Consider the reaction N2(g) + 3 H2(g) <=> 2 NH3(g), which is exothermic as written. What would be the effect on the equilibrium position of adding N2(g)?

Shift to the right side

Explanation:

Remember that any stress that we bring to a chemical equilibrium, will be answered by this in such a way as to minimize the disturbance and attain equilibrium again. This is known as LeChatelier´s principle.

If we add N₂(g) to the system at equilibrium

N₂ ( g) + 3 H₂(g)   ⇄ 2 NH₃(g)

the equilibrium will consume part of the added N₂ gas until it reaches equilibrium again producing more ammonia (NH₃).

Mathematically this is equivalent to a  decrease the pressure of N₂ so that the equilibrium partial pressures of the gases obey the equilbrium pressure constant Kp.

Therefore the equilibrium will shift to the product side.

oxygen, selenium, tellurium, and polonium.

they're all from the same group as sulfur (group 16).

> b takes place in the gas phase in an isothermal tubular reactor. the feed is one mole of a per one mole of c, an inert. the entering temperature and pressure are 427°c and 10 atm, respectively. the gas constant r = 0.08206 atm · l/mol · k.