Question

When 1 kg of ice at 0°C melts to water at 0°C, the
resulting change in its entropy, taking latent heat
of ice to be 80 cal/°C, is
(a) 273 cal/K (b) 8 × 104 cal/K
(c) 80 cal/K (d) 293 cal/K

Answer 1

Answer:

As learnt in

Entropy for solid and liquid -

When heat is given to a substance to change its state at constant temperature.

- wherein

Delta S= frac{mL}{T}

L= Latent , Heat

T in kelvin

\Delta S = \frac{\Delta Q}{T} = \frac{mL}{T}

= \frac{1000\times 80}{273}\ cal/K

= 293\ cal/K

Option 1)

273\: cal/ K

This option is incorrect

Option 2)

8 \times 104\: cal/K

This option is incorrect

Option 3)

80 \:cal/K

This option is incorrect

Option 4)

293\:cal/K

This option is correct

Answer 2

≛ Question :-

When 1 kg of ice at 0°C melts to water at 0°C, theresulting change in its entropy, taking latent heatof ice to be 80 cal/°C, is

$\huge{\boxed{\mathfrak{\underline{\purple{answer!}}}}}$

➡️ (d) 293 cal/k ✔️✔️

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