Embibe Experts Solutions for Chapter: Thermodynamics, Exercise 1: AIPMT - 4th May 2014

Which of the following $\mathrm{p}-\mathrm{V}$ curve represents maximum work done?

Which one among the following is the correct option for right relationship between ${\mathrm{C}}_{\mathrm{p}}$ and ${\mathrm{C}}_{\mathrm{v}}$ for one mole of ideal gas?

For irreversible expansion of an ideal gas under isothermal condition, the correct option is:

If for a certain reaction ${\Delta }_{\mathrm{r}}\mathrm{H}$ is $30 {\mathrm{kJmol}}^{-1}$ at $450\mathrm{K},$ the value of ${\mathrm{\Delta }}_{\mathrm{r}}\mathrm{S}$ (in ${\mathrm{JK}}^{-1}{\mathrm{mol}}^{-1}$) for which the same reaction will be spontaneous at the same temperature is

At standard conditions, if the change in the enthalpy for the following reaction is $-109 {\mathrm{kJmol}}^{-1}$

${\mathrm{H}}_{2\left(\mathrm{g}\right)}+{\mathrm{Br}}_{2\left(\mathrm{g}\right)}\to 2{\mathrm{HBr}}_{\left(\mathrm{g}\right)}$

Given that bond energy of ${\mathrm{H}}_2$ and ${\mathrm{Br}}_2$ is $435 {\mathrm{kJmol}}^{-1}$ and $192 {\mathrm{kJmol}}^{-1}$, respectively, what is the bond energy (in $\mathrm{kJ} {\mathrm{mol}}^{-1}$) of $\mathrm{HBr}?$

For the reaction, $2\mathrm{Cl}\left(\mathrm{g}\right)\to {\mathrm{Cl}}_2\left(\mathrm{g}\right)$, the correct option is

The correct option for free expansion of an ideal gas under adiabatic condition is

For the reaction:
${\mathrm{X}}_2{{\mathrm{O}}_4}_{\left(\mathrm{l}\right)}\to 2\mathrm{X}{{\mathrm{O}}_2}_{\left(\mathrm{g}\right)}$
$∆\mathrm{U}=2.1\mathrm{ }\mathrm{kcal},\mathrm{ }∆\mathrm{S}=20\mathrm{ }\mathrm{cal}\mathrm{ }{\mathrm{K}}^{-1}$ at $300\mathrm{ }\mathrm{K}$
Hence, $∆\mathrm{G}$ is: