The amount of N2 in the reaction vessel will increase

More NH3 will be produced

The reaction will first shift toward the products, then toward the reactants

The reaction will shift to the side with fewer total moles of gas

No change will occur

The reaction shifts to the right

The reaction will not be affected

The reaction shifts to the left

The reaction shifts to the right then to the left

All of these

Increasing the pressure

Increasing the temperature

Increasing the concentration of reactants

Adding a catalyst

increase . . . Le Chatelier's principle

decrease . . . Le Chatelier's principle

not affect . . . the common ion effect

decrease . . . the common ion effect

increase . . . the decreased pH

Decreasing the temperature

Increasing the pressure

Increasing the temperature

Increasing the concentration of reactants

Shaking the reaction flask

Adding to the system would cause the equilibrium to shift to the right, producing more in order to reduce the concentration of

Adding would not have any effect on the equilibrium

Adding to the system would cause the equilibrium to shift to the left, producing more in order to reduce the concentration of

Adding to the system would cause the equilibrium to shift to the right, producing more in order to reduce the concentration of

The effect of adding to the system cannot be predicted

The forward rate will be greater than the reverse rate

The reaction will shift left

The reaction is in equilibrium

The ratio of products to reactants is greater than the equilibrium constant