Problem: Why are the critical temperature and pressure for H2O so much higher than those for H2S, a related substance?

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  • Critical temperature and pressure are the temperature and pressure at which a substance may still co-exist in the gaseous and liquid phase. Above the critical temperature, the gas can no longer be liquefied no matter how much pressure is applied.
  • The critical temperature and pressure are influenced by intermolecular forces of attraction (IMFA). The stronger the IMFA, the higher critical temperature and pressure because more energy in needed to vaporize the liquid until critical point.
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Why are the critical temperature and pressure for H2O so much higher than those for H2S, a related substance?