178.87 grams of sulphur dioxide is formed according to the equation given.
Explanation:
The balanced chemical reaction for the process is:
4 FeS2 + 11 O2 ⇒ 2Fe2O3(-) + 8 SO2
the reaction involving FeS and oxygen having balanced chemical equation as:
moles of oxygen given as 3.84
so when 11 moles of O2 reacts to form 8 moles SO2
3.84 moles of oxygen reacts to form x moles of SO2
= 
x = 
2.792 moles of sulphur dioxide will be formed
The mass can be calculated as number of moles x molar mass of 1 mole of SO2
= 2.792 x 64.066
= 178.87 grams of sulphur dioxide is formed.
Answer:
0.075 moles of iron oxide would be produced by complete reaction of 0.15 moles of iron.
Explanation:
The balanced reaction is:
4 Fe + 3 O₂ → 2 Fe₂O₃
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:
- Fe: 4 moles
- O₂: 3 moles
- Fe₂O₃: 2 moles
You can apply the following rule of three: if by stoichiometry 4 moles of Fe produce 2 moles of Fe₂O₃, 0.15 moles of Fe produce how many moles of Fe₂O₃?
moles of Fe₂O₃= 0.075
<u><em>0.075 moles of iron oxide would be produced by complete reaction of 0.15 moles of iron.</em></u>
Combustion usually occurs when a hydrocarbon reacts with oxygen to produce carbon dioxide and water. Combustion reactions are almost always exothermic CO(g) + ½O2(g) → CO2(g) + 67.6 kcal
base from the reaction, the stoichiometric ratio is 1 mole CO produce 67.6 kcal so the anwer is - 67.6 kcal because is it exothermic
