An irreversible process occuring isothermally in an isolated system leads to

(1) Zero entropy

(2) An increase in the total entropy of the system

(3) A decrease in the total entropy of the system

(4) None of these

The entropy values (in JK^-1 mol^-1) of H_2(g) = 130.6, Cl_2(g) = 223.0 and HCl_(g) = 186.7 at 298 K and 1 atm pressure. Then entropy change for the reaction ${\mathrm{H}}_{2\left(\mathrm{g}\right)}+{\mathrm{Cl}}_{2\left(\mathrm{g}\right)}\to 2{\mathrm{HCl}}_{\left(\mathrm{g}\right)}$ is

(1) + 540.3

(2) + 727.3

(3) – 166.9

(4) + 19.8

The ΔS for the vaporization of 1 mol of water is 88.3 J/mole K. The value of ΔS for the condensation of 1 mol of vapour will be

       1. 88.3 J/mol K

2. (88.3)² J/mol K

3. – 88.3 J/mol K

4. $\frac{1}{88.3}$ J/mol K        

The occurrence of a reaction is impossible if:

1. ΔH is +ve ; ΔS is also + ve but ΔH < TΔS

2. ΔH is – ve ; ΔS is also – ve but ΔH > TΔS

3. ΔH is – ve ; ΔS is + ve

4. ΔH is + ve ; ΔS is – ve

The enthalpy and entropy change for a chemical reaction are

–2.5 × 10³ cal and 7.4 cal deg^–1 respectively.  Predict the reaction at 298 K is

1. Spontaneous

2. Reversible

3. Irreversible

4. Non-spontaneous

Which of the following is true for the reaction $H_{2}O\left(l\right)\underset{}{\overset{}{\rightleftharpoons }}{H}_{2}O\left(g\right)$ at 100°C and 1 atmosphere

1. ΔE = 0

2. ΔH = 0

3. ΔH = ΔE

4. ΔH = TΔS

The enthalpy of vapourization water is 386 kJ. What is the entropy of water

(1) 0.5 kJ

(2) 1.03 kJ

(3) 1.5 kJ

(4) 22.05 kJ

Mark the correct statement regarding entropy.

An engine operating between 150°C and 25°C takes 500 J heat from a higher temperature reservoir if there are no frictional losses, then work done by engine is [MH CET 1999]

(1) 147.7 J

(2) 157.75 J

(3) 165.85 J

(4) 169.95 J

The standard entropies of CO₂(g), C(s) and O₂(g) are 213.5, 5.690 and 205 JK^–1 respectively. The standard entropy of formation of CO₂(g) is

(1) 1.86 JK^–1

(2) 1.96 JK^–1

(3) 2.81 JK^–1

(4) 2.86 JK^–1