For 1 mol of molecules randomly distributed among bulbs A, B, and C, use Boltzmann's formula to calculate the entropy of the state. If the number of microstates is 27, what is the entropy?

A reaction has ΔrH = -107 kJ mol^-1 and ΔrS = 285 J K^-1 mol^-1. At what temperature is the change in entropy for the reaction equal to the change in entropy for the surroundings?

Calculate ΔS°rxn for the reaction: 2NO(g) + O2(g) → 2NO2(g) given the standard molar entropies: S°(NO) = 210.7 J/mol·K, S°(O2) = 205.0 J/mol·K, S°(NO2) = 240.1 J/mol·K.

Calculate ∆S_rxn for the reaction 2NO(g) + O2(g) → 2NO2(g) given the following standard molar entropies: S°(NO) = 210 J/mol·K, S°(O2) = 205 J/mol·K, S°(NO2) = 240 J/mol·K.

If the change in entropy of the surroundings for a process is -326 J/K at 439 K and constant pressure, what is the heat flow (ΔH) absorbed by the system?

The entropy change associated with the expansion of one mole of an ideal gas from an initial volume of V_i to a final volume of V_f at constant temperature is given by the equation, ΔS = R ln (V_f/V_i). If V_i = 2.0 L and V_f = 4.0 L, what is the entropy change associated with the expansion?

The normal boiling point of water is 100.0 °C, and its molar enthalpy of vaporization is 40.67 kJ/mol. What is the change in entropy in the system in J/K when 39.3 grams of steam at 1 atm condenses to a liquid at the normal boiling point?

The standard molar entropy for Br₂(g) is 245.46 J/(mol·K) at 25°C. Given that ΔS° = 104.58 J/K for the dissociation of one mole of Br₂(g) into Br(g) at 25°C, find the standard molar entropy for Br(g) at 25°C.