Answer the questions about the following reaction.
4Al(s) + 3O2(g) 2Al2O3 (s)
How many molecules of O2 are used in the reaction?
How many oxygen atoms are required?
How many moles of Al2O3 are formed?
What is the mole ratio of Al to O2?
for the first three, one wonders. How much (in grams, moles, or else) was invovled in the reaction? 1gram, or 200 tons?
mole ratio of Al to O2: 4::3
1. 3 mols of O2 * 6.022*10^23
1mol
so 3*6.022*10^23= 1.8066*10^24
molecules of O2
2. 3O2 2atoms*3moles=6
2Al2O3 3atoms*2moles=6
6+6= 12 total O atoms
3. 4 moles of Al for every 3 moles of
O2= 4:3 mole to mole ratio
To answer these questions, we need to use the balanced equation for the reaction:
4Al(s) + 3O2(g) → 2Al2O3(s)
1. How many molecules of O2 are used in the reaction?
From the balanced equation, we can see that for every 3 molecules of O2 that react, we form 2 molecules of Al2O3. Therefore, for every 2 molecules of Al2O3, we need 3 molecules of O2.
2. How many oxygen atoms are required?
In each molecule of O2, there are 2 oxygen atoms. So, if we have 3 molecules of O2, we have 3 x 2 = 6 oxygen atoms.
3. How many moles of Al2O3 are formed?
From the balanced equation, we can see that for every 4 moles of Al that react, we form 2 moles of Al2O3. Therefore, the mole ratio of Al2O3 to Al is 2:4, which simplifies to 1:2. So, if we have 4 moles of Al, we will form 2 moles of Al2O3.
4. What is the mole ratio of Al to O2?
From the balanced equation, we can see that for every 4 moles of Al that react, we require 3 moles of O2. Therefore, the mole ratio of Al to O2 is 4:3.
To answer these questions, we can break down the balanced chemical equation and use stoichiometry, which is the calculation of the quantities of reactants and products in a chemical reaction.
1. Question: How many molecules of O2 are used in the reaction?
To determine the number of molecules of O2 used, we can refer to the balanced chemical equation. It states that 4 moles of aluminum (Al) react with 3 moles of oxygen (O2) to produce 2 moles of aluminum oxide (Al2O3).
From the equation, we can infer that for every 4 moles of Al, we need 3 moles of O2. Since 1 mole contains 6.022 x 10^23 molecules (Avogadro's number), we can use this conversion factor to find the number of molecules of O2.
Therefore, to calculate the number of O2 molecules used, we multiply the number of moles of O2 by Avogadro's number:
3 moles O2 x (6.022 x 10^23 molecules/mole) = 1.807 x 10^24 molecules of O2
So, there are approximately 1.807 x 10^24 molecules of O2 used in the reaction.
2. Question: How many oxygen atoms are required?
Each molecule of O2 consists of two oxygen atoms, so to determine the number of oxygen atoms required, we multiply the number of molecules of O2 by 2:
1.807 x 10^24 molecules of O2 x 2 atoms of O per molecule = 3.614 x 10^24 oxygen atoms
Therefore, approximately 3.614 x 10^24 oxygen atoms are required.
3. Question: How many moles of Al2O3 are formed?
According to the balanced chemical equation, the stoichiometric ratio is 2 moles of Al2O3 for every 4 moles of Al. This means that the number of moles of Al2O3 formed will be half of the number of moles of Al used.
If we have the number of moles of Al used, we can divide it by 4 and multiply by 2 to find the moles of Al2O3 formed. However, since the question doesn't provide the number of moles of Al used, we cannot determine the exact amount of Al2O3 formed.
4. Question: What is the mole ratio of Al to O2?
The balanced chemical equation tells us that the mole ratio of Al to O2 is 4:3. This means that for every 4 moles of Al, we need 3 moles of O2 to react fully.