A container with a one-litre capacity at 27$\degree$ 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

Question

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Using the ideal gas law, PV = nRT, where P = 2.0 atm (2.0 * 10^5 N/m^2), V = 1 litre (1 * 10^-3 m^3), R = 8.314 J/(mol·K), and T = 27°C (300 K), we solve for n (moles): n = PV / RT = (2.0 * 10^5 * 1 * 10^-3) / (8.314 * 300) ≈ 0.081 moles.

A Container with a One-Litre Capacity at 27 °\degree° C Is Filled with Helium to a Pressure of 2

A Container with a One-Litre Capacity at 27 $\degree$ C Is Filled with Helium to a Pressure of 2