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Given the following equation: 8 Fe + S8 → 8 FeS

a) What mass of iron is needed to react with 16.0 moles of sulfur?

7148.16 grams of iron

b) How many moles of FeS are produced?

a) answered

b) 128 moles FeS

Step-by-step explanation:

b) 16 moles of S8, original equation multiplied by 16

8 moles of FeS originally, multiplied by 16=128

a) 1 mole of S reacts with 8 moles of Fe

16 mole of S reacts with 128 moles of Fe

128 moles of Fe = 55.8 × 128 gm = 7142.4 gm (approx)

b) 8 moles of Fe reacts with 1 mole S to form 8 moles of FeS

128 moles of Fe reacts with 16 moles of S to form 128 moles of FeS

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it's equivalent, so we can say that its equal.

let's call the denominator x and the numerador is 18 less then denominator, x - 18.

multiply

2.x = 5.(x - 18)

2x = 5x - 90

90 = 5x - 2x

90 = 3x

x = 90/3

x = 30

so:

d

step-by-step explanation: