Question

2.1 The following shows two identical sealed flasks, one containing He and one containing Ne. Both flasks are at the same temperature but the gases are at different pressures. He 298 K Ne 298 K 0.5 atm 1 atm Indicate whether the following statements are true or false and explain fully your reasoning for each. [5] a) Both flasks contain the same number of atoms. b) The He atoms have a greater average kinetic energy than the Ne atoms. c) The He atoms are moving more rapidly than the Ne atoms.

Answer 1

As pV= nRT

P = pressure

V= volume

n= number of moles

R = Universal gas constant

T = temperature

So the volume and temperature of two flasks are same. And also R is constant itslef.

So pressure is directly proportional to number of moles.

So He is having more pressure than Na so moles of He are more.

And as number of atoms = moles × avagadro number

Hence as He is having more moles .

So atoms of He gas are more than Na