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For a perfectly crystalline solid C(p.m)...

For a perfectly crystalline solid `C_(p.m) = aT^(3)`, where a is constant. If `C_(p.m)` is 0.42 J/K `-` mol at 10K, molar entropy at 10K is

A

0.42 J/K-mol

B

0.14 J/K-mol

C

4.2 J/K-mol

D

zero

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The correct Answer is:
B
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Knowledge Check

  • For a perfectly cyrstalline solid C_(p,m) a T^(3) + bT , where a and b are constants. If C_(p, m) is 0.40J/K mol at 10K and 0.92J/K mol at 20K, then molar entropy at 20K is:

    A
    0.92 J/K mol
    B
    8.66 J/K mol
    C
    0.813 J/K mol
    D
    none of these

  • Molar conductivity (^^_m) is defined as conducting power of the ions produced by 1 mole of an electrolyte in a solution. ^^_m =(K)/(C) where K is conductivity (in S-cm^(-1) ), ^^_m is molar conductivity (in Scm^(2) mol^(-1) ) and C is molar concontration (in "mole"//cm^(3) ) The molar conductivity of 0.04 M solution of MgCl_2 is 200Scm^2 mol^(-1) at 298 K. A cell with electrodes that are 2.0cm^(2) in surface area and 0.50 cm apart is filled with MgCl_2 solution. The cell constant is

    A
    `0.25 cm^(-1)`
    B
    `0.50 cm^(2) `
    C
    `0.025 cm `
    D
    ` 0.35 cm^(2)`

  • Molar conductivity (^^_m) is defined as conducting power of the ions produced by 1 mole of an electrolyte in a solution. ^^_m =(K)/(C) where K is conductivity (in S-cm^(-1) ), ^^_m is molar conductivity (in Scm^(2) mol^(-1) ) and C is molar concontration (in "mole"//cm^(3) ) The molar conductivity of 0.04 M solution of MgCl_2 is 200Scm^2 mol^(-1) at 298 K. A cell with electrodes that are 2.0cm^(2) in surface area and 0.50 cm apart is filled with MgCl_2 solution. Conductivity of MgCl_2 solution is :

    A
    `8 xx 10^(-3) S cm^(-1)`
    B
    `32S cm^(-1)`
    C
    `0.032 S cm^(-1) `
    D
    None of these
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