Heat absorbed, $Q = m L = 10 \text{ g} \times 540 \text{ cal/g} = 5400 \text{ cal}$.
At $100^\circ \text{C}$, the temperature in Kelvin is $T = 373 \text{ K}$. Change in entropy:
$\Delta S = \frac{Q}{T} = \frac{5400 \text{ cal}}{373 \text{ K}} \approx 14.48 \text{ cal/K}.$
The official “closest” or typical reported answer is $14.47 \text{ cal/K}$. Possibly the question includes a factor of 10 or an alternative unit interpretation
List I | List II |
---|---|
(A) (∂S/∂P)T | (I) (∂P/∂T)V |
(B) (∂T/∂V)S | (II) (∂V/∂S)P |
(C) (∂T/∂P)S | (III) -(∂V/∂T)P |
(D) (∂S/∂V)T | (IV) -(∂P/∂S)V |
Ultraviolet light of wavelength 350 nm and intensity \(1.00Wm^{−2 }\) falls on a potassium surface. The maximum kinetic energy of the photoelectron is