                        (C)  S + 2e → S^2–                        (D)  O + 2e → O^2–

Ozone is prepared by passing silent electric discharge through oxygen. In this reaction

Which of the following statements is correct about heat of combustion

Which of the following is an endothermic reaction

(A)  2H₂ + O₂ → 2H₂O
(B)  N₂ + O₂ → 2NO
(C)  2NaOH + H₂SO₄ → Na₂SO₄ + 2H₂O
(D)  3O₂ + C₂H₅OH → 2CO₂ + 3H₂O

Which of the following reaction is endothermic

(A)  CaCO₃ → CaO + CO₂                                                          (B)  Fe + S → FeS

(C)  NaOH + HCl → NaCl + H₂O                                              (D)  CH₄ + 2O₂ → CO₂ + 2H₂O

The equation means

(A)  The heat absorbed when one gram molecule of HCl is formed from its elements at 25^oC is 22.060 kcal
(B)  The heat given out when one gram molecule of HCl is formed from its elements at 298 K is 22.060 kcal
(C)  The heat absorbed when one atom of hydrogen reacts with one atom of chlorine to form one molecule of HCl at 25^oC and one atom of chlorine to form one molecule of HCl at 25^oC and one atmosphere pressure is 22.060 kcal
(D)  The heat absorbed when one gram equivalent of HCl is formed from its elements at 298 K is 22.060 kcal
(E)  The intrinsic heat of one molecule of HCl is 22.060 kcal more than the intrinsic heats of one atom of hydrogen and one atom of chlorine

(I) C + O₂ → CO₂                        (II) N₂ + 3H₂ → 2NH₃                    (III)  NH₄Cl → NH₃ + HCl
Which is endothermic process

Ionisation process and formation process are called

Which of the following is not an endothermic reaction

(A)                                                        (B) 
(C)                                                                            (D)  All of these

Evaporation of water is

The total entropy change for a system and its surroundings increases if the process is

Enthalpy of formation of two compounds x and y are – 84 kJ and – 156 kJ Which of the following statements is correct

Internal energy of an ideal gas depends on

If C + O₂ → CO₂ + 94.2 kcal;  kcal ; CH₄ + 2O₂ → CO₂ + 2H₂O + 210.8 kcal, then the possible heat of methane will be

The enthalpy of vaporisation of water is

Heat of reaction at constant volume is equal to its thermodynamical quantity

In which of the following neutralisation reactions, the heat of neutralisation will be highest

(A)  NH₄OH and CH₃COOH                                                         (B)  NH₄OH and HCl
(C)  NaOH and CH₃COOH                                                           (D)  NaOH and HCl

Heat of reaction at constant pressure is equal to its thermodynamical quantity

Which one of the following process is not spontaneous

(A)  Dissolution of CuSO₄ in water                                      (B)  Reaction between H₂ and O₂ to form water

(C)  Water flowing down hill                                                 (D)  Flow of electric current from low potential to high potential

The molar neutralization heat for KOH and HNO₃ as compared to molar neutralization heat of NaOH and HCl

Thermochemical reactions,

From the above reaction, the heat of reaction for will be

Heat of vapourisation of A (l) is x₁ cal and heat of fusion of A(s) is x₂. Hence heat of sublimation of A (s) is

(A)  x₁ – x₂                                 (B)  x₂ – x₁                                 (C)  x₁ + x₂                                    (D)  -(x₁ + x₂)

 kcal mol^–1 ; . Which is/are correct statement (s)

(A)  Heat of formation of CO₂ is –68 kcal mol^–1                                  (B)  Heat of combustion of CO(g) is –68 kcal mol^–1

(C)  Heat of combustion of C(s) is –26 kcal mol^–1                                (D)  None of these

The heat liberated when 10 gm NaOH reacts with an excess of H₂SO₄ in dilute solution is nearly

Which of the following is the chemical interpretation of the statement that the heat of formation of methanol is -239 kJ mol^–1

(A)  CO + 2H₂ → CH₃OH                                                                (B)        

(C)                                                 (D)  All of these

Heat of neutralisation of H₂C₂O₄ (oxalic acid) is – 26 kcal mol^–1. Hence dissociation energy of   is

(A)  12.3 kcal mol^–1                            (B)  1.4 kcal mol^–1                           (C)  – 13.7 kcal mol^–1                       (D)  – 1.4 kcal mol^–1

The heat of transition (∆H_t) of graphite into diamond would be, where
C(graphite) +
C(diamond) +

(A)                           (B)                                       (C)                              (D)  None of these

Correct relationship between heat of fusion (∆H_fus), heat of vaporization (∆H_vap) and heat of sublimation (∆H_sub) is

(A)                                              (B) 
(C)                                             (D)               

Given that,



Heat of formation of acetylene is

Heat of neutralisation of a strong acid by a strong base is a constant value because

Heat of neutralisation of an acid by a base is highest when

Heat of neutralization of a strong acid against strong base is constant and is equal to

(A)  13.7 kcal                            (B)  57 kJ                              (C)  5.7 × 10⁴ J                             (D)  All of these

The value of heat generated when 36.5 gm HCl and 40 gm of NaOH reacts during neutralization

In the reaction ;  ∆H is known as

Heat of combustion of a substance

The heat change for the reaction is called

∆H values for reactions, and are – 100 and 200 kJ respectively. The heat of reaction for the reaction will be

Heat produced in calories by the combustion of one gram of carbon is called

Enthalpy change for reaction is called

The enthalpy of neutralization is about 57.3 kJ for the pair

(A)  HCl and NH₄OH                                        (B)  NH₄OH and HNO₃
(C)  H₂SO₄ and NaOH                                     (D)  CH₃COOH and NaOH

The mutual heat of neutralisation of 40 gm of NaOH and 60 gm CH₃COOH will be

Burning of thing is the process of

The heat of combustion ΔH of C(s) is –94.0 kcal. The heat of formation of CO₂ is

Heat of neutralisation of NH₄OH and HCl is 

What is true

(A) W = PΔV (For C_p)                                                                        (B) W = 0 (For C_p)
(C) C_v = 3/2R (For monoatomic gas)                                            (D) C_v = R (For monoatomic gas)

The heat of reaction does not depend upon

In the reaction ; ΔH represents

The heats of combustion of rhombic and monoclinic sulphur are respectively 70960 and 71030 calories. What will be the heat of conversion of rhombic sulphur to monoclinic

The heat of formation of H₂O(l) is – 68.0 kcal, the heat of formation of H₂O(g) is likely to be

The heat of combustion of carbon is – 94 kcal at 1 atm The intrinsic energy of CO₂ is