Use the data to calculate the standard entropy change for the following reaction: 5. S°[Mt(s)] 43.2 J/K mol Mt(s) + ½ O2(g) → MtO(s) S°[O2(g)] = 305.1 J/K-mol S°[MtO(s)] 62.6 J/K mol a) -133.2 J/K b) -285.7 J/K c) 285.7 J/K d) 133.2 J/K

The element oxygen was prepared by Joseph Priestley in 1774 by heating mercury(II) oxide: HgO(s) → Hg() + 1/2O2(g), AH = 90.84 kJ/mol. Estimate the temperature at which this reaction will become spontaneous under standard state conditions. S'(Hg) = 76.02 J/K mol S(O2) = 205.0 J/K mol C S(HgO) = 70.29 J/K mol 11

What is the change in entropy, AS, for the following reaction? Use Table G in your book for values of standard entropies. Your answer should be in J/K mol. CaCO3(s) + 2 H'(aq) → → Ca² (aq) + H₂O(l) + CO2(g) O 264.9 J/K mol O 118.6 J/K mol 394.3 J/K mol 137.7 J/K mol 2

Using enthalpies of formation, calculate deltaH for the following reaction at 25°C. Also calculate deltaS for this reaction from standard entropies at 25°C. Use these values to calculate deltaG for the reaction at this temperature. Species  deltaHf(kJ/mol)  S(J/mol⋅K) CH3OH(l) –238.7 126.8 O2(g) 0 205.0 CO2(g) –393.5 213.7 H2O(l) –285.8 69.95 2CH3OH(l) +3O2(g) --- 2CO2(g) + 4H2O(l) deltaH =  kJ deltaS =  J/K deltaG =  kJ

Calculate AS°rxn for the following reaction. The S° for each species is shown below the reaction. N2H4(l) + H2(g) → 2 NH3(g) ings S°(J/(mol·K)) 121.2 130.7 192.8 O -59.1 J/K es O 311.0 J/K O 133.7 J/K O -133.7 J/K O 637.5 J/K

Estimate ΔG°rxn for the following reaction at 307 K.CH4(g) + 2 O2(g) → CO2 (g) + H2O (l) ΔH°= -890.4 kJ; ΔS°= -242.2 J/K +816.0 kJ +66.3 kJ -66.3 kJ -816.0 kJ -250 kJ

A reaction has an equilibrium constant (K) of 90.9.  If the entropy of this reaction is -69.1 J/mol K at a temperature of 280 K, what is the enthalpy of this reaction in kJ/mol?Report your answer to one decimal place. ΔG = ΔH - T ΔSΔG = -RT ln K

Determine the standard entropy of NO(g) given the following information: NO(g)+0,(g) → NO, (g) AS xn = -73.2 J/K Substance S° (J/mol · K) NO2(3) 240.0 O2(g) 205.0 NO(g) ? O -210.7 J/K O +210.7 J/K +108.2 J/K -108.2 J/K O +54.1 J/K