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A certain amount of glucose, C6H12O6 burned in oxygen, and produced 22 grams of carbon dioxide, CO2. How many grams of water was produced at the same time?

C6H12O6 (s) + 6O2(g) → 6CO2 (g) + 6H2O (g)

A.22 grams of H2O

B.11 grams of H2O

C.9 grams of H2O

D.4.5 grams of H2O

1 Answer

3 votes

Approximately

60

g of

C

6

H

12

O

6

.

Step-by-step explanation:

We have the balanced equation (without state symbols):

6

H

2

O

+

6

C

O

2

C

6

H

12

O

6

+

6

O

2

So, we would need six moles of carbon dioxide to fully produce one mole of glucose.

Here, we got

88

g

of carbon dioxide, and we need to convert it into moles.

Carbon dioxide has a molar mass of

44

g/mol

. So here, there exist

88

g

44

g

/mol

=

2

mol

Since there are two moles of

C

O

2

, we can produce

2

6

1

=

1

3

moles of glucose

(

C

6

H

12

O

6

)

.

We need to find the mass of the glucose produced, so we multiply the number of moles of glucose by its molar mass.

Glucose has a molar mass of

180.156

g/mol

. So here, the mass of glucose produced is

1

3

mol

180.156

g

mol

60

g

to the nearest whole number.

So, approximately

60

grams of glucose will be produced

User Rosebud
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