The critical temperature `(T_(c))` and pressure `(P_(c))` of `NO` are `177 K` and `6.48MPa`, respectively, and that of `CCl_(4)` are `550 K` and `4.56MPa`, respectively. Which gas `(a)` has the smaller value for the van der Waals constant `b`, `(b)` has the smaller value for constant `a`, `(c)` has the larger critical volume, and `(d)` is most nearly ideal in behaviour at `300 K` and `1.013MPa`.

Explanation

To solve the problem step by step, we will analyze the properties of the gases NO and CCl₄ using the given critical temperature and pressure values. We will calculate the van der Waals constants \( a \) and \( b \), the critical volume, and determine which gas behaves more ideally under the specified conditions.

### Step 1: Calculate the van der Waals constant \( b \)

The van der Waals constant \( b \) can be calculated using the formula:
\[ b = \frac{RT_c}{8P_c} \]
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