In an ideal gas, the average kinetic energy of a molecule is directly proportional to which of the following?
Practice Questions
1 question
Q1
In an ideal gas, the average kinetic energy of a molecule is directly proportional to which of the following?
Pressure
Volume
Temperature
Number of molecules
The average kinetic energy of a molecule in an ideal gas is directly proportional to the absolute temperature of the gas, given by the formula KE_avg = (3/2)kT.
Questions & Step-by-step Solutions
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Q
Q: In an ideal gas, the average kinetic energy of a molecule is directly proportional to which of the following?
Solution: The average kinetic energy of a molecule in an ideal gas is directly proportional to the absolute temperature of the gas, given by the formula KE_avg = (3/2)kT.
Steps: 5
Step 1: Understand what kinetic energy is. Kinetic energy is the energy that a molecule has due to its motion.
Step 2: Learn about ideal gases. An ideal gas is a theoretical gas where the molecules do not interact with each other except during elastic collisions.
Step 3: Know the formula for average kinetic energy. The average kinetic energy (KE_avg) of a molecule in an ideal gas is given by the formula KE_avg = (3/2)kT, where k is the Boltzmann constant and T is the absolute temperature.
Step 4: Identify the relationship. In the formula, you can see that KE_avg is directly proportional to T, which means as the temperature increases, the average kinetic energy also increases.
Step 5: Conclude that the average kinetic energy of a molecule in an ideal gas is directly proportional to the absolute temperature.
