Consider the reaction: 2CO(g) + 2NO(g)2CO2(g) + N2(g) Using standard absolute entropies at 298K, calculate the entropy change for the system when 1.72 moles of CO(g) react at standard conditions.      S°system =  J/K

Calculate the change of the entropy of the system in J/K for the following phase transition: vaporization of 159.2 g propanol The molar mass of n-propanol (C3H7OH) is  60.095 g/mol; the enthalpy of vaporization of n-propanol is 47.5 kJ/mol; the boiling point of n-propanol is 97.7°C  Group of answer choices 128 -486 -339 1280 0.3393

Given the following reaction, calculate the standard entropy at 25oC. 2NO(g) + O2(g) 2NO2(g) (Sof NO2 = 240.1 J mol-1K-1; Sof NO = 210.8 J mol-1K-1; Sof O2 = 205.1 J mol-1K-1)

Consider the reaction: NH4Cl(aq) →→→→NH3(g) + HCl(aq) Using standard thermodynamic data at 298K, calculate the entropy change for the surroundings when 1.90 moles of NH4Cl(aq) react at standard conditions. AS° surroundings = J/K

For a particular chemical reaction H = 6.8 kJ and S = –29 J/K. Under what temperature condition is the reaction spontaneous?

3. What change will increase the entropy of the system? Group of answer choices liquid to solid solid to gas gas to liquid gas to solid 2.ΔSsyst>0 for the following reaction: Group of answer choices A,  2NO (g) + O2(g) → 2NO2(g) B, HCl (g) + NH3(g) → NH4Cl (s) C, C3H8(g) + 5 O2(g) → 3CO2 (g) + 4 H2O (g) D, 2N2 (g) + 3H2(g) → 2NH3(g) E,  Pb2+(aq) + 2Cl-(aq) → PbCl2 (s)

Calculate the change in the molar entropy of solid sodium chloride at constant pressure (1.00 bar) during heating from 0°C to 400°C. The constant-pressure molar heat capacity of NaCl(s) – which is not constant - takes the following form. 45.94 J 16.32 x 10-3 J T. Cp,m3 K mol K2 mol