Use the information and balanced chemical equation to answer the following question. The Haber process is used to manufacture ammonia (NH3) from nitrogen (N2) and hydrogen (H2). 3 N2 (g)  +  3 H2 (g)  ⇌  2 NH3 (g)  What reaction conditions can you alter to increase the production of ammonia (NH3)? Select all that apply.   Question 19 options:   Adding either of the reactants, nitrogen or hydrogen, will shift the equilibrium in the direction of the products, resulting in the production of more ammonia.   Increasing the pressure of the system will shift the equilibrium in the direction of the reactants, resulting in the production of more ammonia.   Increasing the pressure of the system will shift the equilibrium in the direction of the products, resulting in the production of more ammonia.   Decreasing the pressure of the system will shift the equilibrium in the direction of the products, resulting in the production of more ammonia.   Removing either of the reactants, nitrogen or hydrogen, will shift the equilibrium in the direction of the products, resulting in the production of more ammonia.