(a) An ideal gas occupies a volume of 1.8 cm3 at 20°C and atmospheric pressure. Determine the number of molecules of gas in the container.
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PV = nRT n = PV/RT P = 1.00 atm V = 1.8 cm³ = 1.8 cm³ x (1 mL / 1 cm³) x (1 L / 1000 mL) = 0.0018 L R = 0.0821 Latm/moleK T = 20C = 20+273.15 = 293.15K n = (1.00 atm) x (0.0018 L) / [ (0.0821 Latm/moleK) x (293.15K) ] n = 7.48x10^-5 moles.. finally... 7.48x10^-5 moles x (6.022x10^23 molecules / 1 mole) = 4.50x10^19 molecules. you should probably only have 2 sig figs since 1.8 has 2 and 20 has at most 2..... # molecules = 4.5x10^19
using the same formula, we get
2.4 ✕ 10−11 Pa= ?
= 2.4 X10−11 / 10^5 atm
n = (2.4 ✕ 10−11/10^5) x (0.0018 L) / [ (0.0821 Latm/moleK) x (293.15K) ]
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