When one mole of monoatomic ideal gas at TK undergoes reversible adiabatic change under a constant external pressure of 1 atm changes volume from 1 litre to 2 litre. The final temperature in kelvin would be:

1. T/(2)^2/3                                         

2. T + 2/(3x0.0821)

3. T                                                   

4. T - 3/(2x0.0821)

Which is not a spontaneous process?

1. Expansion of gas into the vacuum

2. Water flowing downhill

3. Heat flowing from a colder body to a hotter body

4. Evaporation of water from clothes during drying

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

1. decrease of free energy                     

2. increase of free energy

3. decrease of entropy                           

4. increase of enthalpy

A gaseous system changes from state A(P₁, V₁, T₁) to B(P₂,V₂,T₂), B to C(P₃, V₃, T₃) and finally from C to A. The whole process may be called:

1. reversible process                           

2. cyclic process

3. isobaric process                               

4. spontaneous process

One mole of ice is converted into the water at 273 K. The entropies of H₂O(s) and H₂O(l) are 38.20 and 60.01 J mol^-1K^-1 respectively. The enthalpy change for the conversion is:

1. 59.54 J mol^-1                               

2. 5954 J mol^-1

3. 595.4 J mol^-1                             

4. 320.6 J mol^-1

$∆\mathrm{S}°$ will be highest for the reaction:

1. Ca(s) + 1/2 O₂(g) $\to$CaO(s)

2. CaCO₃(s)$\to$CaO(s) + CO₂(g)

3. C(s) + O₂(g)$\to$CO₂(g)

4. N₂(g) + O₂(g)$\to$2NO(g)

Which statements are correct?

1. $2.303 \log \frac{{\mathrm{P}}_2}{{\mathrm{P}}_1}=\frac{∆{\mathrm{H}}_{\mathrm{vap}.}}{\mathrm{R}}\frac{\left[{\mathrm{T}}_2-{\mathrm{T}}_1\right]}{{\mathrm{T}}_1{\mathrm{T}}_2}$ is called Clausius-Clapeyron equation

2. $\frac{∆{\mathrm{H}}_{\mathrm{vap}.}}{\mathrm{Boiling} \mathrm{Point}}=88 J mo{l}^{-1}{K}^{-1}$ is called Trouton's rule

3. Entropy is a measure of unavailable energy, i.e.,

     unavailable energy = entropy x temperature

4. All of the above

The mathematical form of the first law of thermodynamics when heat (q) is supplied and W is work done by the system (-ve) is:

1. $∆$U=q+W                       

2. $∆$U=q-W

3. $∆$U=-q+W                       

4. $∆$U= -q-W

Change in entropy is negative for:

1. Bromine (l)$\to$Bromine(g)

2. C(s) + H₂O(g) $\to$CO(g) + H₂(g)

3. N₂(g,10 atm)$\to$N₂(g,1 atm) 

4. Fe ( 1mol, 400 K) $\to$ Fe( 1mol, 300 K)

The internal energy change when a system goes from state A to B is 40 kJ/mol. If the system goes from A to B by a reversible path and returns to state A by an irreversible path. What would be the change in internal energy?

1. 40 kJ                                   

2. >40 kJ

3. <40 kJ                                 

4. Zero