Calculate the pressure exerted by one mole of methane in a 450 mL container at `25^@C` using van der Waals' equation. What pressure will be predicted by ideal gas equation ?
(Given : `a = 2.253 " atm " L^2 mol^(-2), b = 0.0428 L mol^(-2),
R =0.0821 L " atm " K^(-1) mol^(_1))`

Explanation

To solve the problem of calculating the pressure exerted by one mole of methane in a 450 mL container at 25°C using van der Waals' equation, we will follow these steps:

### Step 1: Convert Given Values to Appropriate Units
- Volume (V) = 450 mL = 0.450 L
- Temperature (T) = 25°C = 25 + 273 = 298 K
- Number of moles (n) = 1 mole
- Given constants:
- \( a = 2.253 \, \text{atm L}^2 \text{mol}^{-2} \)
...