Question

Potassium and nitrogen react in a combination reaction to produce potassium nitride: 6 K(s)+N2(g) → 2 K3N(s) How many moles of potassium are needed to produce 12.0 mol of K3N when the reaction is carried out in the presence of excess nitrogen?

Answer 1

Moles of potassium needed = 36 moles

Step-by-step explanation:

Moles of
`K_3N` produced = 12.0 mol

According to the given reaction:-

`6 K_((s))+N_2_((g))\rightarrow 2K_3N_((s))`

2 moles of
`K_3N` are produced when 6 moles of potassium undergoes reaction.

Also,

1 mole of
`K_3N` are produced when 6/2 moles of potassium undergoes reaction.

So,

12 mole of
`K_3N` are produced when 3*12 moles of potassium undergoes reaction.

Moles of potassium needed = 36 moles