calculate the number of grams of nitrogen dioxide that are produced from 2 moles of nitric oxide
2NO(g)+Osub2(g)---->2NOsub2(g)
You don't need to write in the sub part. It isn't ideal but those who use these boards know that KNO3 is KNOsub3. If we want it to be a superscript, we write KNO^3.
2 moles NO [rpdice 2 moles NO2; therefore, 2 moles NO is
2 x molar mass = grams.
To calculate the number of grams of nitrogen dioxide produced from 2 moles of nitric oxide, we need to use the balanced chemical equation, molar masses, and stoichiometry.
The balanced equation given is:
2NO(g) + O2(g) → 2NO2(g)
First, we need to determine the molar masses of nitric oxide (NO) and nitrogen dioxide (NO2):
- Nitric oxide (NO) has a molar mass of approximately 30.01 grams/mole.
- Nitrogen dioxide (NO2) has a molar mass of approximately 46.01 grams/mole.
Now, let's use the stoichiometry of the balanced equation to find the molar ratio between nitric oxide (NO) and nitrogen dioxide (NO2):
From the balanced equation, we see that 2 moles of nitric oxide (NO) are required to produce 2 moles of nitrogen dioxide (NO2).
Finally, we can calculate the grams of nitrogen dioxide produced:
1. Calculate the moles of nitrogen dioxide (NO2) produced by multiplying the moles of nitric oxide (NO) by the molar ratio:
Moles of NO2 = Moles of NO × (2 moles of NO2 / 2 moles of NO)
Since we have 2 moles of nitric oxide (NO):
Moles of NO2 = 2 moles of NO × (2 moles of NO2 / 2 moles of NO) = 2 moles of NO2
2. Convert the moles of nitrogen dioxide (NO2) to grams using the molar mass of NO2:
Grams of NO2 = Moles of NO2 × Molar mass of NO2
Since the molar mass of NO2 is approximately 46.01 grams/mole:
Grams of NO2 = 2 moles of NO2 × 46.01 grams/mole = 92.02 grams of NO2
Therefore, 2 moles of nitric oxide would produce 92.02 grams of nitrogen dioxide.