Question

Calculate the moles of potassium sulfide formed when 5.4g of potassium gas reacts with excess sulfur.

2 K+S > K2S

Answer 1

Ans:-

Reaction :

$2 K+S \leftrightarrow K_2S$

We have $5.4 g$ of Potassium firstly find its mole

mole of potassium$=\dfrac{5.4}{39}=0.138$ mole

from the reaction we clearly seen that

According to stoichiometry $2$ mole of potassium formed $1$ mole of potassium sulfide.

$2$ mole of potassium produced = $1$ mole of potassium sulfide

$0.138$ mole of potassium formed =$\dfrac{1}{2}\times0.138=0.276$ mole

$\therefore$ $0.276$ moles of potassium sulfide produced by $5.4$ gof potassium