Question

Equal volume of N2 and H2 react to form ammonia under suitable condition then the limiting reagent is N2 , H2 or no one?? Please explain the answer NO copy paste please Best one will be marked as brainlist

Answer 1

Answer:

N2 + 3H2 => 2NH3

As clearly visible from the stoichiometric co-efficients of the reactants,

1 volume of N2 reacts with 3 volumes of H2

So, as per the given data, N2 and H2 are given in same amount but only ⅓rd of N2 will react with the given volume of H2

So,

• H2 is limiting reagent

• N2 is given in excess

this is the most important part of mole concept

i hope this helps u

Answer 2

Answer:

When equal volume of \mathrm{N}_{2} \text { and } \mathrm{H}_{2}N

2

and H

2

react, the limiting reagent is \mathrm{H}_{2}H

2

.

Explanation:

A limiting reagent or a limiting reactant is that substance in a chemical reaction that gets completely consumed when a reaction is complete. It is important to identify a limiting reagent in a chemical reaction so that the amount of the product obtained can be calculated.

When equal quantities of \mathrm{N}_{2} \text { and } \mathrm{H}_{2}N

2

and H

2

react, we get the balanced equation as given below:

\mathrm{N}_{2}+3 \mathrm{H}_{2} \rightarrow 2 \mathrm{NH}_{3}N

2

+3H

2

→2NH

3

According to mole ratio, 1 mole of N_2N

2

needs 3 moles of H_2H

2

to form 2 moles of ammonia.

We are given that N_2N

2

and H_2H

2

are in equal quantities and so for every N_2N

2

only 1 mole of H_2H

2

is provided whereas 3 moles of H_2 are required to fully react.

This means that there is not enough H_2H

2

to react with the given quantity of N_2N

2

and so H_2H

2

is limiting reagent