Among the following, the set of parameters that represents path function, is : (A) q + w (B) q (C) w (D) H–TS

During compression of a spring the work done is 10kJ and 2kJ escaped to the surroundings as heat. The change in internal energy, $$\Delta$$U(inkJ) is :

A process will be spontaneous at all temperatures if :

The difference between $$\Delta$$H and $$\Delta$$U ($$\Delta$$H – $$\Delta$$U), when the combustion of one mole of heptane(l) is carried out at a temperature T, is equal to :

Enthalpy of sublimation of iodine is 24 cal g–1 at 200 oC. If specific heat of I2(s) and l2 (vap) are 0.055 and 0.031 cal g–1K –1 respectively, then enthalpy of sublimation of iodine at 250 oC in cal g–1 is :

An ideal gas is allowed to expand form 1 L to 10 L against a constant external pressure of I bar. The work done in kJ is :

An ideal gas undergoes isothermal compression from 5m3 to 1 m3 against a constant external pressure of 4 Nm–2. Heat released in this process is used to increase the temperature of 1 mole of Al. If molar heat capacity of Al is 24 J mol–1 K–1, the temperature of Al increases by :

For diatomic ideal gas in a closed system, which of the following plots does not correctly describe the relation between various thermodynamic quantities?

The combination of plots which does not represent isothermal expansion of an ideal gas is –

Consider the reversible isothermal expansion of an ideal gas in a closed system at two different temperatures T1 and T2 (T1 < T2). The correct graphical depiction of the dependence of work done (w) on the final volume (V) is :

The entropy change associated with the conversion of 1 kg of ice at 273 K to water vapours at 383 K is : (Specific heat of water liquid and water vapour are 4.2 kJ K$$-$$1 kg$$-$$1 and 2.0 kJ K$$-$$1 kg$$-$$1; heat of liquid fusion and vapourisation of water are 334 kJ$$-$$1 and 2491 kJ kg$$-$$1, respectively). (log 273 = 2.436, log 373 = 2.572, log 383 = 2.583)

A process has $$\Delta$$H = 200 J mol–1 and $$\Delta$$S = 40 JK–1 mol–1. Out of the values given below, choose the minimum temperature above which the process will be spontaneous :

The process with negative entropy change is :

For the chemical reaction X $$\rightleftharpoons$$ Y, the standard reaction Gibbs energy depends on temperature T (in K) as $$\Delta$$rGo (in kJ mol–1) = 120 - {3 \over 8} T. The major component of the reaction mixture at T is :

Two blocks of the same metal having same mass and at temperature T1 and T2, respectively, are brought in contact with each other and allowed to attain thermal equilibrium at constant pressure. The change in entropy, $$\Delta$$S, for this process is :

For the equilibrium, 2H2O $$\rightleftharpoons$$ H3O+ + OH$$-$$, the value of $$\Delta$$Go at 298 K is approximately :

The reaction, MgO(s) + C(s) $$\to$$ Mg(s) + CO(g), for which $$\Delta$$rHo + 491.1 kJ mol–1 and $$\Delta$$rSo = 198.0 JK–1 mol–1, is not feasible at 298 K. Temperature above which reaciton will be feasible is :

The standard reaction Gibbs energy for a chemical reaction at an absolute temperature T is given by $$\Delta$$rGo = A – BT Where A and B are non-zero constants. Which of the following is TRUE about this reaction?

The aldehydes which will not form Grignard product with one equivalent Grignard reagents are -

The major product of the following reaction is –