Given H2S(9)+3F2(9) – SF4(9)+2HF(9) AHbona (H-S)=+347 kJ/mol AH bond(F-F)=+155 kJ/mol AH bond(S-F)=+327 kJ/mol AH bona(H-F)=+567 kJ/mol...
N2(8) + 3F2(g) → 2 NF3() AH 298 = - 264 kJ mol-'; AS98 = - 278 J K-'mol-' The following questions relate to the synthesis reaction represented by the chemical equation in the box above. a. Calculate the value of the standard free energy change, AG 298. for the reaction. b. Determine the temperature at which the equilibrium constant, Keg, for the reaction is equal to 1.00. (Assume that Hº and AS are independent of temperature.) c. Calculate the...
Using bond enthalpies (given as Average Bond Energies in the Data Sheet) estimate the enthalpy change (ΔH, heat of reaction) for the following gas-phase reaction. (The bond energy value for S−C is 259 kJ mol-1 and that for S−H is 339 kJ mol-1.) HS CH2CH2 SH + 2HF F CH2CH2 F + 2 HSH.
For the reaction: H2(g)+C2H4(g)-->C2H6(g) Bond & Bond Enthalpy H-H 436.4 kJ/mole C-H 414 kJ/mol C-C 347 kJ/mol C=C 620 kJ/mol Substance & delta Hf H2 0 C2H4 52.3 C2H6 -84.7 (a) estimate the enthalpy of reaction, using the bond enthalpy values from the table in kJ/mol (b) Calculate the enthalpy of reaction, using standard enthalpies of formation
Given the bond energies (in kJ/mol) of the following bonds: F–F (155), F–Cl (193), and Cl–Cl (243), estimate the molar enthalpy of formation of ClF(g), that is find ∆H for the following reaction ½Cl2(g) + ½F2(g) → ClF(g) A. 209 kJ/mol B. -50. kJ/mol C. –8 kJ/mol D. –209 kJ/mol E. 8 kJ/mol
Given the following standard enthalpy of formations: AH [C,H,OH() --277.7 kJ/mol; AH(CH3CO,H() = -484.5 kJ/mol); AH® [H2O(1) --285.8 kJ/mol]; AH [O2(g) - 0 kJ/mol). Calculate the AHan for the reaction. C,H,OH(I)+,(g) → CH,CO,H(1) + H2O(l)
Using the bond enthalpies in the Average Bond Enthalpies table, determine the approximate enthalpy (in kJ) for each of the following reactions. (Assume the average bond enthalpy of the Cl–F bond is 254 kJ/mol.) (a) Cl2(g) + 3 F2(g) → 2 ClF3(g) (b) H2C=CH2(g) + H2(g) → H3CCH3(g) (c) 2 CH3(C=O)H(g) + 5 O2(g) → 4 CO2(g) + 4 H2O(g) ITITIT Average Bond Enthalpies AH bond (kJ/mol) bond AHond (kJ/mol) bond AH bond (kJ/mol) bond bond AH bond (kJ/mol) С-Н...
4. Given the following standard enthalpy of formations: AH° C,H,OH() =-277.7 kJ/mol]; AHO [CH CO H) = 484.5 kJ/mol]; AH° [HO) = -285.8 kJ/mol]; AH° (O,(g) 0 kJ/mol] UnvIL Calculate the LDH for the reaction. CH.OHI)+0,(g)- CH,CO,H() H,O()
Use the molar bond enthalpy data in the table to estimate the value of AHin for the equation Bond 0-H 0-0 kJ. mol 464 142 351 kJ. mol 890 390 159 CH,() + 4C1,(8) CCI (8) + 4 HCI(g) C-0 The bonding in the molecules is shown. O=0 502 418 C=0 945 730 347 H- Bond CEN N-H N-N N=N N=N F-F CI-CI Br-Br H-H H-F H-CI - Cl C-CI + C CI CCI C-CI 155 HC + H Cl...
Given 2Al(s) + (3/2)O2(g) → Al2O3(s), AH°f = –1,670 kJ/mol for Al2O3 (s). Determine AH° for the reaction 3Al2O3(s) →6Al(s) + (9/2)02(g). Write answer to three significant figures. Numeric Response
A chemist measures the enthalpy change AH during the following reaction: 8 SO2(9) 16 H2S(g) AH=-1863. kJ 3 Sg(s) + 16 H,20) Use this information to complete the table below. Round each of your answers to the nearest kJ/mol. AH Oto reaction E726. kJ 16S0, (8) +32H,S () -- 6s,) +32H20 () 1863. kJ 3s,() +16H,O()8So, (e)16H,s() 5589. kJ 9s,()48H,0()24SO, (s) +48H,S (g)