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How many nitrogen molecules are contained in 1.00 L of nitrogen gas at 1.00 ATM and 298 K how many nitrogen atoms?
Wiki User
∙ 12y ago
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
Wiki User
∙ 12y ago
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