Use average bond enthalpies (linked above) to calculate the enthalpy change for the following gas-phase reaction. N2(g) + 2 H2(g) →N¿H(g) To analyze the reaction, first draw Lewis structures for all reactant and product molecules. Draw the reaction using separate sketchers for each species. Separate multiple reactants and/or products using the + sign from the drop-down arrow. Separate reactants from products using the → symbol from the drop-down menu. Remember to include nonbonding valence electrons in your Lewis structures.

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The gas hydrazine, N2H4, burns in oxygen like this:NHNHH H(g) + O O (g) N N (g) + 2OHH(g)a Count and list the bonds broken in this reaction.b Count and list the new bonds formed.c Calculate the total energy:i required to break the bondsii released when the new bonds form.(The bond energies in kJ / mole are: N2H 391;N2N 158; NN 945; O2H 464; O5O 498.)d Calculate the energy change in the reaction.e Is the reaction exothermic, or endothermic?f Where is energy transferred from, and to?g Comment on the suitability of hydrazine asa fuel.

What is the enthalpy change, Delta Hrxn, for the following reaction? 2 N2OH (s) + CO2 (g) → Na2CO3 (s) + H2O (I) Select one: a. – 2661.4 kJ b. + 171.9 kJ C. + 991.0 kJ d. – 597.5 kJ e. none of these f. +2661.4 kJ g. – 991.0 kJ h. – 171.9 kJ

part c

Calculate ΔH (in kJ/mol) for the reaction described by the equation. 6 NH3(g) + 5 O3(g) → 6 NO(g) + 9 H2O(l)

Use the table provided to estimate AH for the reaction O3 (g) + O (g) →2 O2 (g). Does this reaction consume or produce heat? Single Bond Energies (kJ/mol of bonds) N OS H. F Cl Br I Н 436 C 413 346 N 391 305 163 O 463 358 201 146 S 347 272 226 F 565 485 283 190 284 155 Cl 432 339 192 218 255 253 242 Br 366 285 201 217 249 216 193 I 299 213 201 278 208 175 151 Multiple Bond Energies (kJ/mol of bonds)_ C=C 602 C=N 615 C=O 799 C=C 835 CEN 887 C=O 1072 N=N 418 N=O 607 NEN 945 O=0 498

predict the enthalpy change for the reaction below using the standard molar enthalpy of formation data provided. 2 SO2+O2 -->2 SO3 SO2, ∆ Hf = -297 KJ/mol SO3, ∆ Hf = -396 KJ/mol a)-198 KJ/mol b)-99 KJ/ mol c)99 KJ/mol

What is the purpose of the n or x in the equation when performing enthalpy calculations?