Problem :

Solution for Problem 1 >>

×4 moles NH3(g) = 10.96 moles NH3(g)
×6 moles NO(g) = 16.44 moles NO(g)

So we have 10.96 moles NH₃(g) and 16.44 moles NO(g).

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Problem : What is the mass of 2 moles of H₂S ?

Solution for Problem 2 >>

GFM of H = 1
GFM of S = 32>br> GFM of H₂S = 2×1 + 32 = 34 grams / mole

×34 grams = 68 grams

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Problem : 2Al +3Cl₂→2AlCl₃

When 80 grams of aluminum is reacted with excess chlorine gas, how many formula units of AlCl₃ are produced?

Solution for Problem 3 >>

×1 mole Al = 2.96 moles Al

There is a 1:1 ratio between Al and AlCl₃ , therefore there are 2.96 moles AlCl₃ .

= 1.78×1025

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Problem : Sb₂S₃(s) + 3Fe(s)→2Sb(s) +3FeS(s)

If 3.87×10²³ particles of Sb₂S₃(s) are reacted with excess Fe(s), what mass of FeS(s) is produced?

Solution for Problem 4 >>

×1 mole Sb2S3(s) = 0.643 moles Sb2S3(s)
×3 moles FeS(s) = 1.93 moles FeS(s)
×88 grams = 170 grams

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Problem : CO(g) +2H₂(g)→CH₃OH(g)

At STP, what volume of H₂(g) is needed to react completely with 8.02×10²³ molecules of CO(g)?

Solution for Problem 5 >>

×1 mole CO(g) = 1.33 moles CO(g)
×2 moles H2(g) = 2.66 moles H2(g)
×22.4 L = 59.7 L

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