The pair of isochoric among the transformation of state is:

1. K to L and L to M

2. L to M and N to K

3. L to M and M to N

4. M to N and N to K

Given, the following reaction:

$N_2{H}_4\left(g\right)\underset{ }{\to }{N}_2{H}_2\left(g\right)+H_2\left(g\right);$
Given:  ∆ H^∘ = 109 kJ/mol

B.E. of (N-N) = 163 kJ/mol

B.E. of (N-H) = 391 kJ/mol

B.E. of (H-H) = 436 kJ/mol

Calculate the bond enthalpy of N = N.

1. 182 kJ/mol

2. 400 kJ/mol

3. 300 kJ/mol

4. 218 kJ/mol

Thermodynamics is not concerned about:

Reversible expansion of an ideal gas under isothermal and adiabatic conditions are as shown in the figure:

 

AB$\to$Isothermal expansion

AC$\to$Adiabatic expansion

Which of the following options is not correct?

1. $∆S_{isothermal}>∆S_{adiabatic}$

2. $T_A=T_B$

3. $W_{isothermal}>W_{adiabatic}$

4. $T_C>T_A$

An ideal gas expands isothermally from ${10}^{-3}{m}^3 to {10}^{-2} m^3$ at 300 K against a constant pressure of ${10}^5 N{m}^{-2}$. The work done by  the gas is:

If for a certain reaction ${∆}_{r}H$ is 30 kJ mol^–1 at 450 K, the value of ${∆}_{r}S$ (in JK^–1 mol^–1) for which the same reaction will be spontaneous at the same temperature is:

Identify the correct statement regarding entropy:

When 1 mol gas is heated at constant volume, the temperature is raised from 298 to 308 K. Heat supplied to the gas is 500 J. The correct statement among the following is:
1.  q = w = 500 J, ∆U = 0
2.  q = ∆U = 500 J, w = 0
3.  q = w = 500 J, ∆U = 0
4.  ∆U = 0, q = w = – 500 J

Consider the following reactions: 

Enthalpy of formation of H₂O(l) is :

1. $-x_3$ $kJ$ $mo{l}^{-1}$

2. $-x_4$ $kJ$ $mo{l}^{-1}$

3. $-x_1$ $kJ$ $mo{l}^{-1}$

4. $-x_2$ $kJ$ $mo{l}^{-1}$

The heat of combustion of carbon to CO₂ is –393.5 KJ/mol. The heat released upon the formation of 35.2 g of CO₂ from carbon and oxygen gas is:
1. –315 KJ
2. +315 KJ
3. –630 KJ
4. +630 KJ