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?

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.

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.

Which of the following values represents the standard entropy change (ΔS°) for the vaporization of diethyl ether at its boiling point?

What is the change in entropy (∆S) when 1.32 g of propane (C3H8) at 0.100 atm pressure is compressed by a factor of five at a constant temperature at 20°C? Assume that propane behaves as an ideal gas. (a) ∆S = +13 J/K(b) ∆S = -13 J/K (c) ∆S = - 0.40 J/K(d) ∆S = + 0.40 J/K