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Sagot :
Answer:
0.1876g
Explanation:
Since iron is in excess, therefore Magnesium is the limiting reactant.
Moles of Mg = mass/molar mass
0.120/24 = 0.005 moles
Compare the coefficient ratio of Mg and iron.
Ratio is 3 : 2
To find moles of iron we take 2/3 x 0.005
Moles of iron is 0.00335 moles
Mass = moles x molar mass
= 0.00335 x 56
= 0.1876g
Taking into account the reaction stoichiometry, 0.186 grams of Fe are produced when 0.120 g of magnesium reacts with excess iron chloride solution.
Reaction stoichiometry
In first place, the balanced reaction is:
3 Mg+ 2 FeCl₃ → 2 Fe+ 3 MgCl₂
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:
- Mg: 3 moles
- FeCl₃: 2 moles
- Fe: 2 moles
- MgCl₂: 3 moles
The molar mass of the compounds is:
- Mg: 24 g/mole
- FeCl₃: 162.35 g/mole
- Fe: 56 g/mole
- MgCl₂: 94.9 g/mole
Then, by reaction stoichiometry, the following mass quantities of each compound participate in the reaction:
- Mg: 3 moles ×24 g/mole= 72 grams
- FeCl₃: 2 moles ×162.35 g/mole= 324.7 grams
- Fe: 2 moles ×56 g/mole= 112 grams
- MgCl₂: 3 moles ×94.9 g/mole= 284.7 grams
Mass of iron produced
The following rule of three can be applied: if by reaction stoichiometry 72 grams of Mg form 112 grams of Fe, 0.120 grams of Mg form how much mass of Fe?
[tex]mass of Fe=\frac{0.120 grams of Mgx112 grams of Fe}{72 grams of Mg}[/tex]
mass of Fe= 0.186 grams
Then, 0.186 grams of Fe are produced when 0.120 g of magnesium reacts with excess iron chloride solution.
Learn more about the reaction stoichiometry:
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