The Haber process produces ammonia commercially. It is represented by the equation N2(g) 3H2(g) --> 2NH3(g) To completely convert 9.0 mol hydrogen gas to ammonia gas, how many moles of nitrogen are required

3 moles

Explanation:

The balanced equation for the reaction is given below below:

N2(g) 3H2(g) --> 2NH3(g)

From the balanced equation above,

1 mole of N2 required 3 moles of H2.

Therefore, Xmol of N2 will require 9 moles of H2 i.e

Xmol of N2 = 9/3

Xmol of N2 = 3 moles

From the calculations made above, 3 moles of nitrogen (N2) is needed to completely convert 9.0 mol hydrogen gas(H2) to ammonia gas (NH3)

adding or remove a gaseous reactant or product changes the concentrations. if the concentration of reactant or product is increased, the system will shift away from the side in which concentration was increased (i.e. if the concentration of reactants is increased, the system will shift toward the products. if more products are added, the system will shift to form more reactants). conversely, if the concentration of reactant or product is decreased, the system will shift toward the side in which concentration was decreased (i.e. if reactants are removed, the system will shift to form more reactants. if the concentration of products is decreased, the equilibrium will shift toward the products).

explanation: