Question

the van der waals equation, (nrt = (p + a(n/v)^{2})(v - nb)), incorporates corrections to the ideal gas law in order to account for the properties of real gases. predict which of the following gas molecules will have the largest value of the constant (a) in this equation?

(co_{2})

(n_{2})

(o_{2})

(ch_{4})

(h_{2})

Explanation:

The Van der Waals constant \(a\) accounts for intermolecular forces. Larger and more polar molecules have stronger intermolecular forces. \(CO_2\) is larger and has stronger intermolecular forces (due to its structure and polarity compared to \(N_2\), \(O_2\), \(CH_4\), and \(H_2\)). \(N_2\) and \(O_2\) are non - polar diatomic molecules. \(CH_4\) is non - polar (symmetrical tetrahedral structure). \(H_2\) is a small non - polar diatomic molecule.

Answer:

\(CO_2\)