How many grams of Nitric oxide are required to produce 145g of nitrogen in this reaction:
Al2O3(s)+6NO(g)---->5N2(g)+6H2o(l)
To determine the number of grams of nitric oxide required to produce 145g of nitrogen in the given reaction, we need to use stoichiometry.
The balanced equation is:
Al2O3(s) + 6NO(g) ---> 5N2(g) + 6H2O(l)
From the balanced equation, we can see that the ratio of nitric oxide (NO) to nitrogen (N2) is 6:5.
To calculate the number of grams of nitric oxide required, we can follow these steps:
Step 1: Determine the molar mass of nitrogen (N2).
The molar mass of N2 is:
2 atoms of nitrogen (N) × atomic mass of nitrogen = 2 × 14.01 g/mol = 28.02 g/mol
Step 2: Use the mole ratio from the balanced equation to convert grams of nitrogen (N2) to moles of nitric oxide (NO).
The molar ratio between NO and N2 is 6:5.
So, the calculation is:
(145 g N2) × (6 mol NO / 5 mol N2) × (30.01 g/mol NO) = 361.5 g NO
Therefore, approximately 361.5 grams of nitric oxide (NO) are required to produce 145 grams of nitrogen (N2) in the given reaction.
To determine the number of grams of Nitric oxide required to produce 145g of nitrogen in the given reaction, we first need to find the molar ratio between Nitric oxide (NO) and nitrogen (N2) in the balanced equation.
Looking at the balanced equation:
Al2O3(s) + 6NO(g) → 5N2(g) + 6H2O(l)
We can see that the coefficient of NO is 6 and the coefficient of N2 is 5. This means that 6 moles of NO are required to produce 5 moles of N2.
To calculate the amount of NO needed to produce 145g of N2, we need to follow these steps:
Step 1: Calculate the molar mass of N2
Nitrogen (N) has an atomic mass of approximately 14.01 g/mol.
Since N2 is a diatomic molecule, we multiply the atomic mass of nitrogen by 2:
Molar mass of N2 = 14.01 g/mol × 2 = 28.02 g/mol
Step 2: Convert the given mass of N2 to moles
Number of moles of N2 = Mass of N2 / Molar mass of N2
Number of moles of N2 = 145 g / 28.02 g/mol ≈ 5.179 moles
Step 3: Use the molar ratio to calculate the moles of NO
From the balanced equation, we determined that 6 moles of NO produce 5 moles of N2.
So, moles of NO = moles of N2 × (6/5) ≈ 5.179 moles × (6/5) ≈ 6.214 moles
Step 4: Convert moles of NO to grams
To convert moles to grams, we need to use the molar mass of NO.
The molar mass of NO = Atomic mass of Nitrogen (N) + Atomic mass of Oxygen (O)
The atomic masses are approximately 14.01 g/mol for N and 16.00 g/mol for O.
Molar mass of NO = (14.01 g/mol + 16.00 g/mol) ≈ 30.01 g/mol
Grams of NO = Moles of NO × Molar mass of NO
Grams of NO = 6.214 moles × 30.01 g/mol ≈ 186.58 g
Therefore, approximately 186.58 grams of Nitric oxide (NO) would be required to produce 145 grams of nitrogen (N2) in the given reaction.
You have a stoichiometry problem. Here is a worked example that will work all of your stoichiometry problems. Just follow the steps.
http://www.jiskha.com/science/chemistry/stoichiometry.html