Thermodynamics practice · Mixed difficulty

Equal volumes of monoatomic and diatomic gases at same initial temperature and pressure are mixed. The ratio of specific heats of the mixture $\;({C_p}/{C_v})$will be

A container has hydrogen and oxygen mixture in ratio of 1 : 1 by weight, then

The entropy change (in cal $\mathrm{K}^{-1} \mathrm{~mol}^{-1}$ ) when one mole of an ideal gas at $27^{\circ} \mathrm{C}$ is expanded reversibly from $1 \ell$ to $10 \mathrm{~I}$ is

1 mole of an ideal gas at 25℃ is subjected to expand reversibly ten times of its initial volume. The change in entropy of expansion is:

Calculate the Gibbs energy change when 1 mole of ${NaCl}$ is dissolved in water at $298 {~K}$. Given,

(a) Lattice energy of ${NaCl}=778 {~kJ} {~mol}^{-1}$.

(b) Hydration energy of ${NaCl}=774.3 {~kJ} {~mol}^{-1}$.

(c) Entropy change at $298 {~K}=43 {~J} {~mol}^{-1}$.

The dissolution of ${CaCl}_2 \cdot 6 {H}_2 {O}$ in a large volume of water is endothermic to the extent of $3.5 \mathrm{~kcal/mol}.$ For the reaction, ${CaCl}_2(\mathrm{s})+6 {H}_2 {O}({l}) \rightarrow{CaCl}_2 \cdot 6 {H}_2 {O}(\mathrm{s}) ; \Delta H$ is $-23.2 \mathrm{~kcal}.$ The heat of solution of anhydrous ${CaCl}_2$ in large quantity of water will be

In which case of mixing of a strong acid and a base each of 1N concentration, temperature increase is highest?

Which is correct relation between $\mathrm{C}_{\mathrm{p}}$ and $\mathrm{C}_{\mathrm{v}}$ for one mole of ideal gas

When $100 \mathrm{~ml}$ of $1.0 \mathrm{~M} \mathrm{~HCl}$ was mixed with $100 \mathrm{~ml}$ of $1.0 \mathrm{~M} \mathrm{~NaOH}$ in an insulated beaker at constant pressure, a temperature increase of $5.8^{\circ} \mathrm{C}$ was measured for the beaker and its constants. If the enthalpy of neutralization of a strong acid with a strong base is $-58.0 \mathrm{~kJ} \mathrm{~mol}^{-1}$. the calorimeter constant in $\left(\mathrm{kJ} \mathrm{k}^{-1}\right)$ is ___
(Given: Heat capacity of solution is $4.2 \mathrm{~J} \mathrm{~g}^{-1} \mathrm{k}^{-1}$ and density of solution is $1 \mathrm{~g} \mathrm{~mL}^{-1}$)

For the reaction, $\mathrm{N}_2+3 \mathrm{H}_2 \rightleftharpoons 2 \mathrm{NH}_3 ; \Delta \mathrm{H}=$ ?

Which one of the following is used to remove most of plutonium from spent nuclear fuel?

In the exothermic reaction, the enthalpy of reaction is always:

Enthalpies of formation of $CO\left( g \right),\,\,\,C{O_2}\left( g \right),\,\,\,{N_2}O\left( g \right)$ and ${N_2}{O_4}\left( g \right)$ are –110, –393, 81 and 9.7 KJ/mol respectively. Find the value of ${\Delta _r}H$ for the reaction ${N_2}{O_4}\left( g \right) + 3CO\left( g \right) \to {N_2}O\left( g \right) + 3C{O_2}\left( g \right)$

For an adiabatic process:

500 J of energy is transferred as heat to 0.5 mol of Argon gas at 298 K and 1.00 atm. The final temperature and the change in internal energy respectively are:

Given: $\mathrm{R}=8.3 \mathrm{~J} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}$

Assertion :- The value of specific heat at constant pressure is more than that at constant
volume.

Reason :- The energy required to raise temperature by a unit at constant pressure is
greater because some amount of heat is used in doing work.

The standard heat of combustion of propane is $-2220.1 \mathrm{~kJ} / \mathrm{mol}.$ The standard heat of vaporization of liquid water is $44 \mathrm{~kJ} / \mathrm{mol}.$ What is the $\Delta H^{\circ}$ of the following reaction?

$\mathrm{C}_3 \mathrm{H}_8(\mathrm{g})+5 \mathrm{O}_2(\mathrm{g}) \rightarrow 3 \mathrm{CO}_2(\mathrm{g})+4 \mathrm{H}_2 \mathrm{O}(\mathrm{g})$

Which of the following taking place in the blast furnace is endothermic?

The entropy change accompanying the transfer of $12,000 \mathrm{~J}$ of heat from a body ${A}$ at $327^{\circ} \mathrm{C}$ to a body $B$ at $127^{\circ} \mathrm{C}$ is

Thermochemistry is the study of relationship between heat energy and :

$56 \mathrm{~g}$ of iron reacts with $\mathrm{HCl}$ in a closed vessel of fixed volume. Again, same amount of $\mathrm{Fe}$ is made to react in an open beaker at $27^{\circ} \mathrm{C}$. The work done (in cal) in both the cases will be respectively

The ratio $K_p$ to $K_c$ of a reaction is $24.63 \mathrm{~L ~atm ~mol}^{-1}$ at $27^\circ \mathrm{C}$. If heat of reaction at constant pressure is 98.8 kcal, what is the heat of reaction (in kcal) at constant volume?

The least random state of ${H_2}O$ is

$\mathrm{NH}_4 \mathrm{Cl}(s)+\mathrm{H}_2 \mathrm{O}(a q) \rightleftharpoons \mathrm{NH}_4 \mathrm{Cl}(a q)$

Due to dissolution of ammonium chloride in $\mathrm{H}_2 \mathrm{O}$, temperature falls rapidly. Thus,

The correct descending order of the heat liberated (in $\mathrm{kJ}$ ) during the neutralisation of the acids $\mathrm{CH}_3 \mathrm{COOH}(W), \mathrm{HF}(X), \mathrm{HCOOH}(Y)$ and $H C N(Z)$ under indentical conditions $\left(K_a\right.$ of $\mathrm{CH}_3 \mathrm{COOH}=1.8 \times 10^{-5}, {H C O O H}=1.8 \times 10^{-4}$, $\mathrm{HCN}={4 . 9} \times 10^{-10}$ and $\mathrm{HF}=3.2 \times 10^{-4}$ ) is

A diatomic gas at pressure $\mathrm{P}$, compressed adiabatically to half of its volume, what is the final pressure?

The standard enthalpy of formation $\left(\Delta_f {H}^{\circ}{ }_{298}\right)$ for methane, ${CH}_4$ is $-74.9 {~kJ} {~mol}^{-1}$. In order to calculate the average energy given out in the formation of a ${C}-{H}$ bond from this it is necessary to know which one of the following?

Spontaneous adsorption of a gas on solid surface is an
exothermic process because

For the reaction,

$\mathrm{CaO}(s)+\mathrm{SO}_3(g) \longrightarrow \mathrm{CaSO}_4(s) ; \Delta G^{\circ}=-345.0 \mathrm{~kJ}$

$\Delta G$ for the reaction at $298 \mathrm{~K}$ when the pressure of $\mathrm{SO}_3$ is $0.5 \mathrm{~atm}$ is

Assertion : For a reaction

$2 {NH}_3({~g}) \longrightarrow {N}_2({~g})+3 {H}_2({~g}) ; \Delta H>\Delta E$

Reason : Enthalpy change is always greater than internal energy change.