Question

Explain Vanderwaal's Gas Equation ❔❔❔❤

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Answer 1

Answer:

• Real gases show deviation from ideal gas law because molecules interact with each other.
• At high pressures molecules of gases are very close to each other.
• Molecular interaction start operating.
• At high pressure, molecules do not strike the walls of the container with full impact because these are dragged back by other molecules due to molecular attractive force.
• This affect the pressure exerted by the molecules on the walls of the container.
• Thus, the pressure exerted by the gas is lower than the pressure exerted by the ideal gas.

• $P_{ideal}=P_{real}+\frac{an^{2} }{V^{2}}$

• In the above equation, a is known as Vander waal's Pressure correction term.
• Repulsive interaction between the molecules happen due to high pressure.
• The volume occupied by the molecules are restricted to volume (V-nb) where "nb" is approximately the total volume occupied by the molecules themselves.
• Like "a", "b" is also called Vander waal's constant namely his Volume correction term.
• We know that, PV=nRT
• Since we applied correction terms, the new equation is:$(P+\frac{an^{2}}{V^{2}})(V-nb)=nRT$
• This equation is thus known as Vander waal's gas equation.

• "a" and "b" depends on the characteristics of the gas.  

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Answer 2

Explanation:

An equation of state that relates the pressure, volume, and absolute temperature of a gas taking into account the finite size of molecules, and their intermolecular attraction, having the form RT = ( P + av −2)( v − b ), where R is the gas constant, T is the absolute temperature, P is the pressure, v is the volume, and a and b are constants.