Calculate the average molar bond enthalpy of the carbon-hydrogen bond in a CH4 molecule.
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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
Calculate the average molar bond enthalpy of the carbon-hydrogen bond in a CH4 molecule. -- Given...
Given that ΔΗ;[H(g)].. 218.0 kJ-mol-1 ari[ck)]-716.7 kJ.mol ' ΔΗ,[CH,(g)]=-74.6 kJ-mol-1 calculate the average molar bond enthalpy of the carbon-hydrogen bond in a CH4 molecule. Number k.J mol
calculate the average molar bond enthalpy of the carbon-chlorine bond in a CCl4 molecule. Given that calculate the average molar bond enthalpy of the carbon-chlorine bond in a CCl4 molecule. Given that delta Hf[Cl(g)]= 121.3 KJ.mol^-1 delta Hf[C(g)]= 716.7 KJ.mol^-1 delta Hf[CCl4(g)]= -95.7 KJ.mol^-1
calculate the average molar bond enthalpy of the carbon-bromine bond in a CBr4 molecule. given thay : deltaH= Br(g)= 111.9 kj dH= C(g)= 716.7 jk dH= CBr4(g)= 29.4
Given that ΔΙ, [Br(g)]-111.9 kJ-mol-1 dH,[dg)]-716.7 kJ-mol-1 ΔΗǐ[CBr,(e)]-29.4 kJ-mol-1 calculate the average molar bond enthalpy of the carbon-bromine bond in a CBr4 molecule. Number : mol
The average C - H bond energy in CH4 is 415 kJ / mol. Use the following data to calculate the average C - H bond energy in ethane ( C2H6;C - C bond ) , in ethane ( C2H4;C C bond ) , and in ethyne ( C2H2;C C bond ) . C2H6 ( g ) + H2 ( g ) rightarrow 2CH4 ( g ) delta H*rxn = - 65.07 kj / mol C2H4 ( g ) +...
explain why the molar enthalpy of formation for Carbon Graphite, is 0 kj/mol, while the molar standard enthalpy of formation for carbon diamond, is +1.90 kj/mol and that of carbon gas is +716.7 kj/mol.
the bond enthalpy of cl2 is 242.7 kj/mol . calculate delta Hf for Cl (g). 3. The bond enthalpy of Cl2(g) is 242.7 kJ/mol. Calculate AHⓇ for Cl (g).
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
Use the molar bond enthalpy data in the table to estimate the value of Delta Hdegreerxn for the equation CH4(g)+4Cl2(g) right arrow ccl4(g)+4HCl(g) The bonding in the molecules is shown here. Average molar bond enthalpies. (Hbond) Delta H degree rxn= Number kJ.mol^-1
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