Consider the following reaction at constant pressure:
$N_2(g)+2 O_2(g) \longrightarrow 2 NO_2(g) \quad \Delta H=+66.4 kJ$
Which of the following is true about change in the entropy of the surrounding and spontaneity of the reaction at 298 K ?
A$\Delta S_{\text {surr }}=+66.4 J / K$, reaction is spontaneous.
B$\Delta S_{\text {surr }}=-66.4 J / K$, reaction is not spontaneous.
C$\Delta S_{\text {surr }}=+223 J / K$, reaction is spontaneous.
D$\Delta S_{\text {surr }}=-223 J / K$, reaction is not spontaneous.
$N_2(g)+2 O_2(g) \longrightarrow 2 NO_2(g) \quad \Delta H=+66.4 kJ$
Which of the following is true about change in the entropy of the surrounding and spontaneity of the reaction at 298 K ?
A$\Delta S_{\text {surr }}=+66.4 J / K$, reaction is spontaneous.
B$\Delta S_{\text {surr }}=-66.4 J / K$, reaction is not spontaneous.
C$\Delta S_{\text {surr }}=+223 J / K$, reaction is spontaneous.
D$\Delta S_{\text {surr }}=-223 J / K$, reaction is not spontaneous.