Thermodynamics practice · Mixed difficulty

$2 {MnO}_4^{-}+16 {H}^{+}+10 {Cl}^{-} \rightarrow 2 {Mn}^{2+}+5 {Cl}_2(\mathrm{g})+8 {H}_2 {O}$

The above reaction is endothermic and hence, the actual temperature of the reaction vessel (isolated from the surrounding) may be different from that expected. Given that the initial temperature of the reaction vessel was used in the calculations, how would this affect the predicted value of moles of ${Cl}_2(n)$ according to the equation $n=P V/ R T?$

Which represents the largest amount of energy?

During an isothermal expansion of an ideal gas its:

Internal energy and pressure of a gas of unit volume are related as:

Which among the following is an extensive property?

Thermochemistry is the study of relationship between heat energy and :

The equilibrium constant $(K)$ of a reaction may be written as,

Which of the following are path functions ?
a) Heat capacity b) work c) Entropy

Consider the following reactions :

$\mathrm{C}(s)+\mathrm{O}_2(\mathrm{~g}) \longrightarrow \mathrm{CO}_2(\mathrm{~g})+x \mathrm{~kJ}$

$\mathrm{CO}(g)+\frac{1}{2} \mathrm{O}_2(g) \longrightarrow \mathrm{CO}_2(g)+y \mathrm{~kJ}$

The heat of formation of $\mathrm{CO}(g)$ is :

Entropy of an adiabatic reversible process is:-

Two moles of helium gas expanded isothermally and irreversible at 27℃ from volume 1 $d{m^3}$ to 1 ${m^3}$ at constant pressure of 100 k Pa. Calculate the work done.

For the reaction $aA\left( s \right) + bB\left( g \right)\xrightarrow{\,}dD\left( s \right) + cC\left( g \right),$ then

When hydrogen and oxygen burn to form water in an oxyhydrogen torch, the entropy change is:

Which of the following relation is correct
regarding reversible adiabatic process?

Which of the following represents the first law
of thermodynamics

Entropy of a perfectly crystalline solid at 0 K is

For a reaction, $A\left( l \right) \to 4B\left( g \right)$ if $\Delta U = 4.5\,kJ$ and $\Delta S = 60\,J{K^{ - 1}}$ at ${27^0}C$ then $\Delta G$ will be

Predict the change in internal energy for an isolated system at constant volume

A well stoppered thermos flask containing some ice cubes is an example of:

For the process, $\mathrm{C}{\mathrm{O}_2}\left( \mathrm{s} \right) \to \mathrm{C}{\mathrm{O}_2}\left( \mathrm{g} \right):$

For a process, entropy change of a system is
expressed a

In isolated system:

An ideal gas absorb $50\, \mathrm{cal}$ heat and expand in the vaccum from $5 \mathrm{~L}$ to $15 \mathrm{~L}$. Change in its internal energy is :-

The bond dissociation energies of $N \equiv N, N=N, O=O \,\&\, N=O$ are $946,418,498$ and $607 \mathrm{~KJ/ mole}$ respectively. If heat of formation of ${N}_2 {O}$ is $82 \mathrm{~KJ/ mole}$ then the magnitude of resonance energy of ${N}_2 {O}$ in $\mathrm{KJ} / \mathrm{mole}$ is ___

Consider an endothermic reaction $X \to Y$ with the activation energies, respectively in general

The heats of neutralization of $C{H_3}COOH,\,\,\,HCOOH,\,\,HCN$ and ${H_2}S$ are $- 13.2,\, - \,13.4,\, - 2.9$ and - 3.8 kcal per equivalent respectively. Arrange the increasing order of strength.

At $25^{\circ} \mathrm{C}$, the enthalpy of the following processes are given

$\mathrm{H}_{2}(\mathrm{g})+\mathrm{O}_{2}(\mathrm{g}) \rightarrow 2 \mathrm{OH}(\mathrm{g}) \Delta \mathrm{H}^{\circ} =78 \,\mathrm{kJ} \,\mathrm{mol}^{-1}$

$\mathrm{H}_{2}(\mathrm{g})+\frac{1}{2} \mathrm{O}_{2}(\mathrm{g}) \rightarrow \mathrm{H}_{2} \mathrm{O}(\mathrm{g}) \Delta \mathrm{H}^{\circ} =-242 \,\mathrm{kJ} \,\mathrm{mol}^{-1}$

$\mathrm{H}_{2}(\mathrm{g}) \rightarrow 2 \mathrm{H}(\mathrm{g}) \Delta \mathrm{H}^{\circ}=436 \,\mathrm{kJ} \,\mathrm{mol}^{-1}$

$\frac{1}{2} \mathrm{O}_{2}(\mathrm{g}) \rightarrow \mathrm{O}(\mathrm{g}) \Delta \mathrm{H}^{\circ}=249 \,\mathrm{kJ} \,\mathrm{mol}^{-1}$
What would be the value of $X$ for the following reaction? _____ (Nearest integer)
$\mathrm{H}_{2} \mathrm{O}(\mathrm{g}) \rightarrow \mathrm{H}(\mathrm{g})+\mathrm{OH}(\mathrm{g}) \Delta \mathrm{H}^{\circ}=\mathrm{X} \,\mathrm{kJ} \,\mathrm{mol}^{-1}$

A closed flask contains water in all its three states, solids, liquid and vapour at 0℃. In this situation the average KE of the water molecule will be:

For the reactions: $\mathrm{C} + {\mathrm{O}_2} \to \mathrm{C}{\mathrm{O}_2};\Delta H = - 393\mathrm{kJ}$ $2\mathrm{Zn} + {\mathrm{O}_2} \to 2\mathrm{ZnO};\Delta H = - 412\mathrm{kJ}$ which one is correct?

An ideal gas undergoes isothermal expansion from $(10 \mathrm{~atm}, 1 \mathrm{~L})$ to $(1 \mathrm{~atm}, 10 \mathrm{~L})$ either by path-I (infinite stage expansion) or by path-II (first against $5 \mathrm{~atm}$ and then against $1 \mathrm{~atm}).$ The value of $\left(\frac{q_{\text {path-I}}}{q_{\text {path-II}}}\right)$ is