Test: Behaviour of Gases - SSC CGL MCQ

Among the five main states of matter, gas is not one of them. Gases are particularly interesting to study due to their behavior being described by various gas laws, detailing the relationships between temperature, pressure, volume, and other properties. Plasma, Bose-Einstein condensate, solid, and liquid are the other four main states of matter.

Boyle's Law, along with other gas laws like Charles's Law and Gay-Lussac's Law, detail the relationships between temperature, pressure, volume, and other properties of gases. Boyle's Law specifically describes the inverse relationship between the pressure and volume of a gas when temperature is held constant.

Boyle's Law explains the relationship between the pressure and volume of a gas when the temperature remains constant. It states that the pressure of a gas is inversely proportional to its volume—an increase in pressure leads to a decrease in volume, and vice versa.

Bose-Einstein condensate is a state of matter that forms at extremely low temperatures close to absolute zero. It is characterized by a unique phase of matter where a group of bosons occupy the same quantum state, behaving as a single quantum entity. This state exhibits properties distinct from those of solids, liquids, and gases.

Charles's Law explains the relationship between the volume and temperature of a gas when pressure is held constant. It states that the volume of a gas is directly proportional to its temperature, meaning as the temperature increases, the volume of the gas also increases, and vice versa.

According to Boyle's Law, when the volume of a gas in a container is increased at a constant temperature, the pressure of the gas decreases. This is because the volume and pressure of a gas are inversely proportional when the temperature is held constant.

Charles' Law states that at constant pressure, the volume of a gas is directly proportional to its absolute temperature. This means that as the temperature of a gas increases, its volume also increases proportionally, assuming the pressure remains constant.

Gay-Lussac's Law states that at a constant volume, the pressure of a gas is directly proportional to its absolute temperature. Therefore, if the absolute temperature of a gas increases while the volume remains constant, the pressure of the gas will also increase.

Avogadro's Law states that under the same temperature and pressure conditions, equal amounts of different gases contain the same number of molecules. This law is fundamental in understanding the relationship between the volume of a gas and the number of molecules present.

At STP, one mole of any gas occupies a volume of 22.4 liters and contains approximately 6.022 x 10^23 molecules. This value is known as Avogadro's number and is crucial in understanding the relationship between the volume and number of molecules in a gas.

The equation of state for a perfect gas is PV = nRT, where P stands for pressure, V represents volume, T denotes absolute temperature, R is the universal gas constant, and n indicates the number of moles of the gas. This equation is fundamental in understanding the behavior of ideal gases under different conditions.

Real gases behave differently from ideal gases primarily because real gas molecules are attracted to each other. This intermolecular attraction causes real gases to deviate from ideal behavior, especially at high pressures and low temperatures. Understanding this attraction is crucial in explaining deviations from ideal gas laws in real-world scenarios.

In the Van der Waal's gas equation, 'a' and 'b' represent Van der Waal's constants. These constants are unique for each gas and are used to correct for the attractive forces between gas molecules (represented by 'a') and the volume occupied by the gas molecules (represented by 'b'). Incorporating these corrections in the equation accounts for the deviations of real gases from ideal behavior.

Inert gases behave similarly to ideal gases when subjected to high temperatures and very low pressures. These conditions allow inert gases to exhibit behavior that closely aligns with the predictions of ideal gas laws. Understanding these conditions is essential in predicting the behavior of gases in various experimental setups.

Equations for real gases require adjustments because real gas molecules exhibit intermolecular attraction and occupy space. These factors differentiate real gases from ideal gases, leading to deviations that necessitate modifications in equations to accurately describe the behavior of gases under non-ideal conditions. Understanding these adjustments is crucial in applying gas laws effectively in realistic scenarios.