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A: The change in Gibbs free energy = -2808 kJ mol-1 Mass of the person = 65 kg
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- In the thermodynamic definition of a spontaneous process, why is it important that the phrase “continuous intervention” be used rather than just “intervention?”A container with 53 g of a certain liquid (c = 4158 J/kg · °C, Lv=2204 kJ/kg) at 21 °C is heated up until all the liquid evaporates at 110°C. What is the change in entropy of the substance in J/K in this process?Two moles of liquid water at 25 ° C is placed in a freezer having a temperature of – 10 ° C. Calculate the change in entropy.Cp,m for liquid water = 75.3 J K-1 mol-1Cp,m for ice = 37.7 J K-1 mol-1For water, ΔΗfusion = 6.01 kJmol-1
- Compound ∆Hf (kJ/mole) ∆S (J/mole K) CO2(g) –393.5 +213.8 CO2 (aq) –413.8 +117.6 N2O4 9.16 +304.4 NO2 33.2 240.1 CaCO3 –1207.6 91.7 CaO –634.9 +38.1 I2 (g) 62.42 260.69 HI(g) 26.5 206.6 H2 (g) 0 130.7 (a) For the following reactions, using the provided ∆H and ∆S data, determine whether each one would be spontaneous or nonspontaneous at 25°C CO2(g) à CO2(aq) N2O4(g)-------- à2 NO2(g) CaCO3(s) ----à CaO (s) + CO2(g) H2 (g) + I2(g)---- à 2 HI (g)Consider the reaction:2C2H6(g) + 7O2(g)4CO2(g) ---------> 6H2O(g)Using standard absolute entropies at 298K, calculate the entropy change for the system when 1.69 moles of C2H6(g) react at standard conditions. S°system = _______ J/KWhat is the standard free-energy change for the following reaction: 2C6H6 (l) + 15O2 (g) 12CO2 (g) + 6H2O (l) at 25 0C? Values of delta Gf of substances at standard conditions are as follows: Benzene = 124.5 kJ/mol, Carbon dioxide = -394.4 kJ/mol, Oxygen gas = 0.0 kJ/mol, and Liquid water = -237.2kJ/mol A. -64.05 kJB. +640.5 kJC. -6405 kJD. None of the above
- Use the information give below to calculate the value of the standard molar entropy, So m of a solid K2O ( in J/mole x K) 2 K2O (s) ---> 4 K (s) + O2 (g) DeltaSo m = +275 J/K So m [K(s)] = +65 J/Mole x K Som [O2 (g)] = + 205 j/mole x kConsider: CO(g, 198, 29.4) + 2 H2(g, 29, 28.8) → CH3OH(g, 240, 44) What is its reaction entropy at 320 K? Given in order in parentheses are the phase, S° (J K-1 mol-1), and Cp,m (J K-1 mol-1) of each compound at 300 K.For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all species. For the reaction N2(g)+3H2(g)↽−−⇀2NH3(g) the standard change in Gibbs free energy is Δ?°=−72.6 kJ/mol. What is ΔG for this reaction at 298 K when the partial pressures are ?N2=0.450 atm, ?H2=0.200 atm, and ?NH3=0.800 atm?
- Consider the reaction: Ca(OH)2(aq)+2HCl(aq)----> CaCl2(s)+2H20(l) Using standard thermodynamic data at 298 K, calculate the entropy change for the surroundings when 1.73 moles of react at standard conditions.Part A) Consider the reactionC2H4(g) + H2O(g)---->CH3CH2OH(g)Using standard thermodynamic data at 298K, calculate the entropy change for the surroundings when 1.70 moles of C2H4(g) react at standard conditions. ΔS°surroundings = ________J/K Part B) NH4NO3(aq)---->N2O(g) + 2H2O(l)Using standard thermodynamic data at 298K, calculate the entropy change for the surroundings when 2.44 moles of NH4NO3(aq) react at standard conditions. S°surroundings = ____________J/KUsing the data below, the reaction: 2SO3(g) → 2S(s, rhombic) + 3O2(g) is nonspontaneous. Thermodynamics Quantities for Selected Substances at 298.15 K (25⁰C) Substance ∆H⁰f (kJ/mol) ∆G⁰f (kJ/mol) S (J/K-mol) O2(g) 0 0 205.0 Sulfur(s, rhombic) 0 0 31.88 SO2(g) -269.9 -300.4 248.5 SO3(g) -395.2 -370.4 256.2 TRUE OR FALSE