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Which of the following best explains the fact that H2S boils at -60 Celsius while H2O boils at 100 Celsius at normal atmospheric pressure? Both H2O and H2S exhibit London dispersion forces, but the dispersion forces are stronger in H2O H2O has a larger net dipole moment than H2S. H2O exhibits hydrogen bonding interactions while H2S does not. H2O has London dispersion forces while H2S does not. H2O has a smaller mass than H2S