[SO2] = 300KJ
[SO3] = -200KJ
=
[produc] -
[reactant]
=
[SO3] -
[SO2]
= -200 - 300 = - 500 KJ/mol
Option A is the right Answer.
Given these equations SO_2(g) rightarrow O_2(g)+ S(s) DeltaHdegree = +300 kJ 2SO_2(g) + O_2(g) rightarrow 2SO_3(g)...
Use the standard reaction enthalpies given below to determine Delta H_rxn degree for the following reaction: 2 S(s) + 3 O_2(g) rightarrow 2SO_3(g) Delta H_rxn degree Given: SO_2(g) rightarrow S(s) + O_2(g) Delta H_rxn degree = +296.8 kJ 2SO_2(g) + O_2(g) rightarrow 2 SO_3(g) Delta H_rxn degree = -197.8 kJ Name those compounds? Li_2SO_3 Al_2S_3 P_2O_3 COBr_2-6H_2O
At a certain temperature, the following reactions have the equilibrium constants shown. S(s) + O_2(g) rightwardsharpoonoverleftwardsharpoon SO_2(g) K_c = 10^2S(s) + 3O_2(g) rightwardsharpoonoverleftwardsharpoon 2SO_2(g) k_ = 9.8 times 10^Calculate the equilibrium constant, K_c. for the following reaction at that temperature. 2SO_2(g) + O_2(g) rightarrow 2SO_3(g)
Calculate the enthalpy of formation of SO_2(g) from the standard enthalpy changes of the following reactions: SO_2(g) + O_2(g) rightarrow 2 SO_3(g) Delta H degree _r times n = - 196 kJ S(s) + 3 O_2(g) rightarrow 2 SO_3(g) Delta H degree _r times n = - 790 kJ S(s) + O_2(g) rightarrow SO_2(g) Delta H degree _r times n = Number _______ kJ
At a particular temperature, 12.0 mol of SO_3 is placed into a 3.0-L rigid container, and the SO_3 dissociates by the reaction| 2SO_3(g) 2SO_2(g) + O_2(g) At equilibrium, 3.0 mol of SO_2 is present. Calculate K_c for this reaction. 1.5 0.11 0.72 0.056 0.17 0.0035
a. write the equilibrium expression and for the balanced reaction: 2 SO_3 (g) leftarrow and rightarrow 2 SO_2 (g) + O_2 (g). b. Given the following information: [SO_3] = 0.0255M, [SO_2] = 1.08M, and [O_2] = 1.45M at equilibrium calculate the equilibrium constant K. The oxidation of ammonia is a reversible exothermic reaction that proceeds as follows: 4 NH_3(g) + 5 O_2(g) leftarrow rightarrow 4 NO(g) + 6 H_2O(g) + heat For each situation described in the table, indicate the...
Use the standard reaction enthalpies given below to determine Delta H degree _rxn for the following reaction: 2 S(s) + 3 O_2(g) rightarrow 2 SO_3(g) Delta H degree _rxn = ? Given: SO_2(g) rightarrow S(s) + O_2(g) Delta H degree _rxn = +296.8 kJ 2 SO_2(g) + O_2(g) rightarrow 2 SO_3(g) Delta H degree rxn = -197.8 kJ Show all your work!
Use the Delta H degree_f and Delta H degree_rxn information provided to calculate Delta H degree_f for SO_3 (g): Delta H degree_f (kJ/mol)SO_2(g) + O_2(g) rightarrow SO_3 (g) Delta H degree_rxn = -198 kJ SO_2(g) - 297
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Help would be greatly appreciated
Consider the following reaction: S(s, rhombic) + O_2 (g) rightarrow SO_2(g) Use standard heats of formation from Gum Dahl 'Chemical Principles' 7th ed. Appendix Four pp. A19 - A22 How much heat is evolved when 2.886 times 10^2 g of S(s, rhombic) is burned in excess oxygen. Answer to 4 sig figs. How much heat is evolved when 3.000 times 10^2 g of SO_2(g) is produced from the combustion of S(s, rhombic). Answer to 4...