Thermodynamics ...

According to Hess’s Law, if a reaction takes place in several steps then its standard reaction enthalpy is

Spontaneity in the context of chemical thermodynamics means

For an adiabatic change

According to the diagram given below, the value of H for conversion of A to B is

Enthalpy of solution of a substance is the enthalpy change

Directions: The following question has four choices out of which ONLY ONE is correct.

Dissolution of ammonium chloride in water is an endothermic change. At constant temperature, it is accompanied by

Directions: The following question has four choices out of which ONLY ONE is correct.

What is the entropy change (in JK^-1 mol^-1) when one mole of ice is converted into water at 0⁰C? (The enthalpy change for the conversion of ice to liquid water is 6.0 kJ mol^-1 at 0⁰C.)

Enthalpy of atomization is enthalpy change on breaking

If the enthalpy of oxidation of methanol to formaldehyde and water is -163 kJ, then what is the enthalpy of the formation of CH₃OH? (Given: Enthalpy of formation of HCHO (l) is -116 kJ and enthalpy of formation of H₂O (l) is -286 kJ.)

Consider the reaction: 2C + O₂  2CO₂, H = - 395.5 kJ/mol. Which of the following statements is/are correct for this reaction?

The enthalpy and entropy changes for the reaction Br₂(I) + CI₂(g) 2 BrCI(g) are 30 kJ mol^–1 and 105 JK^–1 mol^–1, respectively.

The temperature at which the reaction will be in equilibrium is

In a reversible process, S_sys + S_surr is 

Standard enthalpy and standard entropy changes for the oxidation of ammonia at 298 K are - 382.64 kJ mol^-1 and - 145.6 J K^-1 mol^-1, respectively. Standard Gibbs energy change for the same reaction at 298 K is

Directions: The following question has four choices out of which ONLY ONE is correct.

The heat of neutralisation of acetic acid by sodium hydroxide is −50.6 kJ/mol, and the heat of neutralisation of a strong acid by a strong base is −55.9 kJ/mol. What is the value of H for the ionisation of CH₃COOH?

Which of the following reactions corresponds to the definition of enthalpy of formation?

When a solid changes into liquid, the entropy

For the reaction 2H₂ + O₂ 2H₂O, H = -571 kJ, bond energy of H - H = 435 kJ/mol and that of O - O = 498 kJ/mol. Calculate the average bond energy (in kJ/mol) of O - H bond using this data.

The unit of entropy is

Which one of the following relations is incorrect?

Identify the correct statement for change of Gibbs energy for a system (G_system) at constant temperature and pressure.

The lattice enthalpy of an ionic compound is the enthalpy change which occurs when 

A thermodynamic state function is a physical quantity whose value 

The amount of heat liberated when 1 mole of a substance is completely burnt in the presence of oxygen is known as

Entropy is a state function and measures

Bond energy of hydrogen gas is - 433 kJ. What is the bond dissociation energy of 0.5 mole of hydrogen gas?

Hess's Law deals with

If change in Gibbs energy ΔG is negative (< 0) at constant pressure and temperature

If C₆H₆(I) + 15/2 O₂(g)  3H₂O(I) + 6CO_2^(g); = – 3264.6 kJ mol^–1, then the energy obtained by burning 3.9 g of benzene in air is 

For the process, dry ice (g), which of the following is true?

By convention, standard enthalpy for formation of an element in reference state is: