Work done is maximum in -

1. Isobaric work           

2. Isothermal work

3. Isochoric work         

4. Adiabatic work

For exothermic reaction to be spontaneous ($∆\mathrm{S}$=negative) temperature must be -

'The free energy change due to a reaction is zero when-

1. The reactants are initially mixed.

2.  A catalyst is added

3. The system is at equilibrium

4. The reactants are completely consumed

Equilibrium is represented by:

1. $∆$H = 0             

2. $∆$G_Total=0

3. $∆$S_Total=0         

4. $∆$E=0

Entropy decreases in which of the following reactions?

1. Boiling of egg

2. Combustion of benzene at 127$°$C

3. Stretching of rubber band

4. Dissolution of sugar in water

For a given reaction, $∆$H =35.5 kJ mol^-1 and $∆$S = 83.6JK^-1 mol^-1. The reaction is spontaneous at:
(Assume that $∆$H and $∆$S do not vary with temperature)

The standard enthalpy of vaporisation $∆$_vapH$°$ for water at 100$°$C is 40.66 kJ mol^-1. The

internal energy of vaporisation of water at 100$°$C (in kJ mol^-1) is- 

(Assume water vapour to behave like an ideal gas)

1. +37.56                   

2. -43.76

3. +43.76                   

4. +40.66

The enthalpy and entropy change for the reaction :

Br₂ (l) + Cl₂ (g)$\to$ 2BrCl (g)

are 30 kJ mol^-1 and 105 J K^-1 mol^-1 respectively.

The temperature at which the reaction will be in equilibrium is :

Which of the following is not a state function?

The work done in ergs for the reversible expansion of one mole of an ideal gas from a volume of 10 liters to 20 liters at 25°C is -

1. $-2.303\times 298\times 0.082$ $\log$ $2$

2. $-298\times {10}^7\times 8.31\times 2.303$ $\log$ $2$

3. $2.303\times 298\times 0.082$ $\log$ $0.5$

4. $-8.31\times {10}^7\times 298-2.303$ $\log$ $0.5$