Given N2(g) + 3H2 = 2NH3(g), which scenario will allow you to eventually reach an equillibrium mixture involving these chemicals?

A. Place only H2 into a sealed vessel.
B.Place only NH3 into a sealed vessel.
C.Place only N2 into a sealed vessel.
D.All of the above scenarios.
E.none of the above.

According to the collision theory of Chemical reactions:
A. High Energy collisions result in few successful reactions as there isn't sufficient time for the products to react.
B. High Energy collisions lead to the successful formation of products.
C. Low energy collisions do not occur in the gas phase.
D. Low energy collisions result in many successful reactions are there is sufficient time for the reactants to form products.
E. All of the above.

B & B?

D and B

To reach an equilibrium mixture involving N2(g), H2, and NH3(g), all three components must be present together. This means that the scenario that will allow you to eventually reach an equilibrium mixture is Option D: All of the above scenarios (placing only H2, NH3, or N2 into a sealed vessel).

According to the collision theory of chemical reactions, the correct statement is Option A: High Energy collisions result in few successful reactions as there isn't sufficient time for the products to react. High energy collisions do not necessarily lead to successful formation of products. In fact, successful reactions require both sufficient energy and proper orientation of the molecules. Low energy collisions do occur in the gas phase, and they can result in successful reactions if the molecules have enough time and proper orientation to react. Therefore, the correct answer is Option A: High Energy collisions result in few successful reactions as there isn't sufficient time for the products to react.

To reach an equilibrium mixture involving the chemicals N2(g), H2, and NH3(g), the scenario that would be appropriate is D. All of the above scenarios.

In order to reach equilibrium in the given reaction, it is necessary to have all the reactants present. This is because in order for the forward reaction (N2(g) + 3H2 -> 2NH3(g)) to occur, the reactants N2 and H2 must be present. And in order for the reverse reaction (2NH3(g) -> N2(g) + 3H2) to occur, the reactant NH3 must be present.

If only H2 is placed in a sealed vessel, the forward reaction cannot occur as there is no N2 present. If only NH3 is placed in a sealed vessel, the reverse reaction cannot occur as there is no H2 present. If only N2 is placed in a sealed vessel, the forward and reverse reactions cannot occur as there are no appropriate reactants present.

Therefore, to eventually reach an equilibrium mixture involving N2, H2, and NH3, it is necessary to have all of the above scenarios.

As for the collision theory of chemical reactions, the correct statement is A. High-energy collisions result in few successful reactions as there isn't sufficient time for the products to react. High-energy collisions have a higher probability of breaking bonds and leading to the formation of products. However, these collisions often result in fragmented molecules that may not have enough time to reform into stable products.

Option B, high-energy collisions leading to the successful formation of products, is incorrect because high-energy collisions can lead to the fragmentation of molecules rather than successful reaction.

Options C and D are incorrect because low-energy collisions can occur in the gas phase and can lead to successful reactions given sufficient time.

Therefore, the correct statement is A. High-energy collisions result in few successful reactions as there isn't sufficient time for the products to react.