Thermodynamics practice · Medium

On increasing temperature, the equilibrium constant of exothermic and endothermic reactions repectively

1 Mole of ideal gas expanded reversibly and isothermally from 1 lit to 10 lit.
then find out the entropy change in cal/Kelvin.

For a certain reaction the change in enthalpy and change in entropy are $40.63 \mathrm{~kJ} \mathrm{~mol}^{-1}$ and $100 \mathrm{~JK}^{-1}$ respectively. What is the value of $\Delta G$ at $27^{\circ} \mathrm{C}?$

Which statement(s) is/are correct?

Standard molar enthalpy of formation at $298 \mathrm{~K}$ is zero for

Given,

$\begin{aligned} & 2 {Fe}_2 {O}_{3(s)} \longrightarrow 4 {Fe}_{(s)}+3 {O}_{2(g)} ; \\ & \Delta_r G_1^{\circ}=+1487 {~kJ} {~mol}^{-1} \\ & 6 {CO}_{(g)}+3 {O}_{2(g)} \longrightarrow {CO}_{2(g)} ; \\ & \Delta_r G_2^{\circ}=-1543.2 {~kJ} {~mol}^{-1} \end{aligned}$

Select the correct statement :

$1 \mathrm{~g}$ ice absorbs $335 \mathrm{~J}$ of heat to melt at $0^{\circ} \mathrm{C}$. The entropy change will be

Statement I: Heat evolved in the neutralization of either 1 mole of ${HCl}$ or 1 mole of ${H}_2 {SO}_4$ with ${NaOH}$ is same.

Statement II: Both ${HCl}$ and ${H}_2 {SO}_4$ are strong acids.

Among the following the set of parameters that represents path functions, is
(A) $q + W\,\,\,\,\,\,\,\,\,\,$ (B) $q\,\,\,\,\,\,\,\,\,\,$ (C) $W\,\,\,\,\,\,\,\,\,\,$ (D) $H - TS$

Identify the correct statement regarding entropy

The heat of combustion of ${CH}_{4({g})}, {C}_{(\mathrm{graphite})}$ and ${H}_{2({g})}$ are $20 \, \mathrm{kcal},-40 \, \mathrm{kcal}$ and $-10 \, \mathrm{kcal}$ respectively. The heat of formation of methane is

The entropy change for vaporisation of liquid water to steam at 100℃ is…$\mathrm{J}{\mathrm{K}^{ - 1}}\mathrm{mo}{\mathrm{l}^{ - 1}}$Given that heat of vaporisation is $40.8kJmo{l^{ - 1}}.$

Specific heat is defined as:

The enthalpy of a monoatomic gas at $T$ Kelvin is:

At $25^{\circ} \mathrm{C}$ 1 mole of butane upon heating forms $\mathrm{CO}_2$ and $\mathrm{H}_2 \mathrm{O}$. The work done is

The enthalpy of neutralisation of $NH_4 OH$ and $CH_3 COOH$ is $-10.5 \mathrm{k\,cal\,} \mathrm{mol}^{-1}$ and enthalpy of neutralisation of $CH_3COOH$ with strong base is $-12.5 \mathrm{k\,cal\,} \mathrm{mol}^{-1}$. The enthalpy of ionisation of $NH_4OH$ will be

Given that $\mathrm{N}_2(\mathrm{~g})+3 \mathrm{H}_2(\mathrm{~g}) \rightarrow 2 \mathrm{NH}_3(\mathrm{~g})$;
$\Delta_{\mathrm{r}} \mathrm{H}^{\circ}=-92 \mathrm{~kJ}$, the standard molar enthalpy of formation in $\mathrm{kJ} \mathrm{mol}^{-1}$ of $\mathrm{NH}_3(\mathrm{~g})$ is

Butane exists in various conformations in nature. At any given instant, the probability that a given butane molecule is in anti, gauche, eclipsed and fully eclipsed conformation is $0.7,0.2,0.06$ and $0.04 ,$ respectively. If the molar enthalpy of combustion of natural butane is $-690 \mathrm{~kcal} / \mathrm{mol}$ at $25^{\circ} \mathrm{C},$ then calculate the enthalpy of combustion of butane if all the butane molecules are in gauche conformation. The potential energy of gauche form is $2 \mathrm{~kcal} / \mathrm{mol}$ higher than anti form but it is $3 \mathrm{~kcal} / \mathrm{mol}$ less than eclipsed form and $5.5 \mathrm{~kcal} / \mathrm{mol}$ less than fully eclipsed form.

According to the first law of thermodynamics which of the following quantities represents change in a state function?

1 mol of an ideal gas expanded reversibly from 10 L to 100 L at $27^{\circ} \mathrm{C}.$ Work done involved in the process is

A process in which no heat change takes place is called.

The enthalpy changes for the following processes are listed below :

$\begin{array}{ll}\mathrm{Cl}_2(g) \rightarrow 2 \mathrm{Cl}(g), & 242.3 \mathrm{~kJ} \mathrm{~mol}^{-1} \\ \mathrm{I}_2(g) \rightarrow 2 \mathrm{I}(g), & 151.0 \mathrm{~kJ} \mathrm{~mol}^{-1} \\ \mathrm{ICl}(g) \rightarrow \mathrm{I}(g)+\mathrm{Cl}(g), & 211.3 \mathrm{~kJ} \mathrm{~mol}^{-1} \\ \mathrm{I}_2(s) \rightarrow \mathrm{I}_2(g), & 62.76 \mathrm{~kJ} \mathrm{~mol}^{-1}\end{array}$

Given that the standard states for iodine and chlorine are $\mathrm{I}_2(s)$ and $\mathrm{Cl}_2(g)$, the standard enthalpy of formation for $\operatorname{ICl}(g)$ is :

The heat of formations of $\mathrm{CO(g})$ and $\mathrm{CO_2(g})$ are $-26.4 \mathrm{~K} \mathrm{~cal}$ and $-94.0 \mathrm{~kcal}$ respectively. The heat of combustion of carbon monoxide will be

Consider a reversible isontropic expansion of 1.0 mole of an ideal monoatomic gas from $25^{\circ} \mathrm{C}$ to $75^{\circ} \mathrm{C}$. If the initial pressure was $1.0 \mathrm{~bar}$, final pressure is

If the bond energies of $\mathrm{H}_2, \mathrm{Br}_2$ and $\mathrm{H}-\mathrm{Br}$ are 433,192 and $364 \mathrm{~kJ} /$ mol respectively the $\Delta \mathrm{H}^{\circ}$ for the reaction $\mathrm{H}_2(\mathrm{g})+\mathrm{Br}_2(\mathrm{g}) \longrightarrow 2 \mathrm{HBr}(\mathrm{g})$ is:

Which of the following on combustion gives
maximum energy?

A process which is unfavourable with respect to enthalpy,
but favourable with respect to entropy

Heat absorbed at constant volume is measured in a calorimeter in which steel vessel is immersed to ensure that

Assertion (A): The dissolution of $\mathrm{NH}_4 \mathrm{Cl}$ in water is endothermic but it dissolves in water.
Reason (R): On dissolution of $\mathrm{NH}_4 \mathrm{Cl}$, entropy increases.

The molar heat capacity, $\mathrm{C}_{\mathrm{v}}$ of an ideal gas whose energy is that of translational motion only is