A) Iron(II) sulfide reacts with hydrochloric acid according to the reaction: FeS

Question

A) Iron(II) sulfide reacts with hydrochloric acid according to the reaction:
FeS(s)+2HCl(aq)FeCl2(s)+H2S(g)
A reaction mixture initially contains 0.250 mol FeSand 0.650 mol HCl.

Once the reaction has occurred as completely as possible, what amount (in moles) of the excess reactant is left?

B) Elemental phosphorus reacts with chlorine gas according to the equation:
P4(s)+6Cl2(g)4PCl3(l)
A reaction mixture initially contains 45.97 g P4 and 130.8 g Cl2.

Once the reaction has occurred as completely as possible, what mass (in g) of the excess reactant is left?

Explanation / Answer

FeS(s)+2HCl(aq)FeCl2(s)+H2S(g)

1 mole FeS reacts with 2 moles HCl

0.25 mole FeS reacts with 0.25 x 2 / 1 = 0.5 moles HCl

exess HCl left = 0.65 - 0.5 = 0.15 moles

B) P4(s)+6Cl2(g)4PCl3(l)

123.9 g P4 reats with 6 x 71 g Cl2

X g P4 reacts with 130.8 g Cl2

X = (130.8 x 123.9 / 6 x 71) = 16206.12 / 426

X = 38.04 g P4

exess P4 left = 45.97 - 38.04 = 7.93 g

exess reactant left = 7.93 g

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