What happens to the Maxwell-Boltzmann distribution as T increases from T1 to T2?

Answer: Peak shifts to higher speed and curve broadens Higher T raises average kinetic energy; the most probable speed increases, the peak lowers, and the distribution broadens (area is conserved).

KMT assumes that ideal gas molecules

Answer: Are point particles in random motion with negligible volume and no IMF except elastic collisions Real gases deviate at high P and low T (when volumes and IMFs matter); ideal at low P, high T.

Why is the He distribution shifted to higher speeds?

Answer: Lower molar mass means higher average speed at same T At the same T, average KE is the same; vrms = sqrt(3RT/M). Smaller M (He = 4 g/mol) gives larger vrms than Xe (131 g/mol).

AP Chemistry · Topic 3.5

Kinetic Molecular Theory Practice

Part of Properties of Substances and Mixtures.(SAP-7.C)

Practice questions

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Sample questions

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Sample 1difficulty 2/5
$Two Maxwell-Boltzmann speed distributions are drawn for the same gas at temperatures T1 and T2.$
$What happens to the Maxwell-Boltzmann distribution as T increases from T1 to T2?$
- A
  $Peak shifts to higher speed and curve broadens$
  check_circle
- B
  $Peak shifts to lower speed$
- C
  $No change in distribution$
- D
  $Curve narrows and peaks higher$
Why
$Higher T raises average kinetic energy; the most probable speed increases, the peak lowers, and the distribution broadens (area is conserved).$
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Sample 2difficulty 2/5
$KMT assumes that ideal gas molecules$
- A
  $Are point particles in random motion with negligible volume and no IMF except elastic collisions$
  check_circle
- B
  $Move slowly$
- C
  $Have significant volume and attractive forces$
- D
  $Stick together$
Why
$Real gases deviate at high P and low T (when volumes and IMFs matter); ideal at low P, high T.$
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Sample 3difficulty 2/5
$Two gases are at the same temperature.$
$Why is the He distribution shifted to higher speeds?$
- A
  $Lower molar mass means higher average speed at same T$
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- B
  $He has stronger IMFs$
- C
  $He molecules are larger$
- D
  $He has greater kinetic energy than Xe$
Why
$At the same T, average KE is the same; v_rms = sqrt(3RT/M). Smaller M (He = 4 g/mol) gives larger v_rms than Xe (131 g/mol).$
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Sample 4difficulty 3/5
$As temperature increases, the Maxwell-Boltzmann distribution$
- A
  $Stays the same$
- B
  $Becomes narrower with a lower peak at higher speed$
- C
  $Becomes broader and the peak shifts to higher speeds$
- D
  $Both A and C — broader, peak at higher speed, lower height$
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Why
$At higher T, distribution flattens out (more spread), peaks at higher speed, and the average KE grows.$
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Sample 5difficulty 3/5
$Average kinetic energy of gas particles depends on$
- A
  $Mass$
- B
  $Volume$
- C
  $Absolute temperature only$
  check_circle
- D
  $Pressure$
Why
$KE_avg = (3/2)kT. At a given T, all gases have the same average KE (but different speeds because of different masses).$
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