1. When a mor o atomic gas undergoes an adiabatic process, its temperatuer and volume are related by the equation TVn = constant, the value of n will be (A) 1.33(B*) 0.33(C) 2.33(D) 12.The difference between the heats of reaction at constant pressure and a constant volume for the reaction 2C6H6(l) + 15O2(g) CO2(g) + 6H2O(l) at 25C in kJ is (A*) -7.43(B) +3.72(C) -3.72(D) +7.433.A mono atomic gas X and a diatomic gas Y, both initially at the same temperature and pressure are compressed adiabatically from a volume V to V/2, which gas will be at higher temperature(A*) X(B) Y(C) both the same(D) cant say7.A sample of oxygen gas expands its volume from 3 litre to 5 litre against a constant pressure of 3 atm. If the work done during expansion be used to heat 10 mole of water initially present at 290 K, its final temperature will be(Specific heat capacity of water = 4.18 J k-1 g-1)(A) 292.0 k(B*) 290.8 k(C) 298.0 k(D) 293.7 k8.The molar heat capacity of water in equilibrium with ice at constant pressure is (A) zero (B*) infinity (C) 40.45 kJ K-1 mol-1(D) 75.48 J K-1 mol-19.One mole of ice is converted into water at 273 K. The entropies of H2O(s) and H2O(l) are 38.20 and 60.01 J mole-1 K-1 respectively. The enthalpy change for the conversion is (A) 59.54 J mol-1(B*) 5954 J mole-1(C) 594.5 J mole-1(D) 320.6 J mole-110.The for CO2(g), CO(g) and H2O(g) are -393.5, -110.5 and -241.8 kJ. mole-1 respectively. The standard enthalpy change in kJ for the reaction.CO2(g) + H2(g) CO(g) + H2O(g) is (A) + 524.1(B*) + 41.2(C) - 262.5(D) - 41.211.The difference between heats of reaction at constant pressure and constant volume of the following reaction, would be 2C6H6(l) + 15O2(g) CO2(g) + 6H2O(l) at 25C in kJ mol-1 is(A*) -7.43(B) +3.72(C) -3.72(D) +7.4312.The product of combustion of an aliphatic thiol (RSH) at 298 K are(A) CO2(g), H2O(g) and SO2(g)(B*) CO2(g), H2O(l) and SO2(g)(D) CO2(g), H2O(g) and SO2(l)(D) CO2(g), H2O(l) and SO2(l)13.For the combustion reaction at 298 K2Ag(s) + 1/2 O2(g) 2Ag2O(s)Which of the following relation will be true?(A) H = U(B) H > U(C*) H < U(D) H and U bear no relation with each other14.For which of the following equations, will H be equal to U?(A) H2(g) + 1/2 O2(g) H2O(l)(B*) H2(g) + l2(g) 2Hl2(g)(D) 2NO2(g) N2O4(g) (D) 4NO2(g) + O2(G) 2N2O5(g)16.The molar enthalpies of combustion of C2H2(g), C(graphite) and H2(g) are - 1300, -394 and -286 kJ mol-1, respectively. The standard enthalpy of formation of C2H2(g) would be (A) -226 kJ mol-1(B) -626 kJ mol-1(C*) 226 kJ mol-1|(D) 626 kJ mol-117.The for CO2(g), CO(g) and H2O(g) are -393.5, -110.5 and -241.8 kJ. mole-1 respectively. The standard enthalpy change in kJ for the reaction.CO2(g) + H2(g) CO(g) + H2O(g) is (A*) + 524.1(B) + 41.2(C*) - 262.5(D) - 41.2 22.A system is provided 50 J of heat and work done on the system is 10 J. The change in internel energy during the process is (A) 40 J (B*) 60 J (C) 80 J(D) 50 J23.The G in the process of melting of ice at - 15C would be(A) G is -ve(B*) G is +ve(C) G = 0(D) All of these24.Temperature of 1 mole of a gas is increased by 1 at constant pressure. The work done is (A*) R (B) 2R(C) R/2(D) 3R26.The standard enthalpies of formation at 300 K for CCl4(l), H2O(g), CO2(g) and HCl(g) are -107, -242, -394 and -93 kJ mol-1, respectively. The value of U300K for the following reaction, would beCCl1(l) + 2H2O(g) CO2(g) + 4HCl(g)(A) -170 kJ mol-1(B) -175 kJ mol-1(C*) -182.5 kJ mol-1(D) -282.5 kJ mol-128.The enthalpy of vaporization of water at 100C is 40.63 kJ mol-1. The value U for this process would be (A*) 37.53 kJ mol-1(B) 39.08 kJ mol-1(C) 42.19 kJ mol-1(D) 43.73 kJ mol-1|29.Which of the following expressions will be true?(A) (CO, g) = 1/2 (CO2, g) (B) (CO, g) = (C, graphite) + 1/2 (O2, g)(C) (CO, g) = (CO2, g) - 1/2 (O2, g) (D*) (CO, g) = (C, graphite) + (CO, g) 31.For a monatomic gas, the value of the ratio of CP, m and CV , m is (A*) 5/3(B) 7/5(C) 9/7(D) 9/1132.In a flask colourless N2O4 is in equilibrium with brown coloured NO2. At equilibrium when the flask is heated at 100C, the brown colour deepens and on cooling it becomes less coloured. The change in enthalpy, H for this system will be(A) Negative(B*) Positive(C) Zero(D) Undefined36.Which of the following statement will be true?(A) - = R(B) > (C) for ideal gas is zero (D*) All of these37.Latent heat of vaporisation of a liqiud at 500 K and 1 atm pressure is 10.0 kcal mol-1. What will be the change in internal energy of 3 mole of liquid at same temperature?(A) 13.0 kcal(B) -13.0 kcal(C*) 27.0 kcal (D) -27.0 kcal38.The work done in an open vessel at 300 K, when 112 g iron reacts with dil. HCl, will be(A*) 1200 cal(B) 600 cal(C) 300 cal (D) 200 cal39.16 g oxygen gas expands at STP to occupy double of its original volume. The work done during the process will be(A) 260 kcal(B) 180 kcal(C) 130 kcal(D*) 272.84 kcal40.One mole of ice is converted into water at 273 K. The entropies of H2O(s) and H2O(l) are 38.20 and 60.01 J mol-1 K-1 respectively. The enthalpy change for the conversion will be (A) 59.54 J mol-1(B*) 5954 J mol-1(C) 595.4 J mol-1|(D) 320.6 J mol-141.One mole of anhydrous MgCl2 dissolves in water and liberates 25 cal/mol of heat. Hhydration of MgCl2 = 30 cal/mole. Heat of dissolution of MgCl2H2O is :(A*) +5 cal/mol(B) 5 cal/mol(C) 55 cal/mol(D) 55 cal/mol42.One mole of an ideal gas at 300 K is expanded isothermally from an initial volume of 1 litre to 10 litres. The E for this process is (R = 2 cal mol1 K1) :(A) 163.7 cal(B*) zero(C) 138.1 cal(D) 9 lit atm43.If a refrigerators door is opened, then we get :(A*) Room heated(B) Room cooled(C) More heat is passed out(D) No effect on room44.2.1 gm of Fe combines with S evolving 3.77 kJ. The heat of formation of FeS in kJ/mole is:(A) 3.77(B) 1.79(C*) 100.5(D) None of these45.H2(g) + O2 H2O(g)H = 241.8 kJC2H2(g) + 2O2(g) 2CO2(g) + H2O(g)H = 1300 kJEqual volumes of C2H2 and H2 are combustion under identical conditions. The ratio of heats evolved in the two cases is :(A*) 5.37/1(B) 1/5.37(C) 1/1(D) None of these47.For the combustion of methane at 25C, the difference between H and E will be :(A) 4 4.184 298 J(B) +4 4.184 298 J(C*) 2 4.184 298 J(D) zero50.The standard heat of combustion of propane is 2220.1 kg mole1. The standard heat of vaporisation of liquid water is 44.0 kJ mole1. What is H of :C3H8(g) + 5O2 3CO2(g) + 4H2O(g)(A) 2220.1 kJ(B*) 2044.1 kJ(C) 2396.1 kJ(D) 2176.1 kJ51.Given the standard enthalpies at 25C, in kilojoules per mole, for the following two reactions:Fe2O3(s) + C(s) CO2(g) + 2Fe(s)H = +234.1C(s) + O2(g) CO2(g)H = 393.5The H value for 4Fe(s) + 3O2(g) 2Fe2O3(s) is calculated as :(A) (393.5) 234.1(B) (393.5) + 234.1(C) 393.5 234.1(D*) 3(393.5) 2(234.1)52.Which of the following is a path function as well as an extensive property?(A) Temperature(B) Internal energy(C) Molar heat capacity(D*) Heat capatcity53.One gram atom of graphite and one gram atom of diamond were separately burnt to carbon dioxide. The amount of heat liberated were 393.5 kJ and 395.4 kJ respectively. It follows that:(A) Graphite has greater affinity for oxygen(B) Diamond has greater affinity for oxygen(C*) Graphite is stabler than diamond(D) Diamond is stabler than graphite

55.For a reaction to be spontaneous at all temperatures :(A*) G and H should be negative(B) G for the reaction is zero(C) G and H should be positive(D) H < G56.The total entropy change for a system and its surrounding increases, if the process is :(A) Reversible(B*) Irreversible(C) Exothermic(D) Endothermic57.In the following table, which are correct :HSNature of reaction(A)()(+)Spontaneous only at high temperature(B*)(+)()Nonspontaneous regardless of temperature(C)(+)(+)Spontaneous only at low temperature(D)()()Spontaneous at all temperature58.In which of the following case entropy decreases :(A*) Condensation of water vapour(B*) Expansion of a gas(C) Crystals dissolve(D) Polymerisation59.An adiabatic process is one in which :(A*) q = 0(B) Q = PdV(C*) E = w(D) E + VdP60.Which of the following statements are correct?(A*) The work done by the system on the surroudings is negative.(B*) The work done on the system by the surrounding is positive.(C*) The heat absorbed by the system from the surrounding is positive.(D*) The heat absorbed by the surrounding from the system is negative.61.61When the gas is ideal and the process is isothermal then :(A*) P1V1 = P2V2(B*) E1 = E2(C) H1 H2(D) W = 062.C(s) + O2 CO(g), H = 26 kcal mol1CO(g) + O2(g) CO2(g), H = 68 kcal mol1which is/are correct statement(s)?(A) Heat of formation of CO2 is 68 kcal mole1(B) Heat of combustion of C(s) is 26 kcal mole1(C*) Heat of combustion of CO(g) is 68 kcal mole1(D*) Heat of formation of CO(g) is 26 kcal mole163.Variation of heat of reaction with temperature is given by Kirchoffs equation, which is true :(A*) H2 = H1 + CP(T2 T1)(B*) = CP(C*) = CP(D) None is correct64.Which of the following reaction is exothermic :(A) CaCO3 CaO + CO2(B*) Fe + S FeS(C*) NaOH + HCl NaCl + H2O(D*) CH4 + 2O2 CO2 + 2H2O65.For an ideal gas, the relation between the enthalpy change and internal energy change at constant temperature is given by :(A) H = E + PV(B*) H = E + nRT (C*) H = E + PV (D) H = G + TS66.When a solid melts there will be :(A*) An increase in enthalpy(B*) A decrease in free energy(C) No change in enthalpy(D) Decrease in internal energy67.In a reaction H and S both are more than zero. In Which of the following cases, the reaction would not be spontaneous :(A*) H > TS(B*) S = (C) H < TS(D) All68.The heat of combustion of carbon is 394 kJ. The heat evolved in the combustion of 6.02 1022 atoms of carbon is :[IIT 1991](A) 3940 kJ(B) 394.0 kJ(C*) 39.4 kJ(D) 0.394 kJ69.Identify the intensive quantities from the following :[IIT 1993](A) enthalpy(B*) temperature(C) volume(D*) refractive index70.Consider an ideal gas. If 100 joules of work is done in compressing it under adiabatic conditions, then its :[IIT 1993](A) internal energy does not change and heat given out is zero.(B) internal energy does not change and heat given out is non-zero.(C) internal energy decreases by 100 joules and heat given out is zero.(D*) internal energy increases by 100 joules and heat given out is zero.72.Standard molar enthalpy of formation of CO2 is equal to :(A) zero(B) The standard molar enthalpy of combustion(C) The sum of standard molar enthalpies of formation of CO and O2(D*) The standard molar enthalpy of combustion of carbon (graphite)73.Molar heat capacity of water in equilibrium with ice at constant pressure is :(A) zero(B*) Infinity ()(C) 40.45 kJ K1 mol1(D) 75.48 JK1 mol174.One mole of a gas occupying 3 dm3 expands against constant external pressure of 1 atm to a volume of 13 dm3. The work done is :(A*) 10 atm dm3(B) 20 atm dm3(C) 39 atm dm3(D) 48 atm dm3 75.The enthalpy of solution of BaCl2(s) and BaCl2.2H2O(s) are 20.6 and 8.8 kJ mol1, respectively. The enthalpy for the reaction :BaCl2(s) + 2H2O BaCl2.2H2O(s) is :(A*) 29.4 kJ(B) 11.8 kJ(C) 20.6 kJ(D) 29.4 kJ76.For the reaction, A(g) + 2B(g) 2C(g) + 3D(g), the value of H at 27C is 19.0 kcal. The value of E for the reaction would be (R = 2.0 cal K1 mol1) :(A) 20.8 kcal(B) 19.8 kcal(C) 18.8 kcal(D*) 17.8 kcal77.Which of the following is (are) endothermic reactions(s) :(A) combustion of methane(B*) decomposition of water(C*) dehydrogenation of ethane to ethylene(D*) conversion of graphite to diamond78.At 300 K, the reaction which have following values of thermodynamic parameters occur spontaneously:(A*) G = 400 kJ mol1(B) H = 200 kJ mol1, S = 4 JK1 mol1(C*) H = 200 kJ mol1, S = 4 JK1 mol1(D*) H = 200 J mol1, S = 40 JK1 mol180.The Hf for CO2(g), CO(g) and H2O(g) are 393.5, 110.5 and 241.8 kJ mol1 respectively. The standard enthalpy change (in kJ) for the reaction CO2(g) + H2(g) CO(g) + H2O(g) is :(A) 524.1(B*) 41.2(C) 262.5(D) 41.281.For the reaction, N2(g) + 3H2(g) 2NH3(g)H = ?(A) E + 2RT(B*) E 2RT(C) E + RT(D) E RT82.In thermodynamics, a process is called reversible when :(A) surroundings and system change into each other(B) there is no boundary between system and surroundings(C*) the surroundings are always in equilibrium with the system(D) the system changes into the surroundings spontaneously83.One mole of a nonideal gas undergoes a change of state (2.0 atm, 3.0 L, 95K) (4.0 atm, 5.0 L, 245 K) with a change in internal energy, V = 30.0 L atm. The change in enthalpy (H) of the process in L atm is :(A) 40.0(B) 42.3(C*) 44.0(D) not defined84.The difference between heats of reaction in kJ at constant pressure & constant volume for the reaction . 2 C6H6 (l) + 15 O2 (g) 12 CO2 (g) + 6 H2O (l) at 25 C .(A*) - 7.43 (B) + 3.72 (C) - 3.72 (D) + 7.43 86.The product of combustion of an aliphatic thiol (RSH) at 298 k are :(A) CO2(g) , H2O(g) & SO2(g) (B*) CO2(g) , H2O(l) & SO2(g)(C) CO2(l) , H2O(l) & SO2(g) (D) CO2(g) , H2O(l) & SO2(l)87.Identify the intensive quantitities from the following :(A) Enthalpy (B*) Temperature(C) Volume (D*) refractive index 89.Molar heat capacity of water in equilibrium with ice at constant pressure is :(A) Zero (B*) Infinity (C) 40.45 J K -1 mol-1 (D) 75.48 J K -1 mol-1 90.Standard molar enthalpy of formation of CO2 is equal to : (A) Zero (B) the standard molar enthalpy of combustion of gaseous carbon (C) the sum of standard molar enthalpies of formation of CO & O2(D*) the standard molar enthalpy for combustion of C (graphite)