9. The enthalpy of decomposition of gaseous water to oxygen and hydrogen at 298 K and 1 atm is 241.75 kJ/mol. Cal...
6. Calculate the entropy change when 2 moles of gaseous water are formed at 100°C and 1 atm from hydrogen and oxygen gas at the same temperature. H2(g) = 130.57 J/K Standard molar entropy: H2O(g) = 188.72 J/K O2(g) = 205.04 J/K Constant volume molar heat capacity: H2O(g) = 25.3 J/ K O 2(g) = 21.1 J/K Constant pressure molar heat capacity: H2O(g) = 33.6 J/K O2(g) = 29.4 JK H2(g) = 20.5 JK H2(g) = 28.8 J/K
4. The standard enthalpy of formation of NH3 (g) is -46.11 kJ mol-' at 298 K. Given the heat capacity data below and the data in Problem 2, calculate the standard enthalpy of formation at 1200 K Cp.m (H2 (9))/ J mol K-1 = 29.1 - (0.84 x 10- K-)T Cpm (N2 (g))/ J mol K-1 = 26.98 +(5.9 x 10-'K-!)T
When one mole of gaseous hydrogen peroxide, H2O2, is made from hydrogen and oxygen gases, the enthalpy change is –136 kJ. Which of the following correctly represents the thermochemical equation? i. H2(g) + O2(g) → H2O2(g) + 136 kJ ii. H2(g) + O2(g) + 136 kJ → H2O2(g) iii. H2(g) + O2(g) → H2O2(g) ΔH = –136 kJ iv. H2(g) + O2(g) → H2O2(g) ΔH = +136 kJ A.i only B.ii only C.iii only D.i and iii E.ii and iv
For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all species. For the reaction 2NO(g)+O2(g)↽−−⇀2NO2(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 ?NO=0.500 atm , ?O2=0.400 atm , and ?NO2=0.750 atm ?
For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all species. For the reaction 2NO(g)+O2(g)↽−−⇀2NO2(g) 2 NO ( g ) + O 2 ( g ) ↽ − − ⇀ 2 NO 2 ( g ) the standard change in Gibbs free energy is Δ?°=−72.6 kJ/mol Δ G ° = − 72.6 kJ/mol . What is ΔG for this reaction at 298 K when the partial pressures are ?NO=0.300 atm P NO...
For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all species. For the reaction C2H(g)H2(g)2 CH (g) 4 the standard change in Gibbs free energy is AG° -69.0 kJ/mo. What is AG for this reaction at 298 K when the partial 0.400 atm, PH Рс,н, 0.450 atm, and PCH, = 0.600 atm? pressures are kJ/mol AG =
Thermodynamic Quantities for Selected Substances at 298.15 K (25 °C) Substance AHºf (kJ/mol) AG°f (kJ/mol) S (J/K-mol) Oxygen O2 (g) H20 (1) 0 -285.83 205.0 69.91 -237.13 10 CHCOOH 0 Sulfur S (s, rhombie) 0 SO2(g) -269.9 SO3(g) -395.2 -300.4 31.88 248.5 256.2 OM-370.4 FASO for the decomposition of gaseous sulfur trioxide to solid elemental sulfur 3. The value of ASº for the d and gaseous oxygen, 2503 (g) → 28 (s, rhombie) + 302 (g) J/K. mol. (show your...
For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all species. For the reaction N (8) + 3H2(g) + 2NH3(g) the standard change in Gibbs free energy is AGⓇ = -72.6 kJ/mol. What is AG for this reaction at 298 K when the partial pressures are PN, = 0.200 atm, PH, = 0.450 atm, and PNH, = 0.750 atm? AG= L kJ/mol AG= kJ/mol
1. 0.25-mol ice at -5 °C is mixed with n-mol hot water initially at 45 °C in an isobaric adiabatic calorimeter at 1 atm. The final temperature of the mixture becomes 10 °C, and the ice is melted into liquid water. Assume the density of ice is 0.917 g/mL and the density of water is 1.000 g/mL. The molar heat capacity Com of liquid water is 75.291 J/mol K, the molar heat capacity Cm of ice is 38.09 J/mol-K, and...
Ethanol melts at 159K and boils at 351K. The enthalpy of fusion is 5.02 kJ/mol, the enthalpy of vaporization is 35.56 kJ/mol, and the molar mass is 46.07 g/mol. The specific heats of solid ethanol is 0.97 J/g-K, for liquid ethanol it is 2.3 J/g-K, and for gaseous ethanol it is 1.9 J/g-K. How much heat (kJ) is needed to convert 215 g of liquid ethanol at 160 K to gaseous ethanol at 713 K?