The following lists contain reactions and their corresponding equilibrium constants at different temperatures:

List-$I$ (Reaction)	List-$II$ $(K_p)$
$2 SO_{2(g)} + O_{2(g)} \rightleftharpoons 2 SO_{3(g)}$ at $298 \ K$	$4.0 \times 10^{24}$
$2 SO_{2(g)} + O_{2(g)} \rightleftharpoons 2 SO_{3(g)}$ at $700 \ K$	$3.0 \times 10^{4}$
$N_2O_{4(g)} \rightleftharpoons 2 NO_{2(g)}$ at $298 \ K$	$0.98$
$N_2O_{4(g)} \rightleftharpoons 2 NO_{2(g)}$ at $500 \ K$	$1700$

If $\Delta H_1^0$ and $\Delta H_2^0$ are the standard enthalpies for the reactions $2 SO_{2(g)} + O_{2(g)} \rightleftharpoons 2 SO_{3(g)}$ and $N_2O_{4(g)} \rightleftharpoons 2 NO_{2(g)}$ respectively, then:

• A
  Both $\Delta H_1^0$ and $\Delta H_2^0$ are negative
• B
  Both $\Delta H_1^0$ and $\Delta H_2^0$ are positive
• C
  $\Delta H_1^0$ is negative and $\Delta H_2^0$ is positive
• D
  $\Delta H_1^0$ is positive and $\Delta H_2^0$ is negative