Question

If 15 grams of Carbon dioxide is produced in a chemical reaction, how many grams of Carbon must be consumed in the reaction if we know there were 11 grams of Oxygen on the reactants side of the equation?

Answer 1

4.13 g

Step-by-step explanation:

Data Given:

Amount of CO₂ Produced = 15 g

Amount of Oxygen = 11 g

Amount of Carbon used = ?

Solution:

Suppose Carbon dioxide (CO₂) is formed by the reaction of carbon and oxygen then the reaction will be as below

C + O₂ -------------> CO₂

1 mol 1 mol 1 mol

we come to know from the above reaction that

1 mole of carbon react with 1 mole of oxygen to produce 1 mol of carbon dioxide.

molar mass of C = 12 g/mol

molar mass of O₂ = 32 g/mol

molar mass of CO₂ = 12 + 2(16) = 44 g/mol

if we represent mole in grams then

C + O₂ -------------> CO 1 mol (12 g/mol) 1 mol (32 g/mol) 1 mol (44 g/mol)

C + O₂ -------------> CO₂

12 g 32 g 44 g

So,

we come to know that 32 g of Oxygen combine with 12 g of oxygen produce 44 g CO₂

So now how much of Carbon will be combine with 11 g of oxygen

apply unity formula

32 g of O₂ ≅ 12 g of C

11 g of O₂ ≅ g of C

by doing cross multiplication

g of C = 12 g x 11 g / 32 g

g of C = 132 g / 32 g

g of C = 4.13 g

So,

4.13 g of carbon will consume to produce 15 g of Carbon dioxide.

to check this answer

we use the above information

12 g of C ≅ 44 g of CO₂

4.13 g of C ≅ g of CO₂

by doing cross multiplication

g of CO₂ = 44 g x 4.13 g / 12 g

g of CO₂ = 15g

So it is confirmed that

4.13 g of carbon will consume to produce 15 g of Carbon dioxide.