Agas cylinder of volume 5.00 l contains 1.00 g of ar and 0.500 g of ne. the temperature is 275 k. find the partial pressure of ne.

11.3 kPa The ideal gas law is PV = nRT where P = Pressure V = Volume n = number of moles R = Ideal gas constant (8.3144598 L*kPa/(K*mol) ) T = Absolute temperature We have everything except moles and volume. But we can calculate moles by starting with the atomic weight of argon and neon. Atomic weight argon = 39.948 Atomic weight neon = 20.1797 Moles Ar = 1.00 g / 39.948 g/mol = 0.025032542 mol Moles Ne = 0.500 g / 20.1797 g/mol = 0.024777375 mol Total moles gas particles = 0.025032542 mol + 0.024777375 mol = 0.049809918 mol Now take the ideal gas equation and solve for P, then substitute known values and solve. PV = nRT P = nRT/V P = 0.049809918 mol * 8.3144598 L*kPa/(K*mol) * 275 K/5.00 L P = 113.8892033 L*kPa / 5.00 L P = 22.77784066 kPa Now let's determine the percent of pressure provided by neon by calculating the percentage of neon atoms. Divide the number of moles of neon by the total number of moles. 0.024777375 mol / 0.049809918 mol = 0.497438592 Now multiply by the pressure 0.497438592 * 22.77784066 kPa = 11.33057699 kPa Round the result to 3 significant figures, giving 11.3 kPa

n N2(g) = 15.367 mol

Explanation:

airbags generally vary between 35 and 60 liters in volume and for the airbag system to activate, it takes about 20 Kgf/cm² of pressure; with this data taken from literature and knowing the temperature of reaction (495 °C), we determine the moles of nitrogen needed from the ideal gas law.

ideal gas law:

PV = RTn

∴ P = 20 Kgf/cm² * ( 0.9678 atm / Kgf/cm² ) = 19.356 atm

∴ V = 50 L average volume

∴ R = 0.082 atm * L / K * mol

∴ T = 495°C + 273 = 768 K

⇒ n = PV / RT

⇒ n = ((19.356 atm) * (50 L)) / ((0.082atm*L/K*mol) * (768K))

⇒ n = 15.367 mol N2(g)