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.

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.

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?

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

Magnesium m#etal has ΔHfusion = 9.037 kJ>mol and ΔSfusion = 9.79 J>1K mol2. What is the melting point of magnesium in °C? (LO 11.4)(a) 0.923 °C (b) 923 °C(c) 650 °C (d) 1.08 * 103 °C