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What is the entropy change for the conve...

What is the entropy change for the conversion of one gram of ice to water at 167 K and one atmospheric pressure ? `[Delta H_("fussion") = 6.025 kJ mol^(-1)]`

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The correct Answer is:
2
`Delta _("fusion") S = (Delta_("fusion")H)/(T_(f)) rArr (6.025 xx 10^(3))/(167) xx (1)/(18)`
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What is entropy change for the conversion of one gram of ice to water at 273 K and one atmospheric pressure? (DeltaH_("fusion")=6.025kJ" "mol^(-1))

What is the entropy change for conversion of one gram of ice to water at 273K and one atmospheric pressure ( Delta _(fus) H = 6.025 kJ mol^(-1)) ?

Knowledge Check

  • The change of energy on freezing 1.00 kg of liquid water of 0^(@)C and 1 atm is : (Delta H _("ice"))_("fusion") = 6. 01 kJ // mol

    A
    `236.7 kJ kg ^(-1)`
    B
    `236.4 kJ kg ^(-1)`
    C
    `-333.4 kJ kg ^(-1)`
    D
    `- 236.7 kJ kg ^(-1)`

  • What is the entropy that takes place in conversion of 1 mol of alpha- tin to 1 mol beta - tin at 17^(@)C , 1 atm pressure if enthalpy of transition is 2.90 kJ mol^(-1) ?

    A
    `1.0 kJ mol^(-1)`
    B
    `7.32 JK^(-1) mol^(-1)`
    C
    `10JK^(-1)mol^(-1)`
    D
    `100JK mol^(-1)`

    • Similar Questions

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    Calculate the entropy change involved in conversion of one mole ( 18g) of solid ice at 273K to liquid water at the same temperature ( latent heat of fusion =6025J mol^(-1))

    Calculate the entropy change for the conversion of2 moles of liquid water at 373K to vapours , if Delta_(vap) H is 37.3kJ mol^(-1) .

    Calculate the entropy change for the conservation of following: (a) 1g ice to water at 273K , DeltaH_f for ice=6.025kJmol^(-1) . (b) 36g water to vapour at 373K, DeltaH_v for H_2O=40.63kJmol(-1)

    Calculate the change in entropy for the fusion of 1 mole of ice (water). The melting point of water is 273 K and molar enthalpy of funsion for water =6.0 kJ mol^(-1)

    Calculate the entropy change accompanying the conversion of 1 mole of ice at 273.1 K and 1 atm pressure into steam at 373.1 K and 1 atm pressure. At 273.1 K, the molar heat of fusion of ice, DeltaH_(f) is 6.00 kJ mol^(-1) and at 373.1 K, the molar heat of vapourization of water, DeltaH_(v) , is 40.6 kJ mol^(-1) . Also assume that the molar heat capacities, C_(p) , in the temperature range 373.1 to 273.1 K remains constant. Given that C_(p) = 75.25 m mol^(-1)K^(-1) and log 13.66 = 1.1354.

    Calculate the entropy change involved in the converion of one mole of liquid water at 373 K to vapour at the same temperature ( latenet heat of vaporization of water Delta_(vap) H = 2.257 kJ //g)

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