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

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)

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