N2(g) + 3 H2(g) <—> 2 NH3(g)
DH = −92 kJ/mol ; DG = -33 kJ/mol
Consider the reaction represented above at 298 K. When equal volumes of N2(g) and H2(g), each at 1 atm, are mixed in a closed container at 298 K, no formation of NH3(g) is observed. Which of the following best explains the observation?
(A) The N2(g) and the H2(g) must be mixed in a 1:3 ratio for a reaction to occur.
(B) A high activation energy makes the forward reaction extremely slow at 298 K.
(C) The reaction has an extremely small equilibrium constant, thus almost no product will form.
(D) The reverse reaction has a lower activation energy than the forward reaction, so the forward reaction does not occur.
