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

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Quizplus · Accepted Answer

The mass of the neon gas in the flask can be calculated using the ideal gas law:PV = nRTwhere 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.The number of moles of neon gas can be calculated using the atomic mass of neon and the Avogadro's number:n = m/Mwhere m is the mass of the neon gas and M is the atomic mass of neon.Substituting the given values into the ideal gas law, we get:6.0 atm * 5.3 L = n * 8.31 J/mol ? K * 290 Kn = 0.40 molThe mass of the neon gas can now be calculated using the number of moles and the atomic mass of neon:m = n * Mm = 0.40 mol * 20.2 g/molm = 8.08 gTherefore, the mass of the neon gas in the flask is 8.08 g, which is closest to choice A) 2.7 × 10^-2.

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