Higher boiling point of H2S compared to PH3 is best explained by

Stronger dipole - dipole attractions in H 2 S as compared to PH 3

Stronger dipole - dipole attractions in H 2 S as compared to PH 3

Stronger S-H bond enthalpy in H 2 S as compared to P-H bond enthalpy in PH 3

Higher molar mass of H 2 S as compared to PH 3

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Higher boiling point of H₂S compared to PH₃ is best explained by

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Stronger dipole - dipole attractions in H₂S as compared to PH₃

Stronger S-H bond enthalpy in H₂S as compared to P-H bond enthalpy in PH₃

Larger size of sulphur as compared to phosphorous

Higher molar mass of H₂S as compared to PH₃

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Molar mass of H₂S = PH₃ = 34 g/mole.

Sulphur is more electronegative than phosphorous.

Dipole moment of H₂S > Dipole moment of PH₃.

Dipole - dipole attractions in H₂S are stronger as compared to PH₃.

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