Thermodynamics ...

For the process :

A gas mixture consists of $$2$$ moles of $$O_2$$ and $$4$$ moles of Ar at temperature $$T$$. Neglecting all vibrational modes, the total internal energy of the system is 

For vaporization of water at $$ 1$$ atmospheric pressure, the values of $$\Delta$$H and $$\Delta$$S are $$40.63 kJ mol^{-1}  and $$108.8 JK$$^{-1}$$mol$$^{-1}$$, respectively. The temperature when Gibb's energy change ($$\Delta$$G) for this transformation will be zero, is : 

The following two reactions are known 

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

Consider the following processes:
                                                  $$\Delta H\left({kJ}/{mol}\right)$$
$$\dfrac{1}{2} A \rightarrow B$$                               $$+150$$

For the reaction, $$X_2O_4(i)\rightarrow 2XO_2(g)$$, $$\Delta U=2.1k cal, \Delta s=20 cal K^{-1}$$ at 300 K. 

One mole of an ideal diatomic gas undergoes a transition from A to B along a path AB as shown in the figure, The change in internal energy of the gas during the transition is:

Which law of the thermodynamics helps in calculating the absolute entropies of various substances at different temperatures?

Assertion (A) : Zeroth law of thermodynamics gives us the concept of energy
Reason (R) : Internal energy is dependent on temperature