Question

five samples of helium gas are described in the table below. rank the samples in order of increasing average kinetic energy of the atoms in them. that is, select \1\ next to the sample in which the helium atoms have the lowest average kinetic energy. select \2\ next to the sample in which the helium atoms have the next lowest average kinetic energy, and so on. table with columns: sample (amount, pressure, temperature), average kinetic energy of atoms in sample; rows: 1.7 mol, 1.3 atm, -27. °c (select); 1.0 mol, 1.1 atm, -56. °c (select); 1.9 mol, 2.6 atm, -16. °c (select); 1.6 mol, 1.9 atm, -40. °c (select); 2.5 mol, 2.7 atm, -37. °c (select); buttons: refresh, close

Explanation:

Step1: Recall kinetic energy rule

Average kinetic energy of gas atoms depends only on absolute temperature (Kelvin), not amount/pressure. Convert °C to K: $K = °C + 273.15$.

Step2: Calculate each sample's K

• Sample1 (-27°C): $273.15 -27 = 246.15$ K
• Sample2 (-56°C): $273.15 -56 = 217.15$ K
• Sample3 (-16°C): $273.15 -16 = 257.15$ K
• Sample4 (-40°C): $273.15 -40 = 233.15$ K
• Sample5 (-37°C): $273.15 -37 = 236.15$ K

Step3: Rank by increasing K

Order of K (lowest to highest): 217.15 < 233.15 < 236.15 < 246.15 < 257.15 → Sample2 < Sample4 < Sample5 < Sample1 < Sample3.

Answer:

Sample1: 4
Sample2: 1
Sample3: 5
Sample4: 2
Sample5: 3