Thermodynamics practice · Mixed difficulty

The enthalpy of vaporisation of a substance is 840 J/mol and its boiling point is -173℃. Its entropy of vaporisation is

What are the units of entropy?

Which of the following statements is incorrect?

The temperature of the system increases during an:

When 1 mole of $\mathrm{Na}(\mathrm{s})$ is dissolved in large volume of water at $298 \mathrm{~K}$ and $1 \mathrm{~bar}, 184 \mathrm{~kJ} / \mathrm{mol}$ heat is released. When 1 mole of $\mathrm{Na}_2 \mathrm{O}(\mathrm{s})$ is dissolved in large volume of water at $298 \mathrm{~K}$ and $1 \mathrm{~bar}, 238 \mathrm{~kJ} / \mathrm{mol}$ is released. If the enthalpy of formation of water is $-286 \mathrm{~kJ} / \mathrm{mol},$ then the enthalpy of formation of sodium oxide is

One mole of a perfect gas expands isothermally and reversibly from $10 \mathrm{~dm}^3$ to $20 \mathrm{~dm}^3$ at $300 \mathrm{~K}$. $\Delta u, q$ and work done in the process are $\left[\mathrm{R}={8 . 3} \times {1 0}^{-{3}}\,\mathrm\,\,{kJ} \mathrm{K}^{-1} \mathrm{~mol}^{-{1}}\right]$

The heat of formation $({∆H_f})of{H_2}O(l)$is equal to:

Second law of thermodynamics defines

Enthalpy of neutralization of the reaction between $\mathrm{CH}_3 \mathrm{COOH} \text{(aq)}$ and $\mathrm{NaOH} \text{(aq)}$ is $-13.2 \mathrm{~kcal/eq}$ and that of the reaction between $\mathrm{H}_2 \mathrm{SO}_4(\mathrm{aq})$ and $\mathrm{KOH}(\mathrm{aq})$ is $-13.7 \mathrm{~kcal} / \mathrm{eq}.$ The enthalpy of dissociation of $\mathrm{CH}_3 \mathrm{COOH}(\mathrm{aq})$ is

The H─H bond energy is 430 kJ $mo{l^{ - 1}}$ and Cl─Cl bond energy is 240 kJ $mo{l^{ - 1}}$ . ∆H for HCl is -90 kJ. The H─Cl bond energy is about:

The term $-T \Delta S_{\text {total}}$ at constant temperature and pressure is known as

For the process to occur under adiabatic conditions, the correct condition is

Four monobasic acids A,B,C and D have their respective ${\Delta _{neut}}{H^0}$ values are -11.5 , -7.5, -12.4 and -8.9 kcal/mol. Which of the following acids has the highest pKa value ?

16 g oxygen gas expands at STP to occupy double of its original volume. The work done during the process is:

For strong acid strong base neutralisation energy for 1 mole ${H}_2 {O}$ formation is $-57.1 \mathrm{~kJ}$. If $0.25$ mole of strong monoprotic acid is reacted with $0.5$ mole of strong base then enthalpy of neutralisation is

Which is not characteristic of thermochemical equation?

A cylinder of gas is assumed to contain 11.2 kg of butane $\mathrm{(}{\mathrm{C}_4}{\mathrm{H}_{10}})$. If a normal family needs 20000 kJ of energy per day. The cylinder will last (Given that ∆H for combustion of butane is -2658 kJ)

If a chemical change is brought about by one or more methods in one or more steps, then the amount of heat absorbed or evolved during the complete course of reaction is same, whichever method was followed. This law is known as :

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 standard reaction Gibbs energy for a chemical reaction at an absolute temperature $T$ is given by, ${\Delta _r}{G^ \circ } = A - BT$ Where $A$ and $B$ are non-zero constants. Which of the following is true about this reaction?

$\Delta G$ for a spontaneous reaction is

One mole of an ideal gas undergoes a reversible process in which the entropy of the gas changes with absolute temperature $T$ as $S=a T+C_{\mathrm{v}, \mathrm{m}}$ $\ln T,$ where $a$ is a positive constant. If $T=T_0$ at $V=V_0,$ then the volume dependence of the gas on temperature in this process is

Under the same conditions how many mL of 1M KOH and 0.5 M ${\mathrm{H}_2}\mathrm{S}{\mathrm{O}_4}$ solutions, respectively when mixed for a total volume of 100 mL produce the highest rise in temperature?

The enthalpy change is negative for :

An ideal gas with the adiabatic exponent $\gamma$ goes through a process $P=P_{0}-\alpha V,$ where $P_{0}$ and $\alpha$ are positive constants and $V$ is the volume. At what volume will the gas entropy have the maximum value?

Unit of entropy is

Under isothermal condition for one mole of ideal gas what is the ratio of work done under reversible to irreversible process, initially held at $20 {~atm}$ undergoes expansion from $1 {~L}$ to $2 {~L}$, at $298 {~K}$, under external pressure of $10 {~atm}$ ?

The first law of thermodynamic is expressed as

A system absorbs 600 J of heat and work equivalent to 300 J on its surroundings. The change in internal energy is

$\Delta \mathrm{G}$ is equal to