A cubic vessel with each side measuring 20 cm contains diatomic hydrogen (H2) gas at a temperature of 300 K. Each H2 molecule comprises two hydrogen atoms, each with a mass of \( 1.66 \times 10^{-24} \, \text{g} \), separated by a distance of approximately \( 10^{-8} \, \text{cm} \). Assume the gas follows the ideal gas law and neglect the vibrational degrees of freedom. The molar heat capacities \(C_p \) and \(C_V\) are:
1
\( C_P = 20 \, \text{J/mol·K} \) and \( C_V = 29 \, \text{J/mol·K} \)
2
\( C_P = 29 \, \text{J/mol·K} \) and \( C_V = 21 \, \text{J/mol·K} \)
3
\( C_V = 25 \, \text{J/mol·K} \) and \( C_p = 26 \, \text{J/mol·K} \)
4
\( C_V = 21 \, \text{J/mol·K} \) and \( C_p = 22 \, \text{J/mol·K} \)