urea hydrolysis

[observer1]

In the wiki, it is given that urea reacts with water to form ammonia and CO₂.
CO(NH₂)₂ + H₂O → 2 NH₃ + CO₂

But when I add urea into water, neither is there and gas coming out as CO₂ or any decrease in the level of water
The urea just dissolved. 
How to stop this and make the reaction?

[chenbeier]

Need time and bacteria. Smell in toilet room.

[exchemist]

5 hours ago, observer1 said:

In the wiki, it is given that urea reacts with water to form ammonia and CO₂.
CO(NH₂)₂ + H₂O → 2 NH₃ + CO₂

But when I add urea into water, neither is there and gas coming out as CO₂ or any decrease in the level of water
The urea just dissolved. 
How to stop this and make the reaction?

Can you link to where in "the wiki" you saw this? All the links I saw say you need an enzyme (urease) to catalyse this decomposition.

Here is a procedure for doing that: https://edu.rsc.org/download?ac=12704

[observer1]

3 hours ago, exchemist said:

Can you link to where in "the wiki" you saw this?

Urea - Wikipedia, go to automobile systems

[chenbeier]

Add blue reaction is  in the combustion  chamber ( cylinder) of  an internal combustion engine. Add blue is an aqueaous solution of urea. During the combustion  takes place it decompose like in wiki written.

[John Cuthber]

9 hours ago, observer1 said:

In the wiki, it is given that urea reacts with water to form ammonia and CO₂.
CO(NH₂)₂ + H₂O → 2 NH₃ + CO₂

But when I add urea into water, neither is there and gas coming out as CO₂ or any decrease in the level of water
The urea just dissolved. 
How to stop this and make the reaction?

The reaction does happen, but it is very slow.
You can increase the rate of reaction with a suitable catalyst e.g.
https://en.wikipedia.org/wiki/Urease

[exchemist]

1 hour ago, observer1 said:

Urea - Wikipedia, go to automobile systems

Aha, I see. But this is at very high temperatures. In fact, a moment's thought should tell you the reaction won't go at room temperature, because in this system the urea is a supplied as a solution in water. So obviously that is fairly stable. Regarding the kinetics, I imagine you won't need a catalyst if the solution is sprayed into the combustion chamber, or into hot exhaust, at >500C. (Enzyme catalysts would obviously be no use in such a situation anyway.) 

Also, this is a reaction in which 2 molecules react to generate 3 molecules. The entropy change for such processes tends to be favourable, so the reaction will be thermodynamically more favourable at higher temperatures. (ΔG = ΔH -TΔS)   

 

Edited January 13, 2023 by exchemist