The predominant intermolecular forces present in ethyl acetate, a liquid, are:

🧠 Ethyl acetate ($\mathrm{CH_3COOC_2H_5}$) is a polar ester — it has a net dipole moment but no O–H or N–H groups, so it cannot form H-bonds as a donor.

🗺️ Identify the intermolecular forces:

• London dispersion forces: Present in ALL molecules (due to instantaneous dipoles) ✓
• Dipole–dipole forces: Ethyl acetate has a polar C=O and C–O bonds → net dipole ≠ 0 → permanent dipole-dipole interactions ✓
• Hydrogen bonding: Requires H bonded to F, O, or N. Ethyl acetate has no O–H or N–H → cannot donate H-bonds ✗ (it can accept H-bonds from other molecules, but pure ethyl acetate liquid has no H-bond donors)

⚡ Ethyl acetate is a polar non-protic solvent — polar enough for dipole interactions but no H-bond capability.

$\boxed{\text{Answer: London dispersion and dipole–dipole}}$