Henry Moseley organized the periodic table by A. atomic weight. B. atomic number. C. electronegativity. D. overall charge of ato
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Taking into account the reaction stoichiometry, 4.57 grams of H₂O are formed when8.63 grams of Al₂O₃ reacts with HNO₃.
<h3>Reaction stoichiometry</h3>In first place, the balanced reaction is:
Al₂O₃ + 6 HNO₃ → 2 Al(NO₃)₃ + 3 H₂O
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:
- Al₂O₃: 1 mole
- HNO₃: 6 moles
- Al(NO₃)₃: 2 moles
- H₂O: 3 moles
The molar mass of the compounds is:
- Al₂O₃: 102 g/mole
- HNO₃: 63 g/mole
- Al(NO₃)₃: 213 g/mole
- H₂O: 18 g/mole
Then, by reaction stoichiometry, the following mass quantities of each compound participate in the reaction:
- Al₂O₃: 1 mole ×102 g/mole= 102 grams
- HNO₃: 6 moles ×63 g/mole= 378 grams
- Al(NO₃)₃: 2 moles ×213 g/mole= 426 grams
- H₂O: 3 moles ×18 g/mole= 54 grams
The following rule of three can be applied: if by reaction stoichiometry 102 grams of Al₂O₃ form 54 grams of H₂O, 8.63 grams of Al₂O₃ form how much mass of H₂O?
<u><em>mass of H₂O= 4.57 grams</em></u>
Then, 4.57 grams of H₂O are formed when8.63 grams of Al₂O₃ reacts with HNO₃.
Learn more about the reaction stoichiometry:
<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