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# The Ideal Gas Equation Video Lecture - Chemistry Class 11 - NEET

## Chemistry Class 11

195 videos|337 docs|190 tests

## FAQs on The Ideal Gas Equation Video Lecture - Chemistry Class 11 - NEET

 1. What is the ideal gas equation and how is it derived? Ans. The ideal gas equation, also known as the equation of state for ideal gases, is given by the formula PV = nRT, where P is the pressure, V is the volume, n is the number of moles of gas, R is the ideal gas constant, and T is the temperature. It is derived from the combination of Boyle's law, Charles's law, and Avogadro's law, which describe the relationships between pressure, volume, temperature, and the number of moles of gas.
 2. What are the units of the ideal gas constant and how is it determined? Ans. The ideal gas constant (R) is usually expressed in units of liter-atmospheres per mole-kelvin (L·atm/(mol·K)) or joules per mole-kelvin (J/(mol·K)). It can be determined experimentally by measuring the physical properties of a gas and using the ideal gas equation to calculate R. Alternatively, it can be derived from fundamental constants, such as Avogadro's number and Boltzmann's constant.
 3. Can the ideal gas equation be used for real gases? Ans. The ideal gas equation is an approximation that assumes gases behave ideally, meaning they have no intermolecular forces and occupy negligible volume. While real gases do not strictly follow the ideal gas equation, it can still be used as an approximation for many gases at low pressures and high temperatures. However, at high pressures and low temperatures, real gases deviate significantly from the ideal gas behavior, and more complex equations of state, such as the van der Waals equation, are required.
 4. How can the ideal gas equation be used to calculate the molar mass of a gas? Ans. The ideal gas equation can be rearranged to calculate the molar mass (M) of a gas. By measuring the pressure (P), volume (V), temperature (T), and knowing the number of moles (n) of the gas, the equation can be rearranged as M = (mRT)/(PV), where m is the mass of the gas. By substituting the known values into the equation, the molar mass of the gas can be calculated.
 5. What are the limitations of the ideal gas equation? Ans. The ideal gas equation has several limitations. It assumes that gases behave ideally, which means they have no intermolecular forces and occupy negligible volume. This approximation breaks down at high pressures and low temperatures when real gases deviate significantly from ideal gas behavior. Additionally, the ideal gas equation does not account for the effects of molecular size or the presence of condensation or phase changes. For these cases, more advanced equations or corrections, such as the van der Waals equation or the compressibility factor, must be used.

## Chemistry Class 11

195 videos|337 docs|190 tests

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