Question

At $27ºC$ latent heat of fusion of a compound is $2930\ J/mol$. Entropy change is:

• A. $9.77 \ J/molK$
• B. $10.77 \ J/molK$
• C. $9.07 \ J/molK$
• D. $0.977 \ J/molK$

Answer 1

Answer: (A)

$9.77 \ J/molK$

Answer 2

The entropy change $(ΔS)$ can be calculated using the formula:

$ΔS=\frac {ΔH​}{T}$

where $ΔH$ is the latent heat of fusion and $T$ is the temperature in Kelvin.

Given:

Latent heat of fusion $(ΔH) = 2930 \ J/mol$

Temperature $(T) = 27°C = 27 + 273 = 300 K$

Now, put the values:

$ΔS=\frac {2930\ J/mol}{300 K}$

$ΔS =9.77\ J/molK$

So, the correct option is (A): $9.77\ J/molK$