On page 191 of Conquering Chemistry. (1 Viewer)

[SoCal]

On page 191 of Conquering Chemistry about half way down the page (under the synthesis of ammonia reaction) it says "This is an equilibrium reaction which at ordinary pressures and temperatures lies well to the left." Can anyone please tell me what "lies well to the left" means exactly? Thank you.

 

[babydoll_]

two sides of an equation
A + B ----> C + D
left ______right
i.e. equilibrium favours the left: the reactants. get me?

 

[iambored]

yeah, so at ordinary temp and pressure it's on the side of the reactants
i.e. H2 and N2
meaning that there will be mostly H2 and N2 and barely any ammonia

however, if u raise the temp it lies further to the right, coz more ammonia will b formed

if it's confusing u maybe it's just coz they're putting common sense in a weird way

 

[SoCal]

Thank you for the quick reply people. I think I get it now, it is saying that under normal circumstances Nitrogen and Hydrogen is produced from Ammonia?

 

[Constip8edSkunk]

hmmm higher temp -----> equilibrium will shift to the left

thats y the fritzhaber process keeps the temp as low as possible while still high enough to achieve a sufficient rate so a decent yield of ammonia is produced.

presure is the main reason that the reaction lies mainly to the left, one must increase the pressure to 250 atm. in the industrial process to shift it 2 the right and have satisfactory yield

 

[SoCal]

I understand now thank you everyone. Under normal circumstances ammonia will decompose to nitrogen and hydrogen in the reverse direction:

N2(g) + 3H2(g) <----- 2NH3(g)

Only under laboratory conditions will the synthesis of ammonia occur.