For the reaction N2(g) + 3H2(g) 2NH3(g), what will happen if more ammonia gas is added?

The reaction will tend to the right.

For the reaction N2(g) + 3H2(g) 2NH3(g), what will happen if more ammonia gas is added?

If more ammonia gas (NH3) is added to the reaction N2(g) + 3H2(g) -> 2NH3(g), the reaction will shift to the left in order to balance out the increase in NH3. This is known as Le Chatelier's principle, which states that a system at equilibrium will adjust to counteract any changes imposed upon it.

In other words, by adding more NH3 to the mixture, the reaction will shift in the direction that consumes NH3 in order to establish a new equilibrium. In this case, the new equilibrium will involve a decrease in NH3 and an increase in N2 and H2.

To understand this conceptually, imagine that the reaction is like a seesaw. When you add more NH3 to one side, the reaction "seesaw" will tilt towards the N2 and H2 side, as the system tries to counterbalance the increase in NH3.

To quantitatively determine the new equilibrium concentrations, you can use the reaction's equilibrium constant (Kc) and the stoichiometry of the reaction. The equilibrium constant is a mathematical expression that relates the concentrations of reactants and products at equilibrium. In this case, Kc = [NH3]^2 / ([N2][H2]^3), where [X] denotes the concentration of X.

By plugging in the initial concentrations of the reactants and products and calculating their respective changes based on Le Chatelier's principle, you can determine the new equilibrium concentrations. It's important to note that the concentration changes will depend on the initial concentrations and the value of Kc.

So, in summary, if more ammonia gas is added to the reaction N2(g) + 3H2(g) -> 2NH3(g), the reaction will shift to the left to consume the excess NH3, resulting in a decrease in NH3 and an increase in N2 and H2 concentrations to establish a new equilibrium.