Question

5. Use the principle of stoichiometry to determine the amount of oxygen that is required to convert Glucose (C6H12O6) to CO2 and H2O

a. Write a properly balanced overall reaction

b. Calculate the mass of O2 required to complete oxidize 1 g of acetone.

Answer 1

Step-by-step explanation:

(a) When oxidation of glucose occurs the glucose molecules react with oxygen and it results in the formation of carbon dioxide and water.

And, when in a chemical reaction equation number of atoms on the reactant side are equal to the number of atoms on product side then it is known as a balanced equation.

For example,
`C_(6)H_(12)O_(6) + O_(2) \rightarrow CO_(2) + H_(2)O`

Number of atoms on reactant side are as follows.

C = 6

H = 12

O = 8

Number of atoms on product side are as follows.

C = 1

H = 2

O = 3

Therefore, balance this equation by multiplying
`O_(2)` by 6 on reactant side. Also, on reactant side multiply
`CO_(2)` by 6 and
`H_(2)O` by 6.

Hence, the balanced equation is as follows.

`C_(6)H_(12)O_(6) + 6O_(2) \rightarrow 6CO_(2) + 6H_(2)O`

(b) According to the reaction equation, to completely oxidize 1 mole of glucose we need 6 mole of
`O_(2)`.

Therefore, to completely oxidize 180 g of glucose we need,
`6 * 32 g` of
`O_(2)`.

So, calculate the the amount of
`O_(2)` required to completely oxidize 1 g of glucose as follows.

`(6 * 32 g)/(180 g)` g of
`O_(2)`

= 1.07 g

Thus, we can conclude that the mass of
`O_(2)` required to completely oxidize 1 g of glucose is 1.07 g.