The relation between pressure exerted by an ideal gas `(p_("ideal"))` and observed pressure `(p_("real"))` is given by the equation,
`p_("ideal")=p_("real")+ (an^(2))/V^(2)`
(i) If pressure is taken in `NM^(-2)`, number of moles in mol and volume in `m^(3)`, calculate the unit of 'a'.
(ii) What will be the unit of 'a' when pressure is in atmosphere and volume in `dm^(3)`?

Explanation

To solve the problem step by step, we need to analyze the given equation and determine the units for 'a' in two different scenarios.

### Step 1: Understand the Given Equation
The equation provided is:
\[ p_{\text{ideal}} = p_{\text{real}} + \frac{a n^2}{V^2} \]
Here, \( p_{\text{ideal}} \) and \( p_{\text{real}} \) are pressures, \( n \) is the number of moles, and \( V \) is the volume.

### Step 2: Identify the Units
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