The picture explains it.
1 answer:
You might be interested in
Taking into account the reaction stoichiometry, 0.2066 grams of CO₂ are formed from 0.500 grams of iron oxide and an excess of carbon.
<h3>Reaction stoichiometry</h3>In first place, the balanced reaction is:
2 Fe₂O₃ + 3 C → 4 Fe + 3 CO₂
By reaction stoichiometry (that is, the relationship between the amount of reagents and products in a chemical reaction), the following amounts of moles of each compound participate in the reaction:
- Fe₂O₃: 2 moles
- C: 3 moles
- Fe:4 moles
- CO₂: 3 moles
The molar mass of the compounds is:
- Fe₂O₃: 159.7 g/mole
- C: 12 g/mole
- Fe: 55.85 g/mole
- CO₂: 44 g/mole
Then, by reaction stoichiometry, the following mass quantities of each compound participate in the reaction:
- Fe₂O₃: 2 moles ×159.7 g/mole= 319.4 grams
- C: 3 moles ×12 g/mole= 36 grams
- Fe: 4 moles ×55.85 g/mole= 223.4 grams
- CO₂: 3 moles ×44 g/mole= 132 grams
The following rule of three can be applied: if by reaction stoichiometry 319.4 grams of Fe₂O₃ form 132 grams of CO₂, 0.500 grams of Fe₂O₃ form how much mass of CO₂?
<u><em>mass of CO₂= 0.2066 grams</em></u>
Then, 0.2066 grams of CO₂ are formed from 0.500 grams of iron oxide and an excess of carbon.
Learn more about the reaction stoichiometry:
#SPJ1