The temperature of 2.00 mol ne(g) is increased from 25°c to 200°c at constant pressure. assuming the heat capacity of ne is 20.8 j/k·mol, calculate the change in the entropy of neon. assume ideal gas behavior. a.+19.2 j/kb.-7.68 j/kc.+7.68 j/kd.-19.2 j/k

a) + 19.2J/K

Explanation:

The parameters in this question are outlined as follows;

Number of moles (n)= 2

Initial temperature (T1) = 25°C + 273 = 298 K (Converting to Kelvin)

Final temperature (T2) = 200°C + 273 = 473 K (Converting to Kelvin)

Heat Capacity (Cp) = 20.8 J/K·mol

Change in entropy (ΔS) ?

The formular linking the parameters is given as;

ΔS =n * Cp * ln(T2/T1 )  (constant pressure)

Inserting the values into the equation, we have;

ΔS = 2 * 20.8 * ln (473/298)

ΔS = 41.6 * 0.462

ΔS = 19.2J/K

the dissolution of polymer can be thermodynamically described in 2 steps.

1 is the answer to this problem