A 5.3 L flask of ideal neon gas (which is monatomic)is at a pressure of 6.0 atm and a temperature of $290 \mathrm {~K} .$ The atomic mass of neon is 20.2 g/mol.What is the mass of the neon gas in the flask.(R = 8.31 J/mol ∙ K,1 atm = 101 kPa,N_A = 6.022 × 10²³ molecules/mol)

Question

Quizplus · Accepted Answer

The ideal gas law is 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. We can rearrange this equation to solve for n: n = PV/RT. We are given P = 6.0 atm, V = 5.3 L, R = 8.31 J/mol ∙ K, and T = 290 K. Plugging these values into the equation, we get: n = (6.0 atm)(5.3 L)/(8.31 J/mol ∙ K)(290 K) = 0.13 mol. The mass of the neon gas is then: mass = n × molar mass = (0.13 mol)(20.2 g/mol) = 2.7 × 10^-2 g.

A 53 L Flask of Ideal Neon Gas (Which Is Monatomic)is