Calculate ΔH°R for: (please show all work)
2SO2 (g) + N2O4 (g) --> 2SO3 (g) + 2NO (g)
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Calculate ΔH°R for: (please show all work) 2SO2 (g) + N2O4 (g) --> 2SO3 (g) +...
Calculate ΔH°F for C7H14 (l) Please show all work and use ΔH°R = Σ ΔH°F (products) - Σ ΔH°F (reactants) Given: 2 C7H14 (l) + 21 O2 (g) --> 14 CO2 (g) + 14 H2O (l) ΔH°R = -8135 kJ/2 mol c7H14
Consider this reaction at equilibrium 2SO2(g)+O2(g)⇌2SO3(g)ΔH=−198kJ Which of these changes would cause PSO2 to increase? Decreasing the temperature Increasing the volume of the container Increasing the total pressure Adding O2(g)
****please include all the formulas used AND show ALL your work for the following question (preferably on a sheet of paper). I'm really struggling with this concept.**** Given the thermochemical equation 2SO2(g) + O2(g) → 2SO3(g) ΔH = −198.2 kJ/mol, calculate the heat evolved when 87.9 g of SO2 (molar mass = 64.07 g/mol) is converted to SO3. please include all the formulas used AND show ALL your work for the following question. I'm really struggling with this concept.
SO3(g) decomposes to produce SO2(g) and O2(g), as represented by 2SO3(g)⇄2SO2(g)+O2(g) ΔH°=180kJ/molrxn Under what temperature conditions will the reaction be thermodynamically favored: high temperatures, low temperatures, all temperatures, or no temperatures? Justify your answer in terms of the change in enthalpy and the change in entropy during the reaction.
The equilibrium constant, Kp, for the following reaction is 2.74 at 1150 K. 2SO3(g) 2SO2(g) + O2(g) If ΔH° for this reaction is 198 kJ, what is the value of Kp at 1270 K? Kp =
The equilibrium constant, Kp, for the following reaction is 2.74 at 1150 K. 2SO3(g) 2SO2(g) + O2(g) If ΔH° for this reaction is 198 kJ, what is the value of Kp at 1260 K? Kp= ?
Using Hess’s Law to Calculate ΔH Calculate ΔH for 2 NO(g) + O2(g) → N2O4(g) using the following information: N2O4(g)2 NO(g) + O2(g)→→2 NO2(g)2 NO2(g)ΔHΔH==+57.9 kJ−114.1 kJ Calculate for using the following information: Select one 2.7 kJ -55.2 kJ -85.5 kJ -171.0 kJ +55.2 kJ
Use the equilibrium constants for the following reactions at 700 °C 2SO2(g) + O2(g) 2SO3(g) K1 = 4.8 2NO(g) + O2(g) 2NO2(g) K2 = 16 to determine the equilibrium constant for the following reaction. SO 3( g) + NO( g) SO 2( g) + NO 2( g)
Calculate ΔG°R for: (using: ΔG°R = ΔH°R - T ΔS°R ) (Standard T and please show all work!) 2KClO3 (s) --> 2KCl (s) + 3O2 (g)
Consider the reaction: 2SO2(g) + O2(g)2SO3(g) Using standard absolute entropies at 298K, calculate the entropy change for the system when 2.11 moles of SO2(g) react at standard conditions. S°system = J/K