The reaction is
H2 + F2 2 HF
(1)
Bond | Bond enthalpy, KJ/mol |
H-H | 436 |
F-F | 157 |
H-F | unknown |
Substance | Heat of formation (KJ/mole) |
H2 | 0 |
F2 | 0 |
H-F | -271 |
From reaction 1.
Heat of formation of 2× HF =
Bond enthalpy of
reactants -
Bond enthalpy of
products
Or, -271× 2 = (436+157) - 2× Bond enthalpy of HF
Or, 2× Bond enthalpy of HF = - 271×2 - (436 +157)
or, 2× Bond enthalpy of HF = - 1135.3 KJ
Or, Bond enthalpy of HF = (1135 /2) = 567.5 KJ/mole.
TOGO Estimate the H-F bond enthalpy knowing that the Heat of Formation of hydrogen fluoride (AH;,...
Knowing the enthalpy of formation of calcium fluoride is -1228 KJ / mol, the enthalpy of the sublimation of calcium is 168kj/mole, the bond enthalpy of fluorine is 155kj/mole, the electron affinity of fluorine is -328 kj/mole, the first ionization enthalpy of calcium is 590kj/mole and the second ionization enthaply is 1145kj/mole, calculate the lattice enthalpy of calcium fluoride.
Estimate the enthalpy of formation of HF from the following bond energies: (twenty-five points) H2 (g) + F2 (g) → 2 HF (g) Bond: H-H =432KJ/mol F-F=159 KJ/mol H-F= -565 KJ/mol
Calculate the standard enthalpy of formation of gaseous
hydrogen fluoride (HF) using the following thermochemical
information:
C2H4(g) + 6 F2(g) 2 CF4(g) + 4 HF(g) H = -2486.3 kJ
CF4(g) C(s) + 2 F2(g) H = +680 kJ
C2H4(g) 2 C(s) + 2 H2(g) H = -52.3 kJ
H = ??? kJ
Calculate the standard enthalpy of formation of gaseous hydrogen
fluoride (HF) using the following thermochemical information:
C2H4(g)
+ 6 F2(g) 2 CF4(g) + 4 HF(g)
H = -2486.3 kJ
CF4(g) C(s) + 2 F2(g)
H = +680 kJ
C2H4(g)
2 C(s) + 2 H2(g)
H = -52.3 kJ
H = ___?kJ
The answer is not -589.3
Calculate the standard enthalpy of formation of gaseous hydrogen fluoride (HF) using the following thermochemical information: C2H4(g) + 6 F2(g) 2 CF4(g) + 4 HF(g) (delta)H = -2486.3 kJ CF4(g) C(s) + 2 F2(g) (delta)H = +680 kJ 2 C(s) + 2 H2(g) C2H4(g) (delta)H = +52.3 kJ (delta)H =__________ kJ
Using the standard enthalpy of formation data, show how the standard enthalpy of formation of HF(g) can be used to determine the bond energy. (Enter unrounded values.) (a) bond energy calculated from standard enthalpy of formation kJ/mol (b) average bond enthalpy from the bond enthalpy table k]/mol Average Bond Enthalpies bondAH bond (kJ/mol) bond AHbond (kJ/mol) bond AH bond (kJ/mol) bond AH bond (kJ/mol) O-H 0-0 467 146 495 185 203 156 364 522 335 544 413 347 614 839...
Use bond energies to estimate the enthalpy of formation of HBr(g). BE(H–H) = 436 kJ/mol BE(Br–Br) = 192 kJ/mol BE(H–Br) = 366 kJ/mol A –52 kJ/mol B +262 kJ/mol C +104 kJ/mol D +52 kJ/mol E –104 kJ/mol
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
Calculate the average molar bond enthalpy of the carbon-hydrogen bond in a CH4 molecule. -- Given that (Delta)Hf [H(g)]= 218.0 kj/mol (Delta)Hf [C(g)]= 716.7 kJ/mol (Delta)Hf [CH4(g)]= -74.6 kJ/mol
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 Determine the enthalpy of the gas phase reaction (AH).