Question

1) For the reaction below, describe the temperature and pressure conditions that would produce the highest yield for the forward reaction. Explain your answer in terms of Le Châtelier’s principle.

N2 (g) + 3 H2 (g) Two arrows stacked on top of each other. The top arrow points to the right. The bottom arrow points to the left. 2 NH3 (g) deltaH = -92 kJ/mol

2) Explain, in terms of particles, concentration, and reaction rate, what you expect to happen when methane gas (CH4) and hydrogen sulfide gas (H2S) are sealed in a flask and reach a state of equilibrium.

CH4 (g) +2 H2S (g) Two arrow

Answer 1

do you know what is Le Châtelier’s principle

Answer 2

1)
temperature: as reaction is exothermic lower temperatures would move reaction towards products (reaction gives heat, so according to Le Châtelier’s principle by lowering temperature system will try to regain its temperature and only way that is possible is by making more products and thus generating more heat)
pressure:
cause there are 4 moles of reactants and 2 moles of products increasing pressure would have as a consequence that more products are created

although all i said above is logically and according to Le Châtelier’s principle true synthesis of ammonia is done depending on types of facility (Haber-Bosch process) at cca 450-500 bar and 250 - 300 °C (those are pressure and temperature in factory for production of fertilizer in my city)

Answer 3

2) do you mean this reaction:
CH4 + 2 H2S <--> CS2 + 4 H2