Using average bond enthalpies (linked above), estimate the enthalpy change for the following reaction: C2(g) + F2(g)–2CIF(g) kJ

Based on the bond energies for the reaction below, what is the enthalpy of the reaction, in kJ? H₂(g) + N₂(g) + 2 C(g) → 2 HCN(g)

Hess's Law is a useful way for chemists to predict the enthalpy change for a reaction. Use your understanding of energy changes to explain how Hess's Law works. Use the following example as part of your explanation (but you don't have to solve it!). 8. How can Hess's law be applied to determine the enthalpy change for the decomposition of potassium bicarbonate: 2 KHCO, (9) – K,CO; (s) + H,O () + CO2 (2) AH = -963 kJ (1) K (9) + ½ H, (e) Ce +0, (9)→ KHCO; (5) 2 (g) AH = -1150 kJ (2) 2K (9) + C + 02 (e) → K,C03 (6) AH = -242 kJ (3) H2() + ½ O2() H,O (g) AH = -394 kJ (4) C (6)+02 (g) - CO2 (2)

Suppose there is an element X which occurs naturally as X2(g).X2(g) + 2O2(g) → X2O4(g)X2O4 has a structure ΔHof of O(g) is 249 kJ/molΔHof of X(g) is 470.5 kJ/molΔHof of X2O4(g) is 11 kJ/molThe X-X single bond energy is 148 kJ/molUse the above data to estimate the average  bond energy in X2O4. Give your answer to the nearest 1 kJ/mol.

How did we get 807kJ from question a？how did we get 128kJ for b ？is there a step by step explanation？

Calculate the standard enthalpy change for the following reaction: CH4(g) + 2 O₂(g) → CO₂(g) + 2 H₂O(g) O-243 kJ/mol O 188 kJ/mol O 166 kJ/mol O-802 kJ/mol O-166 kJ/mol

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

Given the following reactions, what is the overall enthalpy change for the following reaction? N H 3 ( g ) + H C l ( g ) ⟶ N H 4 C l ( s ) Reaction ΔHo (kJ) N 2 ( g ) + 3 H 2 ( g ) ⟶ 2 N H 3 ( g ) -92 H 2 ( g ) + C l 2 ( g ) ⟶ 2 H C l ( g ) -185 N 2 ( g ) + 4 H 2 ( g ) + C l 2 ( g ) ⟶ 2 N H 4 C l ( s ) -629

Use the molar bond enthalpy data in the table to estimate the value of Δ?∘rxn for the equation   NH3 (g) + 2 O2 (g) --> HNO3 (g) + H20 (g)  Average molar bond enthalpies. (?bond) Bond ??⋅???−1 Bond ??⋅???−1 O−H 464 C≡N 890 O−O 142 N−H 390 C−O 351 N−O 201 O=O 502 N=N 418 C=O 730 N=O 607 C−C 347 F−F 155 C=C 615 Cl−Cl 243 C≡C 811 Br−Br 192 C−H 414 H−H 435 C−F 439 H−F 565 C−Cl 331 H−Cl 431 C−Br 276 H−Br 368 C−N 293 H−S 364 C=N 615 S−S 225

Use the molar bond enthalpy data in the table to estimate the value of Δ?∘rxn for the equation   NH3(g)+2O2(g)⟶HNO3(g)+H2O(g)