Question

Q1. In a tank 2740 grams of nitrogen is compressed. It is held at a temperature of 18.7°C and the pressure is 3.75 x 10 Pa. The tank is opened and gas is allowed to escape into the atmosphere where the pressure is 1 bar. At the end of the process, the pressure in the tank has dropped to 1.80 x 105 Pa. Assuming that the gas is ideal and that the temperature remains constant, what volume of nitrogen has been released into the atmosphere?

Answer 1

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Given it Temprature Ti = 18.7% = 291.7k pressure Ps = 3.75 x 107 Pa Amorint q Na molar mass 2740g of N₂ = 28 g/mol 2740 Мал , 28 g/m initial Pi = 3,75x107 Pa اي عمليا can =) nf = na ni= 97.857 mol Given the final pressure inside conleviner = 1.8x105 Pa final Pf = 108 x 105 pa ni = 97.857mall nf= find me from ideal gas equaftion. Piv Pq v niRT nipo Af RT Ps 97.857 X18X10S nf= 3.75 X 107 6.4697 mol No. of moles of geus escaped - Ing- nisl = 10,4697- 97.857| = 97.387 mol Outside pressure is I bar 1.0/x 105 pa of R = 8.314 m3pa mol k - Value from ideal gas egr V=nRT 97.387x8.314 x 291.7 1.018105 m3 Р = 2.4029 m3 = 2.40 x103 L