You could solve this in two ways: using the ideal gas law (Van der Waals parameters optional), or by using the density. Since you specify a pressure and temperature (in kelvin), I will use the ideal gas law.
Ideal gas law: PV=nRT
P = pressure = 1.00 ATM
V = volume = 1.00 L
n = moles = what you're solving for
R = gas constant = 0.0821 L*ATM/(mol*T) (T is absolute temperature (kelvin))
T = absolute temperature = 298 K
(1.00atm)(1.00L) = n(0.0821L*ATM*mol-1T-1)(298K)
n = 0.04 moles
An = Avogadro's Number = number of molecules in one mole = 6.022141 * 1023
0.04 * 6.022141*1023 = 2.409 * 1022 molecules of N2 in 1.00L at 1.00atm and 298K
This depends on the mass of nitrogen contained in the balloon.
Nitrogen is composed of molecules each containing two nitrogen atoms
5.418E23 molecules
In its natural state, nitrogen is diatomic and will form N2 (two bonded nitrogen atoms).
There are four nitrogen atoms in this compound (C8H10N4O2).
This depends on the mass of nitrogen contained in the balloon.
At standard temperature and pressure, nitrogen contains two atoms per molecule. Therefore 9 molecules contain 18 atoms.
Multiply 8.7 by avagadros number to get the number of molecules. 8.7x6.02x1023=5.24x1024 molecules of NO. as there is 1 atom of N and one of O for each molecule there are 5.24x1024 atoms of each element. this means that the total number of atoms is 2x5.24x1024 = 1.05x1025 atoms
At standard temperature and pressure, nitrogen exists in molecules with two atoms each.
Nitrogen is composed of molecules each containing two nitrogen atoms
NH3 is a molecule with 4 atoms in it, 1 nitrogen and three hydrogens.
There are 10 atoms in two nitric acid molecules. Namely they are two hydrogen atoms, two nitrogen atoms and six oxygen atoms.
3 x 12 = 36 moles of Nitrogen atoms N or 18 moles of Nitrogen molecules N2
Ammonia molecule: NH32 NH3 N2 + 3 H2Nitrogen molecule N2 , each molecule containing 2 atoms (of the element) N
3 i think N2O is the molecule, so that means within that molecule there is 2 nitrogen atoms and an oxygen atom
5.418E23 molecules
no of moles in aspartame =mass/molar mass=1.2/294=0.00408mols no of molecules=0.00408* avagadros no.=0.00408*6.022*10^23=0.02456*10^23 no. of atoms =no.of molecules*2(coz 2 atoms of nitrogen are present)=0.02456*10^23*2