If 34.7 g of O2 reacts with iron to form 79.34 g of iron oxide, how much iron was used in the reaction? A.

19.84 g

B.

44.64 g

C.

104.1 g

D.

114.04 g

Question

Physics

Rayan Wong

9 January, 03:03

If 34.7 g of O2 reacts with iron to form 79.34 g of iron oxide, how much iron was used in the reaction? A.

19.84 g

B.

44.64 g

C.

104.1 g

D.

114.04 g

+2

Answers (1)

Know the Answer?

Darren Gilmore · Answer 1

Answer: B. 44.64 g

Explanation:

According to the law of conservation of mass, mass can neither be created nor be destroyed. Thus the mass of products has to be equal to the mass of reactants. The number of atoms of each element has to be same on reactant and product side. Thus chemical equations are balanced.

Mass of reactants = mass of iron + mass of oxygen = mass of iron + 34.7 g

Mass of product = mass of iron oxide = 79.34 g

As Mass of reactants = Mass of product

mass of iron + 34.7 g = 79.34 g

mass of iron = 44.64 g

Thus 44.64 g of iron was used in the reaction

If 34.7 g of O2 reacts with iron to form 79.34 g of iron oxide, how much iron was used in the reaction? A.19.84 gB.44.64 gC.104.1 gD.114.04 g

If 34.7 g of O2 reacts with iron to form 79.34 g of iron oxide, how much iron was used in the reaction? A.

19.84 g

B.

44.64 g

C.

104.1 g

D.

114.04 g