A container with a one-liter capacity at 27° C is filled with helium to a pressure of 2.0 atm. (1 atm = 1.0 × 10⁵ N/m².) How many moles of helium does it hold? A) 0.041 B) 0.081 C) 0.45 D) 0.90 E) 1.0

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Quizplus · Accepted Answer

To find the number of moles of helium, we can use the ideal gas law, PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature in Kelvin. Given P = 2.0 atm (which is 2.0 × 1.0 × 10^5 N/m^2), V = 1 liter (which is 1 × 10^-3 m^3), and T = 27°C (which is 300K when converted to Kelvin), and using R = 8.31 J/(mol·K), we can solve for n. Rearranging the equation gives n = PV/(RT). Substituting the given values and converting units where necessary, we get n ≈ 0.081 moles.

A Container with a One-Liter Capacity at 27° C Is