<u>Answer:</u> The mass of excess reagent (ammonium chloride) remained after the reaction is 62.7 grams
<u>Explanation:</u>
To calculate the number of moles, we use the equation:
.....(1)
- <u>For aluminium nitrite:</u>
Given mass of aluminium nitrite = 27.4 g
Molar mass of aluminium nitrite = 41 g/mol
Putting values in equation 1, we get:
- <u>For ammonium chloride:</u>
Given mass of ammonium chloride = 169.9 g
Molar mass of ammonium chloride = 53.5 g/mol
Putting values in equation 1, we get:
The chemical equation for the reaction of aluminium nitrite and ammonium chloride follows:
By Stoichiometry of the reaction:
1 mole of aluminium nitrite reacts with 3 moles of ammonium chloride
So, 0.668 moles of aluminium nitrite will react with = of ammonium chloride.
As, given amount of ammonium chloride is more than the required amount. So, it is considered as an excess reagent.
Thus, aluminium nitrite is considered as a limiting reagent because it limits the formation of product.
Excess moles of ammonium chloride = (3.176 - 2.004) mol = 1.172 moles
Calculating the mass of ammonium chloride by using equation 1, we get:
Excess moles of ammonium chloride = 1.172 moles
Molar mass of ammonium chloride = 53.5 g/mol
Putting values in equation 1, we get:
Hence, the mass of excess reagent (ammonium chloride) remained after the reaction is 62.7 grams