The thermodynmaic state of gas changes configuration from one with 3.8 * 10¹⁸ multiplicity to one with 7.9 * 10¹⁹ microstates. The Boltzmann constant is 1.38 *10^-²³ J/K. The change in entropy is: A) $\Delta$ S = 0 B) $\Delta$ S = 1.04 *10^-²³ J/K C) F$\Delta$ S = -1.04 *10^-²³ J/K D) $\Delta$ S = 4.19 *10^-²³ J/K E) $\Delta$ S = -4.19 *10^-²³ J/K

Question

Quizplus · Accepted Answer

The change in entropy (ΔS) is calculated using the formula ΔS = k * ln(W_final/W_initial), where k is the Boltzmann constant, W_final is the final multiplicity, and W_initial is the initial multiplicity. Substituting the given values, ΔS = 1.38 x 10^-23 J/K * ln(7.9 x 10^19 / 3.8 x 10^18) = 4.19 x 10^-23 J/K.

The Thermodynmaic State of Gas Changes Configuration from One with 3.8