Use the given K’s below determine Ktot for the following reaction:
4 SO3(g) → 4 S(s) + 6 O2(g)
Ktot = ?
Given:
SO2(g) → S(s) + O2(g)
K1 = 2.9 x 10-3
2 SO2(g) + O2(g) → 2 SO3(g)
K2 = 7.5 x 104
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Use the given K’s below determine Ktot for the following reaction: 4 SO3(g) → 4 S(s)...
Use the standard reaction enthalpies given below to determine ΔH°rxn for the following reaction: 4 SO3(g) → 4 S(s) + 6O2(g) ΔH°rxn = ? Given: SO2(g) → S(s) +O2(E) ΔH°rxn = +296.8 kJ 2 SO2(g) + O2(g) → 2SO3(g) ΔH°rxn = -197.8 kJ-494.6 kJ -692.4 kJ -791.4 kJ 1583 kJ 293.0 kJ
E) - 03. 9) Use the standard reaction enthalpies given below to determine AHºrxn for the following reaction: AHºrxn = ? 4 S(s)+6 O2() → 4 SO3(e) Given: SO2(g) → S(s) + O2(e) 2 SO2(8)+O2(g) - 2 SO3(8) AHºrxn = 1296.8 kJ AHºrxn=-197.8 kJ D) -791.4 kJ E) 1583 kJ C) -1583 kJ A) -494.6 kJ B) -692.4 kJ
Given the following balanced equation, determine the rate of reaction with respect to (SO3). If the rate of Oz loss is 3.56x10 M/s, what is the rate of formation of SO3? 2 SO2 (g) + O2(g) - 2 SO3(g)
s(s) + 3/2 O2 (g) = SO3
15. (6 pts) Given the data below, calculate the ΔΗ,xn for the reaction: AH -296.1 kJ S (s) + O2 (g) → SO2 (g) 2SOs (g)
(10) 5. Use the given reactions and their enthalpies to determine the AHºrxn for the following reaction: 2 S(x) + 3 O2(g) → 2503(g) Hºrxn - ? Given Reactions and their Standard Enthalpies of Reaction: SO2(g) - S(s) + O2(g) 2 SO2(g) + O2(g) 2 S03(g) AHºrxn = +296.8 kJ Hºrxn = -197.8 kJ (10) 6. Use standard enthalpies of formation (AH°f) to determine AHºrxn for the reaction below. 2 CH3OH(1) + 3 02(g) → 2 CO2(g) + 4H2O(g)
Given the following reactions: 2 S (s) + 3 O2 (g) ⟶ 2 SO3 (g) ΔH1= LaTeX: -− 790 kJ S (s) + O2 (g) ⟶ SO2 (g) ΔH2= LaTeX: -−297 kJ What is the enthalpy change of the following reaction? 2 SO3 (g) ⟶ 2 SO2 (g) + O2 (g) ΔH3=?
52) Use the standard reaction enthalpies given below to determine AHryn for the tonowe reaction P4() + 10 C12(e) → 4PC15(s) Hºrxn = ? Given: PC15(s) → PC13(g) + Cl2(e) AHørxn = +157 kJ P4(B) + 6 Cl2(e) → 4 PC13(g) AH*rxn=-1207 kJ A) -1835 kJ B) -1364 kJ C) -1050. kJ D) -1786 kJ E) -2100. kJ 53) Use the standard reaction enthalpies given below to determine AHørxn for the following reaction 4 SO3(e) — 4 S(s) + 6...
7 Coleulate Kt Given the following data: 4. (Equation 1) S(s) +3/202(g) - SO3(g) AG= - 371 kJ slsb to gts2 gniwollot od lo do09 rw onimtsbThan 24 HA To (Equation 2) 2SO2(g)+ O2(g)2 SO3(g) AG°= - 142 kJ SO2(g) Calculate AG° for the goal equation S(s) +O2(g) 008 Is this reaction spontaneous? 00 02T 00 noitons gaivollot slt To doc9 10l 2410
Calculate heat for the following reaction to produce sulfur dioxide, S(3) + O2(g) = SO2(E) given the thermochemical equations below. 2 S(s) + 3 O2(g) =2 SO3(g) AH° = -791.5 kJ 2 SO2(g) + O2(g) = 2 SO3(g) AH° = -197 9 kJ Show all work and calculate to the correct number of sig figs.
3. Consider the following reaction: 2 SO2 (g) + O2 (g) → 2 SO3 (g) AH.x = -197.6 kJ a. If 285.3 g of SO2 is allowed to react with 158.9 g of O2, what is the limiting reactant and theoretical yield of SO3 in liters if the reaction is performed at 315 K and 50.0 mmHg? How much of each reactant remains at the end of the reaction? [10] LR: SO TY: SO2 remaining: O2 remaining: Imol soa 64.000log...