The balance chemical equation is as follow,
2 Al + 3 O₂ → Al₂O₃
Aluminium is the Limiting Reagent,
As,
107.92 g Al required = 96 g of O₂
Then,
82.49 g of Al will require = X g of O₂
Solving for X,
X = (82.49 g × 96 g) ÷ 107.92 g
X = 73.37 g of O₂
But,
We are provided with 117.65 g of O₂, So, it is provided in excess and 44.28 g of it will remain unreacted.
Solving for Amount of Al₂O₃ formed,
As,
107.92 g of Al produced = 203.92 g of Al₂O₃
Then,
82.49 g of Al will produce = X g of Al₂O₃
SOlving for X,
X = (82.49 g × 203.92 g) ÷ 107.92
X = 155.86 g of Al₂O₃
primary,secondary,hereditary
Answer: The metal probably increases reaction rate by either holding reactant molecules in the correct orientation to react or by weakening or breaking bonds in reactant molecules to make them more reactive.
This is an example of heterogeneous catalysis.
Explanation: It is heterogeneous catalysis because the catalyst is a solid and the reactants are gases. In heterogeneous catalysis, the catalyst is in a different phase than the reactants.
Answer:
2.107×10²⁴
Explanation:
no of moles=no of particles/Avogadro's number
3.5=X/6.02×10²³
by cross multiplication
3.5×6.02×10²³
=2.107 ×10²⁴
Answer:
man ion even know but u fr struggling today huh?
Explanation:
