Calculate the increase in entropy (approximate) of $3 \ mol$ of hydrogen gas as it changes from $300 \ K$ at $0.1 \ atm$ to $1000 \ K$ at $1 \ atm$ $(C_p = 7 \ cal \ K^{-1} \ mol^{-1})$. $[\log \ 3.33 \approx 0.52, \ \ln \ x = 2.3 \ \log \ x]$ .......$cal \ K^{-1}$

Which of the following is zero during the adiabatic expansion of a gas?

State the limitation of the $2^{nd}$ law of thermodynamics.

The $S^o$ of the following substances are:
$CH_{4(g)} : 186.2 \ J \ K^{-1} \ mol^{-1}$
$O_{2(g)} : 205.2 \ J \ K^{-1} \ mol^{-1}$
$CO_{2(g)} : 213.6 \ J \ K^{-1} \ mol^{-1}$
$H_2O_{(l)} : 69.9 \ J \ K^{-1} \ mol^{-1}$
The entropy change $\Delta S^o$ . . . . . . $J \ K^{-1} \ mol^{-1}$ for the reaction
$CH_{4(g)} + 2O_{2(g)} \to CO_{2(g)} + 2H_2O_{(l)}$ is

Observe the following reactions:
$I$. $CaCO_{3(s)} \rightarrow CaO_{(s)} + CO_{2(g)}$
$II$. $Cl_{2(g)} \rightarrow 2 Cl_{(g)}$
$III$. $H_2O_{(l)} \rightarrow H_2O_{(s)}$
Identify the reactions in which entropy increases.

Which state functions are required to understand the second law of thermodynamics?