Thermodynamics practice · Mixed difficulty

The heats of neutralization of four acids A,B,C and D are – 13.7, –9.4, –11.2 and –12.4 kcal respectively when they are neutralized by a common base. The acidic character obeys the order :

In which case will the efficiency of a Carnot cycle be higher, when the hot body temperature is increased by $\Delta T$ or when the cold body temperature is decreased by the same magnitude?

A sample of argon gas at $1 \mathrm{~atm}$ pressure and $27^{\circ} \mathrm{C}$ expands reversibly and adiabatically from $1.25 \mathrm{~dm}^3$ to $2.50 \mathrm{~dm}^3.$ Calculate the enthalpy change in this process. $\mathrm{C}_{\mathrm{v}, \mathrm{m}}$ for argon is $12.48 \mathrm{~JK}^{-1} \mathrm{~mol}^{-1}$

Identify the correct statement regarding entropy

STATEMENT-1 : The magnitude of the work involved in an isothermal expansion is greater than that involved in an adiabatic expansion.

STATEMENT2 : $P-V$ curve ( $P$ on $y$-axis and $V$ on $x$-axis) decrease more rapidly for reversible adiabatic exparision compared to reversible isothermal expansion starting from same initial state.

Which one of the following is an exothermic reaction?

Which are correct to express work terms?

For which one of the following system $\Delta H > \Delta E$

What is entropy change in $2 {~mol} {~N}_2$, when its temperature is taken from $400 {~K}$ to $800 {~K}$, adiabatically.

Which among the following is not a state function?

A mixture of hydrogen and chlorine on exposure to ultra violet sunlight reacts with explosion. The step involved in the initiation of the reaction is :

An adiabatic process occurs in

Following reaction occurs in an automobile $2{C_8}{H_{18}}(g) + 25\,{O_2}(g) \to 16\,C{O_2}(g) + 18{H_2}O(g)$ The sign of $\Delta H,\,\Delta S\mathrm{ }\,\mathrm{and}\,\,\mathrm{ }\Delta G$ would be

Statement I : When enthalpy factor is absent then randomness factor decides spontaneity of a process
Statement II : When randomness factor is absent then enthalpy factor decides spontaneity of aprocess

Given the bond energies of N ≡ N, H─H and N─H bonds as 945, 436 and 391 $kJ\,\,mo{l^{ - 1}}$respectively, the enthalpy of the reaction, $2{\mathrm{N}_2}\left( \mathrm{g} \right) + 3{\mathrm{H}_2}\left( \mathrm{g} \right) \to 2\mathrm{N}{\mathrm{H}_3}\left( \mathrm{g} \right)$ is :

Combustion of glucose takes place according to the equation ${\mathrm{C}_6}{\mathrm{H}_{12}}{\mathrm{O}_6} + \mathrm{C}{\mathrm{O}_2} \to 6\mathrm{C}{\mathrm{O}_2} + 6{\mathrm{H}_2}\mathrm{O};\Delta H = - 72\;kcal$ How much energy will be required for the production of 1.6 g of glucose (Molecular mass of glucose = 180)?

Consider following statements:
(a) The absolute value of internal energy cannot be
evaluated.
(b) Entropy is a state function and extensive
property
(c) Temperature is an extensive property
(d) The standard enthalpy of formation of an element $\left(\Delta \mathrm{H}_{\mathrm{f}}\right)$ is always considered to be zero

(e) For an adiabatic process $\Delta S>0$
wrong statements are :

When the change of entropy is greater, then the ability for work is:

1 mole of an ideal gas is allowed to expand isothermally and reversibly at $27^{\circ} \mathrm{C}$ until its volume is tripled. Calculate $\Delta \mathrm{S}_{\mathrm{sys}}$ (Give answer approximately).

Consider the following cases of standard enthalpy of reaction $\left(\Delta \mathrm{H}_{\mathrm{r}}^{\circ}\right.$ in $\left.\mathrm{kJ} \mathrm{~mol}^{-1}\right)$

$\begin{aligned} & \mathrm{C}_2 \mathrm{H}_6(\mathrm{g})+\frac{7}{2} \mathrm{O}_2(\mathrm{g}) \rightarrow 2 \mathrm{CO}_2(\mathrm{g})+3 \mathrm{H}_2 \mathrm{O}(\ell) ;\Delta \mathrm{H}_1^{\circ}=-1550 \\ & \mathrm{C}(\text {graphite})+\mathrm{O}_2(\mathrm{g}) \rightarrow \mathrm{CO}_2(\mathrm{g}) ;\Delta \mathrm{H}_2^{\circ}=-393.5 \\ & \mathrm{H}_2(\mathrm{g})+\frac{1}{2} \mathrm{O}_2(\mathrm{g}) \rightarrow \mathrm{H}_2 \mathrm{O}(\ell) ;\Delta \mathrm{H}_3^{\circ}=-286 \end{aligned}$

The magnitude of $\Delta \mathrm{H}_{\text{f }\mathrm{C}_2 \mathrm{H}_6(\mathrm{g})}^{\circ}$ is ____ $\mathrm{kJ} \mathrm{~mol}^{-1}$ (Nearest integer).

The standard enthalpies of formation of $C{O_2}\left( g \right),\,\,{H_2}O\left( l \right)$ and glucose (s) at ${25^\mathrm{o}}\,\,C$ are $- 400\,\,KJ \cdot mo{l^{ - 1}},\,\, - 300\,\,KJ \cdot mo{l^{ - 1}}$ and $- 1300\,\,KJ/mol$ respectively. The standard enthalpy of combustion per gram of glucose at ${25^\mathrm{o}}\,\,C$ is

When a gas undergoes adiabatic expansion, it gets cooled due to

The enthalpies of all the elements in their standard states are

The change in the enthalpy during the reaction,$\;\mathrm{NaOH} + \mathrm{HCl} \to \;\mathrm{NaCl} + {\mathrm{H}_2}\mathrm{O},$ is called :

∆S is positive for the change:

It is impossible to attain the lowest temperature known as zero degree absolute. This is a simple statement of:

Given that,
$3\mathrm{C}\left( s \right) + 2\mathrm{F}{\mathrm{e}_2}{\mathrm{O}_3}\left( s \right) \to 4\mathrm{Fe}\left( s \right) + 3\mathrm{C}{\mathrm{O}_2}\left( \mathrm{g} \right)\Delta {H^o} = - 93657\,\,cal$
$\mathrm{C}\left( s \right) + {\mathrm{O}_2}\left( \mathrm{g} \right) \to \mathrm{C}{\mathrm{O}_2}\left( \mathrm{g} \right);\Delta {H^o} = - 94050$ cal
If both the values of ∆H are at $25\,^\circ C$ then calculate $?H_{\mathrm{F}{\mathrm{e}_2}{\mathrm{O}_3}}^\mathrm{o}$

Heat of reaction at constant $p$ or constant $V$ varies with temperature as given by Kirchoff's equation is/are

We believe in the laws of thermodynamics because they are

The state of a gas can be described by quoting the relationship between