How many O2 molecules are needed to react with 4.59 g of S?in 2S ＋3O2→2SO3

Elemental S reacts with O2 to form SO3 according to the reaction 2S+3O2→2SO3 Part B: What is the theoretical yield of SO3 produced by the quantities described in Part A? Express your answer numerically in grams.

Part A: 1.88x10^23 O2 molecules are needed to react with 6.67 g of S.

We address the equation...

S

(

s

)

+

3

2

O

2

(

g

)

→

S

O

3

(

g

)

Explanation:

The question specifies that we got

1.88

×

10

23

dioxygen molecules

...i.e. a molar quantity of...

1.88

×

10

23

⋅

molecules

6.022

×

10

23

⋅

molecules

⋅

m

o

l

−

1

=

0.312

⋅

m

o

l

...

But we gots with respect to sulfur,

6.67

⋅

g

32.06

⋅

g

⋅

m

o

l

−

1

=

0.208

⋅

m

o

l

...

And a bit of arithmetic later, we establish that we got stoichiometric quantities of dioxygen, and sulfur….in the reaction we produce a mass of ………..

0.208

⋅

m

o

l

×

80.07

⋅

g

⋅

m

o

l

−

1

=

16.65

⋅

g

.

Note that when

sulfur trioxide

is made industrially (and this a very important commodity chemical), sulfur is oxidized to

S

O

2

, and this is then oxidized up to

S

O

3

with some catalysis...

S

O

2

(

g

)

+

1

2

O

2

(

g

)

V

2

O

5

−−→

S

O

3

(

g

)

S

O

3

(

g

)

+

H

2

O

(

l

)

→

H

2

S

O

4

(

a

q

)



sulfuric acid

The industrial sulfur cycle must be a dirty, smelly, unfriendly process. The process is undoubtedly necessary to support our civilization

can you list the answers so i can answer