Use gaseous mole numbers for pressure and reaction enthalpy for temperature, while stating that a catalyst speeds both directions equally and does not shift equilibrium.
Ammonia is manufactured in the Haber Process.
In this process, pressures between 100 atm and 300 atm and temperatures between 675 K and 725 K are usually used.
The pressure of the system is doubled at constant temperature.
Explain the effect of this on the yield of ammonia by considering the change in the Kp expression and hence the position of equilibrium.
(3)
An explanation that makes reference to the following points: - ( K_p ) remains the same (1) - Fraction / quotient / Q / Q_p / apparent value of K_p decreases in value (when pressure increases) (1) - so equilibrium shifts to right hand side (to return K_p to its original value / to keep K_p constant) (1) Allow partial pressures of denominator / N_2 and H_2 increases more than the numerator / NH_3 Ignore use of Le Chatelier's Principle Must be linked to Q_p returning to the value of K_p not as a result of Le Chatelier's Principle Allow produces more ammonia (so K_p is constant / returns to original value)