The answer is Boyle's law. Boyle's law states that the volume of a fixed mass of a gas is inversely proportional to its pressure at a constant absolute temperature.
That is; V α 1/P , at constant temperature and a fixed amount of the gas.
Such that V= k/P where k is a constant
The computation for molarity is:
(x) (0.175 L) = 0.0358 g / 598 g/mol
x = 0.000342093 M
Whereas the osmotic pressure calculation:
pi = iMRT
pi = (1) (0.000342093 mol/L) (0.08206 L atm / mol K) (298 K)
pi = 0.0083655 atm
Converting the answer to torr, will give us:
0.0083655 atm times (760 torr/atm) = 6.35778 torr
which rounds off to 6.36 torr
It's 18 (the same as the number of protons:)
<span>The partial pressure contributed to the overall pressure is proportional to the number of moles of gas particles. Both Neon and Argon are noble gases so there's just 1 atom per molecule. So let's determine how many moles of each we have:
Atomic weight neon = 20.1797
Atomic weight argon = 39.948
Moles neon = 10.0 g / 20.1797 g/mol = 0.495547506 mol
Moles argon = 10.0 g / 39.948 g/mol = 0.250325423 mol
So there's a total of 0.495547506 + 0.250325423 = 0.745872929 moles of gas particles. And for neon, it contributes 0.495547506/0.745872929 = 0.664385965 = 66.4385965% of them, so it contributes 66.4385965% of the total pressure. Which is 66.4385965% * 1.6 atm = 1.063017544 atm.
Rounding to 3 significant figures gives 1.06 atm, or 66.4% of the total pressure.</span>
I think it is heat and pressure
