N\(_2\)(g) + 3H\(_2\)(g) ↔ 2NH\(_3\)(g) ΔH = - 90 kJ
In the equation above, the yield of ammonia can be decreased by

ekes0n

9 years ago

in exothermic reaction, increase in temperature favours the backward reaction.

goodlive715

1 year ago

A and C are correct
Becos in an exothermic reaction a decrease in temperature will shift the equilibrium to the right while an increase in pressure will favour the side with a lower number of mole therefore A and C are correct

Robertkolapo

6 years ago

the answer is B. removing ammonia formed reduces the concentration of the product thereby causing the equilibrium to shift from left to right

Ekwokk

1 year ago

I think the answer is A
increase in pressure always favour the side with lesser amount
since is an exothermic rxn increase in temperature Will favour the backward rxn.🤔

omgimd

1 year ago

wrong answer