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.

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?

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 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.

What is the change in entropy of the surroundings (ΔSsurr) for the reaction of 2 SO2(g) + O2(g) → 2 SO3(g) at 25.0 °C, given that ΔH = -196 kJ?

Calculate the change in entropy (ΔS) that occurs in a system when 1.50 mol of isopropyl alcohol melts at its melting point of -89.5°C, given that the enthalpy of fusion (ΔH_fus) is 5.37 kJ/mol.