Question: 2. NO 2 is an intermediate in the industrial synthesis of nitric acid, millions of tons of which are produced each year for use primarily in the production of fertilizers.At higher temperatures it is a reddish-brown gas. 2NO + O2 yields N2O4. When equilibrium is reached, 58% of the N2O4 has decomposed to NO2. The vapor density is the mass of a volume of the mixture divided by the mass of an equal volume of H2 at . calculate the change in H for the reaction. So the addition of heat will favor endothermic reaction. Explanation: As the reverse reaction which is the formation of N2O4 is an exothermic reaction and the formation of NO2 is an endothermic reaction. C. spontaneous at low temperatures, but not at high temperatures. ... 2NO2(g) was established in a 1.00-liter vessel. NO + 1/2O2 yields NO2 and the change in H is -56 kJ. B. spontaneous at high temperatures, but not at low temperatures. At constant pressure, the reaction 2NO2(g) ↔ N2O4(g) is exothermic. Answer: The formation of the products is favored by the addition of heat. Note that the table for Alkanes contains Δ f H o values in kcal/mol (1 kcal/mol = 4.184 kJ/mol), and the table for Miscellaneous Compounds and Elements contains these values in kJ/mol. D. never spontaneous. chemistry. Any help is appreciated! The standard enthalpy (∆H rxn = -57.2 kJ) and the entropy (∆S rxn = -175.83 J) of reaction can be calculated from the following standard-state enthalpies of formation and standard-state entropies: NO2/N2O4 Equilibrium Demonstration . The reaction is endothermic, because heat is required to break the bonds of N2O4, thus producing NO2. N2O4 has stronger bonds than NO2, so it requires more energy (in the form of heat) in order to break the bonds. The reaction is A. always spontaneous. What . science What is the standard enthalpy change of the this reaction? The standard enthalpies of formation of NO2(g) and N2O4(g) 8and 2 kcal per mole respectively.the heat of dimerisation of NO2 in gaseous state is-Dear Shubham 2 Heating or cooling flasks of NO 2 and N 2 O 4 shifts the equilibrium between these two species. 10.0. N2O4 --> 2NO2; So the concentration of N2O4 decreases. and for the reaction. When more NO 2 is produced, the color of the gas inside the flask becomes darker brown. N2O4 yields 2NO2 and the change in H is +58 kJ . N2O4 rightarrow 2NO2 delta H degree f for N2O4 is 10. kj/mol delta H degree f for NO2 is 34 kj/mol The equilibrium system can be represented as. Nitrogen dioxide is a paramagnetic, bent molecule with C 2v point group symmetry Nitrogen dioxide is a chemical compound with the formula NO 2.It is one of several nitrogen oxides. Can someone please explain how to do this? 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