Kinetic Theory of Gases
Physics ⇒ Heat and Thermodynamics
Kinetic Theory of Gases starts at 10 and continues till grade 12.
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See sample questions for grade 12
A gas at 27°C is heated to 127°C at constant pressure. By what factor does its volume change?
A gas is compressed to half its original volume at constant temperature. What happens to the mean free path of its molecules?
A gas is contained in a 2 L vessel at 300 K and 1 atm pressure. Calculate the number of molecules present. (R = 0.0821 L·atm/mol·K, Avogadro's number = 6.022 × 1023 mol−1)
A gas sample contains 2 moles of nitrogen at 273 K. Calculate the total kinetic energy of the gas. (R = 8.314 J/mol·K)
A sample of oxygen gas at 300 K has a root mean square speed of 484 m/s. Calculate the molar mass of oxygen. (R = 8.314 J/mol·K)
A vessel contains 0.5 mol of helium at 400 K. Calculate the average kinetic energy per molecule. (k = 1.38 × 10−23 J/K)
Describe the difference between the root mean square speed, average speed, and most probable speed of gas molecules.
Explain the physical meaning of the Boltzmann constant (k).
Explain why lighter gas molecules move faster than heavier ones at the same temperature.
Explain why real gases deviate from ideal behavior at high pressures and low temperatures.
If the temperature of a gas is increased, what happens to the average kinetic energy of its molecules?
State the ideal gas equation and define each term.
The pressure exerted by an ideal gas is given by P = (1/3)ρvrms2. What does ρ represent in this equation?
The pressure of a fixed amount of gas is doubled at constant temperature. What happens to the volume?
