Answer to Question #300694 in General Chemistry for bbibbiuuu

Question

The Haber process for the synthesis of ammonia from nitrogen and hydrogen gases in an exothermic process.

N2(g) + 3H2(g) ⇌ 2 NH3 (g) ΔHrxn= -92.4 kJ

How will the following conditions affect the equilibrium of the system?

a) adding more N₂ =

b) removing 3H₂    =

c) removing NH₃    =

d) increasing the pressure in the reaction vessel   =

e) decreasing the temperature of the system        =

Answer 1

According to the Le Chatelier's principle, if the stress is applied to the system, the equilibrium will shift in the direction that counteracts the stress. Therefore,

a) Equilibrium will shift to the right;

b) Equilibrium will shift to the left;

c) Equilibrium will shift to the right;

d) Equilibrium will shift to the right (less moles of the gas = lower pressure);

e) Equilibrium will shift to the right (since the process is exothermic, the heat should be considered as a product).