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H2O > H2Te > H2Se > H2S - M.P & B.P

H2O> H2S > H2Se > H2Te - Ka value

H2O> H2S > H2Se > H2Te --X-H bond enthalpy

O-H < S-H < Se-H < Te-H - Bond length

answer is B.

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Detailed Solution

Down the group in the hydrides of 15th , 16th , 17th groupsA) Affinity towards Hydrogen decreasesB) X-H bond enthalpy decreasesC) X-H bond length increasesD) Thermal stability decreasesE) Acidic strength (Ka) increasesF) Reducing power increasesThus 'Ka' of H2O< H2S < H2Se < H2Te∆HB.D.E of H2O> H2S > H2Se > H2Te (BDE=Bond dissociation enthalpy)X-H bond length O-H < S-H < Se-H < Te-Hfrom H2O to H2Te molecular weight and molecular size increases , vanderwaals forces become stronger Expected MP & BP - H2O< H2S < H2Se < H2TeBut H2O molecules are associated through intermolecular H- bonding.It has abnormally high MP & BPMP & BP order will be H2S< H2Se < H2Te< H2O (or) H2O > H2Te> H2Se > H2S

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