Calculate ΔS and ΔG for the evaporation of 1 mol water at T = 100°C and p = 1 atm. The latent heat of evaporation of water is 9.7 kcal/mol.
Calculate ΔS and ΔG for the evaporation of 1 mol water at T = 100°C and...
For a particular reaction at 205.1205.1 °C, ΔG=−45.90 kJ/molΔG=−45.90 kJ/mol, and ΔS=395.61 J/(mol⋅K)ΔS=395.61 J/(mol⋅K). Calculate ΔG for this reaction at −6.1−6.1 °C.
Please show all work and explanations! Calculate ΔE, ΔS, ΔG, Q and W for the vaporization of 3.00 moles of liquid water to form water vapor at 100°C and 1.00 atm pressure. The standard molar enthalpy of vaporization of water is 40.67 kJ/mol. The density of liquid water at 100°C is 0.958 g/cm3 . Assume that the water vapor is an ideal gas, but be careful – the initial state is liquid water, so this is not simply an ideal...
For the sublimation of CO2 at 0 C and 1 atm: a) ΔS<0, ΔG<0 b) ΔS>0, ΔG<0 c) ΔS>0, ΔG>0 d) ΔS<0, ΔG>0 e) ΔS>0, ΔG=0
At 100°C, 1.00 mol of liquid water is allowed to expand isothermally into an evacuated vessel of such a volume that the final pressure is 0.500 atm. The amount of heat absorbed in the process was found to be 30.0 kJ/mol. Assume ideal behaviour of the gas. What are w, ΔU, ΔH, ΔS, and ΔG Data: ΔvapH = 40600 J/mol (at 1.00 atm) Hint: Employ a step-wise approach to be able to use the given data at the provided pressure.
Why a Substance Can Be a Liquid at Room Temperature? Calculate ΔS∘total for the evaporation of water at 25∘C. H2O (l) ⇄ H2O (g) ΔH∘f (kJ/mol) Sm∘ (J/mol*K) H2O (l) - 285.830 69.91 H2O (g) - 241.818 188.83 ΔS∘ system? ΔS∘surroundings? ΔS∘total?
For the conversion of ice to water at 0°C and 1 atm, ΔG is zero, ΔH is positive, and ΔS is positive. ΔG is zero, ΔH is positive, and ΔS is negative. ΔG is negative, ΔH is positive, and ΔS is negative. ΔG is positive, ΔH is zero, and ΔS is positive.
For a particular reaction at 209.8 °C, ΔG = -318.09 kJ/mol, and ΔS = 994.40 J/(mol·K). Calculate ΔG for this reaction at -58.2 °C.
For a particular reaction at 134.8 °C, ΔG = -1319.75 kJ/mol, and ΔS = 863.35 J/(mol·K). Calculate ΔG for this reaction at -79.1 °C.
For a particular reaction at 139.3 °C, ΔG = 354.61 kJ/mol, and ΔS = 658.46 J/(mol·K). Calculate ΔG for this reaction at -55.9 °C.
A process at constant T and P can be described as spontaneous if ΔG < 0 and nonspontaneous if ΔG > 0. Over what range of temperatures is the following process spontaneous? Assume that gases are at a pressure of 1 atm. (Hint: Use the data below to calculate ΔH and ΔS [assumed independent of temperature and equal to ΔH° and ΔS°, respectively] and then use the definition of ΔG.) PCl3(g) + Cl2(g) → PCl5(g) ΔHf° (kJ mol-1) -287.0 -374.9...