Question

33) A student has three 5.00L vessels at 25°C. One is filled with helium. Another is filled with neon and the third is filled with carbon dioxide? All three vessels have the same pressure. a) Which vessel has the greater number of moles of gas? Explain your answer. (4 points) b) Which vessel has the greater mass? (4 points) c) Which vessel has the greater kinetic energy? (4 points) d) Inside of which vessel are the particles moving the fastest? (4 points) e) Which vessel is the most dense? (4 points)

Answer 1

Ideal gas law state that PV = nRT P, V and T are came for all the three vessel R = universal gas constant (a) All the three vessel have equal moles of gas. This is because P, V & T are also came for all the three vessel. Implies P V/R T = n = constant (b) Molar mass of helium = 4 g/mol Molar mass of Neon = 20 g/mol Molar mass of CO_2 = 44g/mol mass of gas = moles of gas(n) times Molar mass of gas proportionalto Molar mass of gas This is because n is came for all gases therefore CO_2 has the greatest mass as it has the greatest molar mass. (c) K E_average = 3/2 KT K is Boltzmann constant proportionalto T So all the vessel will have came kinetic energy as temperature is maintained came for all the three vessel. (d) We know V_rms of particle is V_rms = squareroot 3RT/M implies