Thermodynamics practice · Mixed difficulty

Which is not a spontaneous process?

For the precipitation of AgCl by $\mathrm{A}{\mathrm{g}^ + }$ ions and HCl:

When $110 \mathrm{~g}$ of manganese (At. mass $=55$ ) dissolves in dilute $\mathrm{HNO}_3$ at $27^{\circ} \mathrm{C}$ under atmospheric pressure, the work done in the process is :

Calorie is equivalent to:

The value of $\Delta E$ for an open and isolated system respectively is

Consider the following reactions:
$\mathrm{(i)}\,\,\,{H^ + }(aq) + O{H^ - }(aq) \to {H_2}O(l),\,\,\Delta H = - {X_1}\,\,\mathrm{kJ}\,\,\mathrm{mo}{\mathrm{l}^{ - 1}}$
$\mathrm{(ii)}\,\,\,{H_2}(g) + \frac{1}{2}{O_2}(g) \to {H_2}O(l),\,\,\Delta H = - {X_2}\,\,\mathrm{kJ}\,\,\mathrm{mo}{\mathrm{l}^{ - 1}}$
$\mathrm{(iii)}\,\,\,C{O_2}(g) + {H_2}(g) \to CO(g) + {H_2}O,\,\,\Delta H = - {X_3}\,\,\mathrm{kJ}\,\,\mathrm{mo}{\mathrm{l}^{ - 1}}$
$\mathrm{(iv)}\,\,\,{C_2}{H_2}(g) + \frac{5}{2}{O_2}(g) \to 2C{O_2}(g) + {H_2}O(l),\,\,\Delta H = +4 {X_4}\,\,\mathrm{kJ}\,\,\mathrm{mo}{\mathrm{l}^{ - 1}}$
Enthalpy of formation of ${H_2}{O_{(l)}}$ is

If ${\mathrm{H}^ + } + \mathrm{O}{\mathrm{H}^ - } \to {\mathrm{H}_2}\mathrm{O} + 13.7$ kcal then the heat of neutralization for complete neutralization of one mole of ${\mathrm{H}_2}\mathrm{S}{\mathrm{O}_4}$ by a base will be :

Heat of neutralisation of which acid-base reaction is - 57.32 kJ for?

The correct relation between electron gain enthalpy and electron affinity is

Given that
$\mathrm{C}+\mathrm{O}_2 \rightarrow \mathrm{CO}_2: \Delta \mathrm{H}^{\circ}=-\mathrm{x} \mathrm{kJ}$

$2 \mathrm{CO}+\mathrm{O}_2 \rightarrow 2 \mathrm{CO}_2: \Delta \mathrm{H}^{\circ}=-\mathrm{y} \mathrm{kJ}$

the enthalpy of formation of carbon monoxide will be

All the naturally occurring processes, i.e., spontaneous proceed spontaneously in a direction which leads to:

Absorption of gasses on solid surface is generally exothermic because

The work done during the process when 1 mole of gas is allowed to expand freely into vacuum is:

Which one among the following is the correct expression for isothermal reversible change?

$\Delta {S^ \circ }$ will be highest for the reaction:

Entropy change of fusion at constant pressure is given by:

The enthalpy change accompanying a reaction
is called

The enthalpy and entropy change for the reaction,$\mathrm{B}{\mathrm{r}_2}\left( l \right) + \mathrm{C}{\mathrm{l}_2}\left( \mathrm{g} \right) \to 2\mathrm{BrCl}\left( \mathrm{g} \right)$Are 30 kJ$\mathrm{mo}{\mathrm{l}^{ - 1}}$and$105\mathrm{J}{\mathrm{K}^{ - 1}}\mathrm{mo}{\mathrm{l}^{ - 1}}$respectively. The temperature at which the reaction will be in equilibrium is:

An ideal gas undergoes isothermal compression from $5\,{m^3}$ to $1\,{m^3}$ against a constant external pressure of $4\,N{m^{ - 2}}$. Heat released in this process is used to increase the temperature of 1 mole of $Al$. If molar heat capacity of $Al$ is $24\,J\,mo{l^{ - 1}}\,{K^{ - 1}}$, the temperature of $Al$ increases by

The value of $\Delta S$ for freezing of 10g of ${H_2}O\left( \ell \right)$ (enthalpy of fusion is 80 cal/g) at $0^\circ C$ and 1 atm pressure is:

To raise the temperature of 1 mole gas from $400 \mathrm{~K}$ to $500 \mathrm{~K}$, how much heat is require while $C_p=3+1.2 \times 10^{-3} \mathrm{~T} \mathrm{~cal} / \mathrm{mol}$

At constant pressure and temperature, the direction of any chemical reaction is one where, the … decrease.

$x$ g sample of $\mathrm{NH}_4 \mathrm{NO}_3$ is decomposed in a Bomb calorimeter. The temperature of calorimeter increase by $4^{\circ} \mathrm{C}$. The heat capacity of the system is $125 \mathrm{~kJ} /{ }^{\circ} \mathrm{C}$. The value of $x$ is
(Given molar heat of decomposition of $\mathrm{NH}_4 \mathrm{NO}_3$ at constant volume is $400 \mathrm{~kJ} \mathrm{~mol}^{-1}$ )

Heat of formation of $CO$ and $C{O_2}$ are -26.4, -94.0 Kcal/mole respectively. What is the heat of combustion of CO in K cals?

The heat of neutralisation of a strong acid and a strong alkali is 57.0 kJ $\mathrm{mo}{\mathrm{l}^{ - 1}}$. The heat released when 0.5 mole of $\mathrm{HN}{\mathrm{O}_3}$ solution is mixed with 0.2 mole of KOH is

The work done in ergs for the reversible expansion of one mole of an ideal gas from a volume of 10 litres to 20 litres at $25^{\circ} \mathrm{C}$ is

Standard state Gibbs free energy changes for the isomerization reaction,cis-2-pentene⇌trans-2-pentene is -3.67 kJ/mol at 400K. If more trans-2-pentene is added to the reaction vessel, then:

What is the melting point of benzene if $\Delta H_{\text {fusion }}=9.95 \mathrm{~kJ} / \mathrm{mol}$ and $\Delta S_{\text {fusion }}=35.7 \mathrm{~J} / \mathrm{K}-\mathrm{mol}$ ?

In an irreversible process taking place at constant T and P and in which only pressure volume work is being done, the change in Gibbs free energy (dG) and change in entropy

When 500 J heat is given to the gas X in an isobaric process its work done comes out as 142.8 J. The gas X is