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 two moles of a gas confined in a four litre flask exerts a pressure of 11.0 atmospheres 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 two moles of a gas confined in a four litre flask exerts a pressure of 11.0 atmospheres at a temperature of 300 K. The value of b is 0.05 L "mol"^(-1)

Using van der Waals' equation, find the constant 'a' (in atm L^(2)mol^(-2) ) when two moles of a gas confined in 4 L flask exerts a pressure of 11.0 atmospheres at a temperature of 300 K. The value of b is 0.05 L mol^(-1) .(R = 0.082 atm.L/K mol)

Two moles of a real gas confined in a 5 L flask exerts a pressure 9.1 atm at a temperature of 27^(@)C . Calculate the value of 'a' given the value of b is "0.052 L mol"^(-1) .

Find out the value of the van der Waals constant 'a' when two moles of a gas confined in a 4 L flask exerts a pressure of 11.0 atm at 300 K. (b= 0.05 L mol^(-1)) .