A chemist combine did 3.50g of potassium level with chlorine gas to yield 6.6 7g of potassium for it. Assuming all the potassium was consumed, and that potassium chloride was the only product that formed, what mass of chlorine reacted?

mass of chlorine reacted is 3.18 g

Explanation:

2 K + Cl2 = 2KCl

no. of moles of K = mass / molar mass

= 3.50 / 39

= 0.0897

no. of moles of KCl = mass / molar mass

= 6.67 / 74.5

= 0.0895  

no. of moles of Cl2 required = number of moles of KCl / 2

= 0.0895 / 2

= 0.0448 moles  

mass of Cl2 required = no. of moles of Cl2 required x molar mass

= 0.0448 x 71

= 3.1808 g ≈ 3.18 g

Therefore mass of chlorine reacted is 3.18 g

increased stability in the completion of fluorine's outer shell.

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