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

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. We can convert the pressure to Pa: 6.0 atm * 101 kPa/atm = 606 kPa. We can now plug these values into the equation to solve for n: n = (606 kPa * 5.3 L) / (8.31 J/mol ∙ K * 290 K) = 0.13 mol. We can now use the molar mass of neon to convert moles to grams: 0.13 mol * 20.2 g/mol = 2.7 g. Therefore, the mass of the neon gas in the flask is 2.7 g.

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