Question

Given the following equation, what is the correct form of the conversion factor needed to convert the number of moles of O₂ to the number of moles of Fe₂O₃ produced? 4Fe(s) + 3O₂ (g)
`\rightarrow` 2Fe₂O₃(s)
`a. (2 moles of Fe_2O_3)/(4 moles of Fe)\\b. (4 moles of Fe)/(3 moles of O_2)\\c. (2 moles of Fe_2O_3)/(3 moles of O_2)\\d. (4 moles of Fe)/(2 moles of Fe_2O_3)\\e. (3 moles of O_2)/(2 moles of Fe_2O_3)`

Answer 1

E

Step-by-step explanation:

The question deals with the stoichiometry of the conversion of the number of moles of oxygen to the number of moles of iron III oxide.

Since three moles of oxygen yields two moles of iron III oxide according to the balanced reaction equation, it then follows that 3/2 moles of oxygen will give the number of moles of iron III oxide produced in the reaction. Hence the answer.

Answer 2

Answer : The correct option is (c)
`\frac{2\text{ mole of }Fe_2O_3}{3\text{ mole of }O_2}`

Explanation :

The given balanced chemical reaction is,

`4Fe(s)+3O_2(g)\rightarrow 2Fe_2O_3(s)`

From the balanced chemical reaction, we conclude that

As, 3 moles of
`O_2` react to give 2 mole of
`Fe_2O_3`

So, 1 mole of
`O_2` react to give
`\frac{2\text{ mole of }Fe_2O_3}{3\text{ mole of }O_2}` moles of
`Fe_2O_3`

Thus, the conversion factor needed to convert the number of moles of
`O_2` to the number of moles of
`Fe_2O_3` produced is
`\frac{2\text{ mole of }Fe_2O_3}{3\text{ mole of }O_2}`

Hence, the correct option is (c)
`\frac{2\text{ mole of }Fe_2O_3}{3\text{ mole of }O_2}`