Answer to Question #189224 in General Chemistry for Tyler Drotning

Question

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

2 K+S > K2S

Answer 1

Reaction :

$2 K+S \leftrightarrow K_2S$

We have 5.4 g5.4g of Potassium firstly find its mole

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

from the reaction we clearly seen that

According to stoichiometry 22 mole of potassium formed 11 mole of potassium sulfide.

22 mole of potassium produced = 11 mole of potassium sulfide

0.1380.138 mole of potassium formed $=\dfrac{1}{2}\times0.138=0.276$

Therefore∴ 0.276 moles of potassium sulfide produced by 5.45gof potassium