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 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) A)2.7 × 10^-2 B)1.6 × 10^-2 C)1.3 × 10¹ D)2.7 × 10¹ E)2.7 × 10³

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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. We can convert the pressure to Pa: 6.0 atm * 101 kPa/atm = 606 kPa.Now we can plug in our values and solve for n:n = (606 kPa * 5.3 L) / (8.31 J/mol ∙ K * 290 K) = 0.13 molThe mass of the neon gas is then:mass = n * molar mass = 0.13 mol * 20.2 g/mol = 2.7 gTherefore, the mass of the neon gas in the flask is 2.7 × 10^-2 g.

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