Using the following thermochemical data, what is the change in enthalpy for the following reaction: 3H2(g) + 2C(s) + ½O2(g) C2H5
1 answer:
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<u>Answer:</u> The limiting reactant is magnesium and mass of excess reactant present in the vessel is 96.35 grams.
<u>Explanation:</u>
To calculate the number of moles, we use the equation:
.....(1)
- <u>For magnesium:</u>
Given mass of magnesium = 41.0 g
Molar mass of magnesium = 24 g/mol
Putting values in equation 1, we get:
- <u>For iron(III) chloride:</u>
Given mass of iron(III) chloride = 175.0 g
Molar mass of iron(III) chloride = 162.2 g/mol
Putting values in equation 1, we get:
The chemical equation for the reaction of magnesium and iron(III) chloride follows:
By Stoichiometry of the reaction:
3 moles of magnesium reacts with 2 moles of iron(III) chloride
So, 1.708 moles of magnesium will react with = of iron(III) chloride
As, given amount of iron(III) chloride is more than the required amount. So, it is considered as an excess reagent.
Thus, magnesium is considered as a limiting reagent because it limits the formation of product.
Moles of excess reactant left (iron(III) chloride) = [1.708 - 1.114] = 0.594 moles
Now, calculating the mass of iron(III) chloride from equation 1, we get:
Molar mass of iron(III) chloride = 162.2 g/mol
Moles of iron(III) chloride = 0.594 moles
Putting values in equation 1, we get:
Hence, the limiting reactant is magnesium and mass of excess reactant present in the vessel is 96.35 grams.