Elemental S reacts with O2 to form SO3 according to the reaction 2S+3O22SO3 as d

Question

Elemental S reacts with O2 to form SO3 according to the reaction

2S+3O22SO3

as depicted here.(Figure 1)

Part A

How many O2 molecules are needed to react with 3.91 g of S?

Express your answer numerically in units of molecules.

Part B

What is the theoretical yield of SO3 produced by the quantities described in Part A?

Express your answer numerically in grams.

Limiting reactant

Next, consider a situation in which all of the S is consumed before all of the O2reacts, or one in which you have excess S because all of the O2 has been used up.

Explanation / Answer

PART A

Avagadros number is need to calculate required molecules 6.023E-23

O2 required = (3.91 g. of S / 32.066 g per mole of S)*(3 oxygen molecule moles / 2 S moles)*(6.02E23 oxygen molecules / mole of oxygen molecules)

= 1.11016E23 O2 molecules

PART B

from the given reaction the ratio of S:O is 2:3

for 3.91g of S the moles is (3.91/32.066) = 0.1219

molecular weight of SO3 is 80---> 80g/mole

from part A we get 1.11016E23 O2 molecules required amount

so theoritical yield of SO3 is (0.1219mole * 80g/mole) = 9.752 gm

from part A calculation it is clear O2 is limiting reactant

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