Embibe Experts Solutions for Chapter: Thermodynamics, Exercise 1: Exercise-1

Is the entropy of the universe constant ?

What is the equilibrium constant $\mathrm{K}$ for the following reaction at $400 \mathrm{K}$?

$2\mathrm{NOCl}\left(\mathrm{g}\right)\rightleftharpoons 2\mathrm{NO}\left(\mathrm{g}\right)+{\mathrm{Cl}}_2\left(\mathrm{g}\right)$

$∆\mathrm{H}°=77.2 \mathrm{kJ} {\mathrm{mol}}^{-1} \mathrm{and} ∆\mathrm{S}°=122 {\mathrm{JK}}^{-1}{\mathrm{mol}}^{-1 }\mathrm{at} 400\mathrm{K}$

In an isochoric process, the increase in internal energy is:

State the second law of thermodynamics.

State the thermodynamic conditions of spontaneous occurrence of the processes.

Which of the following conditions, regarding a chemical process, ensures its spontaneity at all temperatures?

What is the free energy change $\left(\mathrm{\Delta G}\right)$ when $1.0$ mole of water at $100°\mathrm{C}$ and $1 \mathrm{atm}$ pressure is converted into steam at $100°\mathrm{C}$ and $1 \mathrm{atm}$ pressure ?

Diborane is a potential rocket fuel which undergoes combustion according to the reaction, ${\mathrm{B}}_2{\mathrm{H}}_6\left(\mathrm{g}\right)+3{\mathrm{O}}_2\left(\mathrm{g}\right)⟶{\mathrm{B}}_2{\mathrm{O}}_3\left(\mathrm{s}\right)+3{\mathrm{H}}_2\mathrm{O}\left(\mathrm{g}\right)$

From the following data, calculate the enthalpy change for the combustion of diborane 

$2\mathrm{B}\left(\mathrm{s}\right)+\frac{3}{2}{\mathrm{O}}_2\left(\mathrm{g}\right)⟶{\mathrm{B}}_2{\mathrm{O}}_3\left(\mathrm{s}\right); \mathrm{\Delta H}=-1273 \mathrm{kJ}$            ...$\left(1\right)$

${\mathrm{H}}_2\left(\mathrm{g}\right)+\frac{1}{2}{\mathrm{O}}_2\left(\mathrm{g}\right)⟶{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right); \mathrm{\Delta H}=-286 \mathrm{kJ}$            ....$\left(2\right)$

${\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)⟶{\mathrm{H}}_2\mathrm{O}\left(\mathrm{g}\right); \mathrm{\Delta H}=44 \mathrm{kJ}$            ....$\left(3\right)$

$2\mathrm{B}\left(\mathrm{s}\right)+3{\mathrm{H}}_2\left(\mathrm{g}\right)⟶{\mathrm{B}}_2{\mathrm{H}}_6\left(\mathrm{g}\right); \mathrm{\Delta H}=36 \mathrm{kJ}$     ...$\left(4\right)$