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Chapter 2: Problem 4

A 1.446 g sample of potassium reacts with 8.178 g of chlorine to produce potassium chloride as the only product. After the reaction, 6.867 g of chlorine remains unreacted. What mass of potassium chloride was formed?

Short Answer

Expert verified
The mass of potassium chloride formed is 2.757 g.

Step by step solution

01

Calculate the total weight of potassium and chlorine before the reaction

Add the weight of potassium and chlorine to find the total weight before the reaction:\(1.446 g (potassium) + 8.178 g (chlorine) = 9.624 g\)
02

Find the weight of chlorine that reacted

Subtract the weight of chlorine that remained unreacted from the total weight of chlorine before the reaction to find the weight of chlorine that reacted: \(8.178 g (chlorine initially) - 6.867 g (chlorine unreacted) = 1.311 g (chlorine that reacted)\)
03

Calculate the weight of produced potassium chloride

Add the weight of the reacted potassium and chlorine to find the weight of potassium chloride that was formed: \(1.446 g (potassium) + 1.311 g (chlorine) = 2.757 g\)

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