Question

The entropy change for the conversion of 1 mole of $\alpha $ tin (at 13C,1atm) to one mole of $\beta $ tin (at 13C, 1 atm ), if the enthalpy of transition is 2.095 K $Jmo{l^{ - 1}}{K^{ - 1}}$is
(A) $7.32Jmo{l^{ - 1}}{K^{ - 1}}$
(B) 14.62$Jmo{l^{ - 1}}{K^{ - 1}}$
(C) 56$Jmo{l^{ - 1}}{K^{ - 1}}$
(D) 0

Answer 1

Hint: Entropy is a thermodynamic term. Entropy is the measure of thermal energy per unit temperature.
use the formula $\Delta S = \dfrac{{\Delta H}}{T}$Where temperature is in kelvin

Step by step explanation :
1. Convert the temperature in kelvin

$T = 273 + 13 = 286$K

2. Put the values in the equation

Given: enthalpy of transition = 2.095 KJ mol

             Temperature = 286

$\Delta S = \dfrac{{\Delta H}}{T} = \dfrac{{2095}}{{286}} = 7.32Jmo{l^{ - 1}}{K^{ - 1}}$

$\Delta S = \dfrac{{\Delta H}}{T} = \dfrac{{2095}}{{286}} = 7.32Jmol$ $$

Option (a) is correct

Additional information: Enthalpy is another thermodynamic term. It is the sum of the system’s internal energy and the product of pressure and volume of the system. It is a state function. State functions are those variables which depend on the state of the system and are independent of the path used i.e. whether the reaction is carried out in one step or in several steps the enthalpy change will remain the same. Entropy is also a state function.

Note: In these types of questions , convert temperature into kelvin and put the values in the formula. The entropy is also the measure of the molecular disorder or the randomness of the system.