In the equation N2 + 2 O2 → 2 NO2, 14 g of nitrogen can produce how many grams of nitrogen dioxide?
mols N2 = grams/molar mass = 14/28 = 0.5
Using the coefficients in the balanced equation, convert mols N2 to mols NO2.
That's 0.5 mol N2 x (2 mols NO2/1 mol N2) = 0.5 x 2/1 = 1 mol NO2
Now convert mols NO2 to grams. g = mols x molar mass = 1 mol x 46 = 46 grams NO2
To calculate the grams of nitrogen dioxide (NO2) produced from 14 grams of nitrogen (N2), we need to determine the molar ratio between nitrogen and nitrogen dioxide in the balanced equation.
1. Calculate the molar mass of nitrogen (N2):
The molar mass of nitrogen is 28 g/mol since nitrogen has an atomic mass of 14 g/mol and there are 2 nitrogen atoms in 1 molecule of nitrogen gas (N2).
2. Determine the molar ratio between nitrogen (N2) and nitrogen dioxide (NO2):
From the balanced equation N2 + 2 O2 → 2 NO2, we can see that for every 1 mole of nitrogen (N2) that reacts, 2 moles of nitrogen dioxide (NO2) are produced.
3. Calculate the moles of nitrogen (N2) in 14 grams:
To find the number of moles, we divide the given mass by the molar mass:
moles of N2 = mass of N2 / molar mass of N2
moles of N2 = 14 g / 28 g/mol
moles of N2 = 0.5 mol
4. Calculate the moles of nitrogen dioxide (NO2) produced:
Since the molar ratio between N2 and NO2 is 1:2, we can determine the moles of NO2:
moles of NO2 = moles of N2 * (2 mol NO2 / 1 mol N2)
moles of NO2 = 0.5 mol * (2 mol NO2 / 1 mol N2)
moles of NO2 = 1 mol
5. Calculate the mass of nitrogen dioxide (NO2) produced:
To find the mass, we multiply the moles of NO2 by the molar mass of NO2:
mass of NO2 = moles of NO2 * molar mass of NO2
mass of NO2 = 1 mol * (46 g/mol - molar mass of NO2)
mass of NO2 = 46 g
Therefore, 14 grams of nitrogen can produce 46 grams of nitrogen dioxide.
To determine how many grams of nitrogen dioxide (NO2) can be produced from 14 g of nitrogen (N2), we need to use the given chemical equation: N2 + 2 O2 → 2 NO2.
First, we need to find the molar masses of nitrogen (N2) and nitrogen dioxide (NO2). The molar mass of an element or compound is the mass of one mole of that substance.
The molar mass of nitrogen (N2) can be calculated by adding up the molar masses of two nitrogen (N) atoms:
N2: 2 × M(N) = 2 × 14.01 g/mol = 28.02 g/mol.
The molar mass of nitrogen dioxide (NO2) can be calculated by adding up the molar masses of one nitrogen (N) atom and two oxygen (O) atoms:
NO2: M(N) + 2 × M(O) = 14.01 g/mol + 2 × 16.00 g/mol = 46.01 g/mol.
Next, we can use the molar masses to calculate the number of moles of nitrogen (N2) in 14 g:
Number of moles = Mass / Molar mass
Number of moles of N2 = 14 g / 28.02 g/mol = 0.499 mol.
According to the balanced equation, for every 1 mole of N2, 2 moles of NO2 are produced. Therefore, the number of moles of NO2 can be calculated as:
Number of moles of NO2 = Number of moles of N2 × (2 moles of NO2 / 1 mole of N2)
Number of moles of NO2 = 0.499 mol × (2 mol / 1 mol) = 0.998 mol.
Finally, we can calculate the mass of nitrogen dioxide (NO2) produced using the number of moles and the molar mass:
Mass of NO2 = Number of moles of NO2 × Molar mass of NO2
Mass of NO2 = 0.998 mol × 46.01 g/mol = 45.93 g.
Therefore, 14 g of nitrogen can produce approximately 45.93 grams of nitrogen dioxide.