will the following reaction take place nh3+h2o= nh2 + h3o
It forms NH4^+ + OH^-
The reaction you have provided is not balanced correctly. Let's balance it first:
NH3 + H2O → NH2 + H3O+
Now, let's check if this reaction will occur. To determine if a chemical reaction will occur, we need to consider the reactants' and products' chemical properties and conditions such as temperature, pressure, and catalysts.
In this case, unless there are specific conditions, such as high temperature or the presence of a catalyst, the reaction between NH3 (ammonia) and H2O (water) to form NH2 (amide) and H3O+ (hydronium ion) is unlikely to occur.
Generally, ammonia (NH3) tends to react with water (H2O) to form ammonium hydroxide (NH4OH) through the following reaction:
NH3 + H2O → NH4OH
It is more common for ammonia to act as a base and accept a proton (H+) from water, forming ammonium hydroxide (NH4OH) rather than forming an amide (NH2) and hydronium ion (H3O+).
To determine whether a reaction will take place, we need to consider the relative reactivity of the reactants and the feasibility of the chemical transformation.
In this case, the reaction you've given is not balanced and seems to involve the transfer of a hydrogen atom. This is known as a proton transfer or acid-base reaction.
First, let's balance the equation:
NH3 + H2O → NH2 + H3O+
Now, let's analyze the reaction. NH3 (ammonia) can act as a base and accept a proton (H+) from H2O (water), which acts as an acid. This results in the formation of NH2- (amidide ion) and H3O+ (hydronium ion).
In water, the equilibrium between NH3 and NH2- is shifted towards NH3, as NH2- can react with water to form NH3 and OH-. Similarly, the equilibrium between H2O and H3O+ is shifted towards H2O because H3O+ can react with water, producing H2O and H3O+.
So, based on this information, the reaction NH3 + H2O → NH2 + H3O+ can take place. However, it is important to note that whether this reaction occurs to a significant extent depends on the specific concentration and conditions of the reactants.