Thermodynamics practice · Mixed difficulty

Heat of formation of compound is defined as :

Mathematical from of 1st Law

Which of the following gas will liberate maximum heat on combustion per gram?

In which of the following condition a chemical reaction can not occur?

Amongst the following statement's regarding adsorption, those that are valid are –
(A) Activation energy is high for chemisorption process
(B) Physisorption converts into chemisorption at high temperature
(C) Chemisorption converts into physisorption at low temperature
(D) With increase in temperature, the equilibrium concentration of adsorbate increases

A positive change in enthalpy occurs in :

In which case, a spontaneous reaction is possible at any temperature?

For an ideal gas, the relation between the enthalpy change and internal energy change at constant temperature is given by :

Equal volume of ${C_2}{H_2}$ and ${H_2}$ are combusted under identical condition. The ratio of their heat of combustion is:
${H_2}(g) + \frac{1}{2}{O_2}(g) \to {H_2}O(g);\Delta H = - 241.8\,\,\,kJ$
${C_2}{H_2}(g) + 2\frac{1}{2}{O_2}(g) \to 2C{O_2}(g) + {H_2}O(g);\,\,\Delta H = - 1300\,\,\,kJ$

The change in internal energy, if $60 {~J}$ of heat is given to the system at constant pressure and $30 {~J}$ of work is done by the system, will be:

Equilibrium constant of a reaction is related to:

In the exothermic reaction, the enthalpy of
reaction is always:

For a gas $\left( {R/{C_v}} \right) = 0.67$ the gas is made up of molecules which are:

Calorific value of carbohydrates is approximately:

In an adiabatic process, no transfer of heat takes place between system and surroundings. Choose the corerct option for free expansion of an ideal gas under adiabatic condition from the following.

A gas is allowed to expand in an insulated container against a constant external pressure of 5 atm from an initial volume of 1.75 L to a final volume of 6.75 L. The change in internal energy $(\Delta U)$ of the gas will be

A solution of $500 \mathrm{~ml}$ of $2 \mathrm{~M}-{KOH}$ is added to $500 \mathrm{~ml}$ of $2 \mathrm{~M}-{HCl}$ and the mixture is well shaken. The rise in temperature $T_1$ is noted. The experiment is again performed using $250 \mathrm{~ml}$ of ${KOH}$ solution and $500 \mathrm{~ml}$ of ${HCl}$ solution and rise in temperature $T_2$ is again noted. Which of the following is correct?

Which correctly represents the physical significance of Gibbs energy change?

Statement I Due to atomisation of gaseous molecule,
entropy increases.
Statement II Atoms are more ordered than the molecules.

Work done by a sample of an ideal gas in a process ${A}$ is double the work done in another process ${B}.$ The temperature rises through the same amount in the two processes. If $C_{{A}}$ and $C_{{B}}$ are the molar heat capacities for the two processes, then

In which state matter have highest entropy?

The energy that opposes dissolution of a solvent
is

The heat of combustion of a substance is :

The enthalpy of atomization of $\mathrm{PH}_3(\mathrm{g})$ is $+954 \mathrm{~kJ} /\mathrm{mol}$ and that of $\mathrm{P}_2 \mathrm{H}_4$ is $+1.488 \mathrm{~MJ} / \mathrm{mol}.$ The bond energy of the $\mathrm{P}-\mathrm{P}$ bond is

A person requires 2870 kcal of energy to lead normal daily life. If heat of combustion of cane sugar is -1349 kcal, then his daily consumption of sugar is:

The work done by a system in an expansion against a constant external pressure is:

A thermodynamic state function is:

Heat of formation of ${H_2}O$ is -188 kJ /mol and ${H_2}{O_2}$ is -286 kJ/mol.The enthalpy change for the reaction $2{H_2}{O_2} \to 2{H_2}O + {O_2}$ is

The work done during the expansion of a gas from a volume of $4\,d{m^3}$ to $6\,d{m^3}$ against a constant external pressure of 3 atm is

1 mole of an ideal gas at 25℃ is subjected to expand reversibly ten times of its initial volume. The change in entropy of expansion is: