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

1.	High	2.	Zero
3.	Constant	4.	Low

'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

Under which process is the maximum work achieved?

1. Isobaric work           

2. Isothermal work

3. Isochoric work         

4. Adiabatic work

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, if ΔH = 35.5 kJ/mol and ΔS = 83.6 J/K·mol, at what temperature is the reaction spontaneous?
(Assume ΔH and ΔS remain constant 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. $-8.31\times {10}^7\times 298-2.303$ $\log$ $0.5$