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

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

One mole of non-ideal gas undergoes a change of state $\left(1.0 \mathrm{atm}, 3.0 \mathrm{L}, 200 \mathrm{K}\right)$ to $\left(4.0 \mathrm{atm}, 5.0 \mathrm{L}, 250 \mathrm{K}\right)$, with a change in internal energy $\left(\mathrm{\Delta U}\right)=40 \mathrm{L}-\mathrm{atm}$. The change in enthalpy of the process in $\mathrm{L}-\mathrm{atm}$;

In figure, $A$ and $B$ are two adiabatic curves for two different gases. Then, $A$ and $B$ correspond to,

For the gas - phase decomposition, ${\mathrm{PCl}}_5 \left(\mathrm{g}\right)\stackrel{\mathrm{\Delta }}{\rightleftharpoons }{\mathrm{PCl}}_3 \left(\mathrm{g}\right)+{\mathrm{Cl}}_2 \left(\mathrm{g}\right)$:

Which of the following statements is true? The entropy of the universe

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 ?

The enthalpy change for a given reaction at $298 \mathrm{K}$ is $-\mathrm{x} \mathrm{J} {\mathrm{mol}}^{-1}$ ($\mathrm{x}$ being positive). If the reaction occurs spontaneously at $298 \mathrm{K}$, the entropy change at that temperature