How many moles of K₂S are consumed when 14.0 g of KBr react completely in the following equation? FeBr₂ + K₂S $\rarr$ 2KBr + FeS

Question

Quizplus · Accepted Answer

First, we need to balance the equation:

FeBr2 + 2KBr + FeS -> 2KBr + FeS2

From the balanced equation, we can see that 2 moles of KBr are required to produce 1 mole of FeS.

To find the number of moles of KBr consumed when 14.0 g of KBr are reacted, we need to use the molar mass of KBr:

molar mass of KBr = 119.0 g/mol

number of moles of KBr = mass/molar mass = 14.0 g/119.0 g/mol = 0.1176 mol

Since 2 moles of KBr are required to produce 1 mole of FeS, we can calculate the moles of FeS by dividing the number of moles of KBr by 2:

moles of KBr = 0.1176 mol
moles of FeS = 0.1176 mol/2 = 0.0588 mol

Therefore, the answer is A) 0.0588.

How Many Moles of K2S Are Consumed When 14 →\rarr→ 2KBr + FeS A)0