Calculate the standard Free Energy change for the following two reactions, using Gof data only. a) H2(g) + Br2(l) à 2 HBr(g) b) 2 C2H6(g) + 7 O2(g) à 4 CO2(g) + 6 H2O(l)

If Gibbs free energy (at standard conditions) of a reaction is -22.8 kj/mol, what is the equilibrium constant of the reaction?

hello, i need help with this question  It is quite common for a solid to change from one solid state structure to another at a temperature below its melting point.For example, sulfur undergoes a phase change from the α-orthorhombic form (S8; density≅2.07 g/cm3) to the β-monoclinic form (S8; density≅2.00 g/cm3) as it is warmed above 95.3 °C.Assuming that ΔH for this phase change is 0.220 kJ/mol, calculate ΔS for this phase change.

Calculate the standard enthalpies of formation of (a) KCIO3(s) with the following information: K(s) + 1/2 Cl₂(g) KCI(s) 2 KCIO3(s)→2 KCl(s) + 3 O₂(g) ArH=-436.75 kJ mol-¹ A,H-89.4 kJ mol-¹ (b) NaHCO3(s) with the following information: Na(s) + 1/2 O₂(g) + 1/2 H₂(g) → NaOH(s) C(s) + O₂(g) → CO₂(g) NaOH(s) + CO₂(g)→→NaHCO3(s) A,H-425.61 kJ mol-¹ ArH=-393.51 kJ mol-¹ A,H= -127.5 kJ mol-¹

also, Change in Gibbs Free energy Reaction Spontaneity

Given the heat of formation of the following compounds:                 CO2(g)                ΔfH° = -393.5 kJ/mol                 H2O(l)                 ΔfH° = -285.9 kJ/mol                 CH3OH(l)          ΔfH° = -238.6 kJ/mol   What is the value of ΔrH° for the reaction:                 CH3OH(l) + 3/2 O2(g) → CO2(g) + 2 H2O(l)

Using the table of bond enthalpies in your textbook, predict ArH for the following reaction. Express your answer in kJ/mol. HCECH + 2 H2 → H3C-CH3

2. Please calculate the standard enthalpy of reaction (AHrxn, in kJ/mol) for the preparation of nitrous acid, HNO2, using the thermodynamic data given below. Preparation of nitrous acid: HCl(g) + NaNO2(s) → HNO2(1) + NaCl(s) 2NaCl(s) + H₂O(l) → 2HCl(g) + Na₂O(s) NO(g) + NO₂(g) + Na2O(s) → 2NaNO2 (s) NO(g) + NO₂(g) → N₂O(g) + O₂(g) 2HNO2(1)→ N₂O(g) + O2(g) + H₂O(g) H₂O(1)→ H₂O(g) ΔΗ = 507.31 kJ/mol AH = -427.14 kJ/mol AH = - 42.68 kJ/mol 34.35 kJ/mol ΔΗ ΔΗ = 44.012 kJ/mol =

Calculate ΔH° in kilojoules for the following reaction, the preparation of the unstable nitrous acid, HNO2.   Use the following thermochemical equations:

Using bond energies from the table, estimate ΔH for the reaction below. The OH group on the product side is attached to a carbon.CH2=CH2(g) + H2O(g) ↔ CH3CH2OH(g) Bond Energies, kJ/mol Single Bonds   H C N O S F Cl Br I H 432                 C 411 346               N 386 305 167             O 459 358 201 142           S 363 272 --- --- 286         F 565 485 283 190 284 155       Cl 428 327 313 218 255 249 240     Br 362 285 243 201 217 249 216 190   I 295 213 --- 201 --- 278 208 175 149 Multiple Bonds C=C 602 C=N 615 C=O 799 CºC 835 CºN 887 CºO 1072 N=N 418 N=O 607 S=O (in SO2) 532 NºN 942 O2 494 S=O (in SO3) 469