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The standard molar entropy of H(2)O(l) i...

The standard molar entropy of `H_(2)O(l)` is `70 J K^(-1) "mol"^(-1)`.Will the standard molar entropy of `H_(2)O(s)` be more or less than `70 J K^(-1) "mol"^(-1)`?

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In ice, molecules of`H_(2)O` are less random than in liquid water. Hence , molar entropy of ice, `H_(2)O(s)`, will be less than that of liquid water, `H_(2)O(l)`.
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The standard molar entropy of H_(2)O(l) is 70 JK^(-1)mol^-1 . Standard molar entropy of H_(2)O(s) is

For the reaction (1)/(2) N_(2)(g) + (3)/(2) H_(2)(g) rarr NH_(3)(g), DeltaH =-30 KJ to be at equilibrium at 477^(@) C. If standard entropy of N_(2)(g) and NH_(3)(g) are 60 and 50 "J" "mole"^(-1)K^(-1) respectively then calculate the standard entropy of H_(2)(g) in "J mole"^(-1) K^(-1).

Determine the entropy change for the reaction 2H_(2)(g) +O_(2)(g) rarr 2H_(2)O(l) at 300K . If standard entropies of H_(2)(g),O_(2)(g) and H_(2)O(l) are 12.6, 201.20 and 68.0 J K^(-1) "mole"^(-1) respectively.

The volume strength of 1M H_(2)O_(2) is (Molar mass of H_(2)O_(2) = 34 g mol^(-1) )

Calculate free energy change for the reaction: H_(2)(g) + CI_(2)(g) rarr 2H-CI(g) by using the bond enegry and entropy data. Bond energies of H-H, CI-CI , and H-CI bonds are 435, 240 , and 430 kJ mol^(-1) , respectively. Standard entropies of H_(2),CI_(2) , and HCI are 130.59, 222.95 , and 186.68 J K^(-1) mol^(-1) , respectively.

Determine the entropy change for the reaction given below: 2H_(2)(g) +O_(2)(g) rarr 2H_(2)O(l) at 300K . If standard entropies of H_(2)(g), O_(2)(g) , and H_(2)O(l) are 126.6, 201.20 , and 68.0 J K^(-1) mol^(-1) , respectively.

Knowledge Check

  • The standard molar entropy of H_(2)O(l) is 70 JK^(-1)mol^-1 . Standard molar entropy of H_(2)O(s) is

    A
    more than 70 `JK^(-1)mol^(-1)`
    B
    less than 70 `JK^(-1)mol^(-1)`
    C
    equal to 70 `JK^(-1) mol^(-1)`
    D
    none of these

  • The standard molar entropy of H_(2)0_(l) is 70JK^-1 moJ^-1 Standard molar entropy of H_(2)0 (s) is

    A
    more than `70JK^-1mol^-1`
    B
    less than `70JK^-1mol^-1`
    C
    equal to `70JK^-1mol^-1`
    D
    None of the above

  • The standard enthalpy of formation of gaseous H_(2)O at 298 K is -241.82 kJ mol^(-1) . Calculate DeltaH_(f)^(@) at 373K, given the following values of the molar heat capacities at constant pressure. Molar heat capacity of H_(2)(g)=33.58JK^(-1)mol^(-1) Molar heat capacity of H_(2)(g)=28.84JK^(-1)mol^(-1) Molar heat capacity of O_(2)(g)=29.37JK^(-1)mol^(-1) Assume that the heat capacities are independent of temperature.

    A
    `-"242.6 kJ mol"^(-1)`
    B
    `-"485.2 kJ mol"^(-1)`
    C
    `-"121.3 kJ mol"^(-1)`
    D
    `-"286.4 kJ mol"^(-1)`
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