How many grams of Oxygen are needed to react with 100g of Nitrogen monoxide?
53.3g
To determine the number of grams of Oxygen needed to react with 100g of Nitrogen monoxide, we need to use the balanced chemical equation for the reaction.
The balanced equation for the reaction between Nitrogen monoxide (NO) and Oxygen (O2) is:
2NO + O2 → 2NO2
From the balanced equation, we can see that 2 moles of NO react with 1 mole of O2 to produce 2 moles of NO2.
1 mole of any substance is equal to its molar mass in grams. So, first, we need to determine the molar mass of Nitrogen monoxide (NO) and Oxygen (O2).
Nitrogen (N) has a molar mass of approximately 14.01 g/mol, and Oxygen (O) has a molar mass of approximately 16.00 g/mol. Therefore, the molar mass of Nitrogen monoxide (NO) is:
Molar mass of Nitrogen (N) + Molar mass of Oxygen (O)
= (14.01 g/mol) + (16.00 g/mol)
≈ 30.01 g/mol
Now, we can calculate the number of moles of Nitrogen monoxide (NO) in 100 grams. We'll use the formula:
moles = mass / molar mass
moles of NO = 100 g / 30.01 g/mol
≈ 3.33 mol
From the balanced equation, we know that 2 moles of NO react with 1 mole of O2. Therefore, the number of moles of O2 needed for the reaction can be calculated as:
moles of O2 = (2/1) * moles of NO
= (2/1) * 3.33 mol
≈ 6.67 mol
Finally, to find the mass of Oxygen (O2) needed, we multiply the number of moles of Oxygen by its molar mass:
mass of O2 = moles of O2 * molar mass of O2
The molar mass of Oxygen (O2) is approximately 32.00 g/mol. Therefore:
mass of O2 = 6.67 mol * 32.00 g/mol
≈ 213.44 g
Therefore, approximately 213.44 grams of Oxygen (O2) are needed to react with 100 grams of Nitrogen monoxide (NO).