Thermodynamics practice · Mixed difficulty

If 1 mole of gas expands from 1 litre to 5 litre against constant atmospheric
pressure than calculate the work done.

Hess’s law of constant heat summation is an application of :

In which of the following cases entropy decreases?

An ideal gas was subjected to a reversible adiabatic expansion then its initial volume was restored by reversible, isothermal compression. If ' $q$ ' denotes the heat added to the system and $w$ the work done on the system for the overall process then

Select the incorrect statement

One mono atomic gas is expanded adiabatically from $2L$ to $10L$ at $1\,\,atm$ external pressure, find $\Delta U$ (in $\mathrm{atm}\,\,L$ )

A $20 \mathrm{~g}$ piece of iron (specific heat capacity $=0.5 \mathrm{~J} / \mathrm{g}^{\circ} \mathrm{C}$ ) at $200^{\circ} \mathrm{C}$ is immersed in $100 \mathrm{~g}$ water of $27^{\circ} \mathrm{C}$.
What will be the temperature $\left({ }^{\circ} \mathrm{C}\right)$ of this system at thermal equilibrium?

$\mathrm{C} + {\mathrm{O}_2} \to \mathrm{C}{\mathrm{O}_2};$
$\mathrm{CO} + \frac{1}{2}{\mathrm{O}_2} \to \mathrm{C}{\mathrm{O}_2}$
Then the heat of formation of CO is

Which one among the following is the correct option for right relationship between ${C_p}\mathrm{ and }{C_v}$ for one mole of ideal gas?

Which is the correct Gibb's Helmholtz
equation?

The dissociation energy of $\mathrm{C}{\mathrm{H}_4}$ and ${\mathrm{C}_2}{\mathrm{H}_6}$ are respectively 360 and 620 kcal/mol. The bond energy of C-C bond is:

Which of the following is not a thermodynamic property of a system?

The enthalpy of vaporization of a liquid is 30 kJ $\mathrm{mo}{\mathrm{l}^{ - 1}}$ and entropy of vaporization is 75 J $\mathrm{mo}{\mathrm{l}^{ - 1}}$. The boiling point of liquid at 1 atm is :

For one mole of an ideal gas

The enthalpy and entropy change for a chemical reaction are  $- \,2.5\,\, \times {10^\mathrm{3}}\mathrm{cal}\,\,\mathrm{and}\,\,7.4\,\,cal\,{K^{ - 1}}$  respectively.Predict that nature of reaction at 298 K is:

A reaction occurs spontaneously if:

$If,{\mathrm{H}_2}\left( \mathrm{g} \right) + \mathrm{C}{\mathrm{l}_2}\left( \mathrm{g} \right) \to 2\mathrm{HCl};\Delta {H^0} = - 44\mathrm{kcal}$
2Na(s)+2HCl(g)→2NaCl(s)+${H_2}$ (g);
∆H= -152 kcal then,
$\mathrm{Na}\left( s \right) + 0.5\mathrm{C}{\mathrm{l}_2}\left( \mathrm{g} \right) \to \mathrm{NaCl}\left( s \right);\Delta {H^0} = ?$

Which statements are correct?

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

Which is true for internal energy of system is

Statement I: A reaction which is spontaneous and
accompanied by decrease of randomness must be
exothermic.

Statement II: All exothermic reactions are
accompanied by decrease of randomness.

A boiled egg show a/an …in entropy.

Statement I: The final temperature of an ideal
gas in adiabatic compression is less in reversible
compression than in irreversible compression
against a constant external pressure.

Statement II: The magnitude of work done on
an ideal gas in adiabatic compression is more in
irreversible process than that in reversible process.

For one mole of an ideal gas, which of these statements must be true?
A) $U\,\,\mathrm{ and}\,\,\mathrm{ }H$ each depends only on temperature
B) Compressibility factor Z is not equal to 1.
C) ${C_{p,\,\,m}} - {C_{V,\,\,m}} = R$
D) $dU = {C_V}dT$ for any process.

$\mathrm{A}_{2}+\mathrm{B}_{2} \rightarrow 2 \mathrm{AB} . \Delta \mathrm{H}_{\mathrm{f}}=-200 \,\mathrm{kJ} \,\mathrm{mol}^{-1}$
$\mathrm{A B, A_{2}}$ and $\mathrm{B_{2}}$ are diatomic molecules. If the bond enthalpies of $\mathrm{A_{2}, B_{2}}$ and $\mathrm{A B}$ are in the ratio $1: 0.5: 1$, then the bond enthalpy of $\mathrm{A_{2}}$ is ____ $\mathrm{kJ} \,\mathrm{mol^{-1}}$ (Nearest integer)

A mixture of two moles of carbon monoxide and one mole of oxygen, in a closed vessel is ignited to convert the carbon monoxide to carbon dioxide. If ∆H is the enthalpy change and ∆E is the change in internal energy, then

The heat of neutralization of $HCl$ by $NaOH$ is – 55.9 KJ/mol. If the heat of neutralization of $HCN$ by $NaOH$ is – 12.1 KJ/mol. The heat of dissociation of $HCN$ is

The heat of combustion of methane is $- \;880\;\mathrm{kJ\;mo}{\mathrm{l}^{ - 1}}.$. If 3.2 g of methane is burnt:

The second law of thermodynamics introduced the concept of:

STATEMENT-1 : There cannot be chemical equilibrium in an open system.

STATEMENT-2 : There is no fixed mass in an open system.