Choose the correct answer. A thermodynamic state function is a quantity (I) used to determine heatchanges (II) whose value is independent ofpath (III) used to determine pressure volumework (IV) whose value depends on temperature only.

For the process to occur under adiabatic conditions, the correct condition is: (I) ?T =0 (II) ?p =0 (III) q =0 (IV) w = 0

The enthalpies of all elements in their standard states are: (I) unity (II) zero (III) <0 (IV) different for each element

?U^?of combustion of methane is – X kJ mol^–1. The value of ?H^? is (i) = ?U^? (I) >?U^? (II) ?(iv) = 0

The enthalpy of combustion of methane, graphite and dihydrogen at 298 K are, –890.3 kJ mol^–1 –393.5 kJ mol^–1, and –285.8 kJ mol^–1 respectively. Enthalpy of formation of CH_4(g) willbe (i) –74.8kJmol^–1(ii) –52.27 kJ mol^–1(iii) +74.8 kJ mol–1 (iv) +52.26 kJ mol–1.

A reaction, A + B ? C + D + q is found to have a positive entropy change. The reaction will be (I) possible at hightemperature (II) possible only at lowtemperature (III) not possible at anytemperature (IV) possible at any temperature

In a process, 701 J of heat is absorbed by a system and 394 J of work is done by the system. What is the change in internal energy for the process?

The reaction of cyanamide, NH₂CN_(s), with dioxygen was carried out in a bomb calorimeter, and ?U was found to be –742.7 kJ mol^–1 at 298 K. Calculate enthalpy change for the reaction at 298K.

Calculate the number of kJ of heat necessary to raise the temperature of 60.0 g of aluminium from 35°C to 55°C. Molar heat capacity of Al is 24 J mol^–1 K^–1.

Calculate the enthalpy change on freezing of 1.0 mol of water at 10.0°C to ice at – 10.0°C. ?_fusH = 6.03 kJ mol^–1 at 0°C. C_p[H₂O(l)] = 75.3 J mol^–1 K^–1 C_p[H₂O(s)] = 36.8 J mol^–1 K^–1

Enthalpy of combustion of carbon to CO₂ is –393.5 kJ mol^–1. Calculate the heat released upon formation of 35.2 g of CO₂ from carbon and dioxygen gas.

Enthalpies of formation of CO_(g), CO_2(g), N₂O_(g) and N₂O_4(g) are –110 kJ mol^–1, – 393 kJ mol^–1, 81 kJ mol^–1 and 9.7 kJ mol^–1 respectively. Find the value of ?_rH for the reaction: N2O4(g)+3CO(g)N2O(g) +3CO2(g)

Given ; ?rH? = –92.4 kJ mol–1 What is the standard enthalpy of formation of NH3 gas?

Calculate the standard enthalpy of formation of CH₃OH_(l) from the following data: CH₃OH_(l)+O_2(g)CO_2(g) + 2H₂O_(l) ; ?_rH^? = –726 kJ mol^–1 C_(g)+ O_2(g)CO_2(g) ; ?_cH^? = –393 kJmol^–1 H_2(g) +O_2(g)H₂O_(l) ; ?_fH^? = –286 kJ mol^–1.

Calculate the enthalpy change for the process CCl4(g) ? C(g) + 4Cl(g) and calculate bond enthalpy of C–Cl in CCl_4(g). ?_vapH^? (CCl₄) = 30.5 kJ mol^–1. ?_fH^? (CCl₄) = –135.5 kJ mol^–1. ?_aH^? (C) = 715.0 kJ mol^–1, where ?_aH^? is enthalpy of atomisation?aH? (Cl2) = 242 kJ mol–1

For an isolated system, ?U = 0, what will be ?S?

For the reaction at 298 K, 2A + B ? C ?H = 400 kJ mol^–1 and ?S = 0.2 kJ K^–1 mol^–1 At what temperature will the reaction become spontaneous considering ?H and ?S to be constant over the temperature range?

For thereaction,2Cl(g) ? Cl2(g), what are the signs of ?H and ?S ?

For the reaction 2A(g) + B(g) ? 2D(g) ?U^? = –10.5 kJ and ?S^?= –44.1 JK^–1. Calculate?G^?forthereaction,andpredictwhetherthereactionmayoccur spontaneously.

The equilibrium constant for a reaction is 10. What will be the value of ?G^?? R = 8.314 JK^–1 mol^–1, T = 300 K.

Comment on the thermodynamic stability ofNO_(g),givenN_2(g) + O_2(g)? NO_(g) ; ?_rH^? = 90 kJ mol^–1 NO(g) + O2(g) ? NO2(g) : ?rH?= –74 kJ mol–1

Calculate the entropy change in surroundings when 1.00 mol of H₂O_(l) is formed under standard conditions. ?_fH^? = –286 kJ mol^–1.