Using van der Waals equation, calculate the constant `a` when `2 mol` of a gas confined in a `4 L` flasks exerts a pressure of `11.0 atm` at a temperature of `300 K`. The value of `b` is `0.05 L mol^(-1)`.

Using van der Waals equation, calculate the constant `a` when `2 mol`

1.	Using van der Waals equation, calculate the constant `a` when `2 mol` of a gas confined in a `4 L` flasks exerts a pressure of `11.0 atm` at a temperature of `300 K`. The value of `b` is `0.05 L mol^(-1)`.
Answer» The van der Waals equation of state for a gas is `(P+(an^(2))/(V^(2)))(V-nb)=nRT` `:. (11+(axx2^(2))/(4^(2)))(4-2xx0.05)=2xx0.0821xx300` or `a=6.46 atm L^(2) mol^(-2)`

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Using van der Waals equation, calculate the constant `a` when `2 mol` of a gas confined in a `4 L` flasks exerts a pressure of `11.0 atm` at a temperature of `300 K`. The value of `b` is `0.05 L mol^(-1)`.

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