The question asks to identify which statement is NOT a postulate of the kinetic theory of gases. We need to recall the fundamental assumptions of the kinetic theory of gases and compare them with the given options.
D) Gas molecules exert strong attractive forces on each other
This statement contradicts a fundamental postulate of the kinetic theory of gases. According to the kinetic theory, there are no significant attractive or repulsive forces between gas molecules. This assumption is crucial for ideal gas behavior. If strong attractive forces existed, the gas would deviate significantly from ideal behavior, especially at low temperatures and high pressures.
The question asks about the relationship between the average kinetic energy of gas molecules and various physical properties. This can be understood by recalling the kinetic theory of gases.
Correct Option: C) Absolute temperature. As derived from the kinetic theory of gases, the average kinetic energy of gas molecules is directly proportional to the absolute temperature of the gas.
This question asks about the kinetic energy of gas molecules at absolute zero. To answer this, we need to recall the definition of absolute zero and its relation to molecular motion and kinetic energy, particularly from the perspective of the kinetic theory of gases.
D) Zero. At absolute zero (0 K), the absolute temperature is zero, and since the average kinetic energy of gas molecules is directly proportional to the absolute temperature, the kinetic energy becomes zero according to the kinetic theory of gases.
The question asks to identify the gas law that describes the inverse relationship between the pressure and volume of a gas when the temperature is kept constant. We need to recall the definitions of the major gas laws.
Correct Option: C) Boyle's Law states that at constant temperature, the pressure of a gas is inversely proportional to its volume. This relationship is fundamental in understanding the behavior of ideal gases.
The question asks about Charles's Law, which describes the relationship between the volume and temperature of a gas when pressure is kept constant. We need to recall the fundamental statement of Charles's Law.
where \(V\) is the volume of the gas and \(T\) is its absolute temperature (measured in Kelvin).
D) Directly proportional to absolute temperature. This statement accurately reflects Charles's Law, which defines the relationship between the volume and absolute temperature of a gas at constant pressure.
The question asks for the correct representation of the ideal gas equation. This fundamental equation in chemistry and physics describes the behavior of an ideal gas under various conditions. It combines Boyle's Law, Charles's Law, Avogadro's Law, and Gay-Lussac's Law into a single relationship.
Recall the individual gas laws:
Combine these laws to derive the ideal gas equation. From Boyle's Law, \(P \propto 1/V\). From Charles's Law, \(V \propto T\). From Avogadro's Law, \(V \propto n\). Combining these, we get:
\[ PV \propto nT \]To convert this proportionality into an equation, a proportionality constant is introduced. This constant is known as the ideal gas constant, denoted by \(R\).
Thus, the ideal gas equation is:
\[ PV = nRT \]Where:
Correct Option: D) PV = nRT