Question

Calculate the grams of C6H6 needed to produce 25 g of CO2 Show your work

Answer 1

Answer:

The given reaction is a combustion reaction of benzene,

C

6

H

6

. From its balanced chemical equation,

2

C

6

H

6

+

15

O

2

→

12

C

O

2

+

6

H

2

O

,

the mass of carbon dioxide

(

C

O

2

)

produced from 20 grams (g) of

C

6

H

6

is determined through the molar mass of the two compounds, given by,

M

M

C

O

2

=

44.01

g

/

m

o

l

M

M

C

6

H

6

=

78.11

g

/

m

o

l

and their mole ratio:

12

m

o

l

C

O

2

2

m

o

l

C

6

H

6

→

6

m

o

l

C

O

2

1

m

o

l

C

6

H

6

With this,

m

a

s

s

o

f

C

O

2

=

(

20

g

C

6

H

6

)

(

1

m

o

l

C

6

H

6

78.11

g

C

6

H

6

)

(

6

m

o

l

C

O

2

1

m

o

l

C

6

H

6

)

(

44.01

g

C

O

2

1

m

o

l

C

O

2

)

=

(

20

)

(

6

)

(

44.01

)

g

C

O

2

78.11

=

5281.2

g

C

O

2

78.11

m

a

s

s

o

f

C

O

2

=

67.6

g

C

O

2

Therefore, the mass in grams of

C

O

2

formed from 20 grams of

C

6

H

6

is

67.6

g

C

O

2

.

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