• The thermodynamic quantity “enthalpy” is state function that depends on the initial and final states of the system.
• The enthalpy is measured when a system is at the constant pressure; the heat released or absorbed is equal to the change in enthalpy.
• The bond enthalpy is also known as the bond energy, and it is defined as the energy required for breaking the chemical bonds in a molecule.
• The average molar bond enthalpy can be calculated by dividing the bond enthalpy with total number of bonds present in a molecule.
The arbitrary reaction is given below:
The formulae to calculate the enthalpy of reaction is given below:
Consider the formation of molecule from its elements.
Given that,
The number of carbon-bromine bonds in molecule is four.
Therefore, the average bond enthalpy is given below:
Therefore, the average molar bond enthalpy is 283.725kJ.
Ans:The average molar bond enthalpy of the carbon-bromine bond in a molecule is 283.725kJ.
calculate the average molar bond enthalpy of the carbon-bromine bond in a CBr4 molecule....
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
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
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
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
A Reaction is given: ½Br2(l) --> Br(g) Ho = 112kJ/mol The bond enthalpy of Br-Br is 193 kJ/mol A. Formulate the vaporization process of 1 mol bromine Br2(l). B. Calculate the enthalpy of the vaporization process bromine. Show calculations C. Calculate the energy invested \ emitted by the evaporation of 3.2 gr of bromine. Show calculations. (Explain how you determined whether the energy is invested or emitted in this process). D.A Reaction is given: ½H2(g) + ½Br2(l) --> HBr(g) Ho...
Use the molar bond enthalpy data in the table to estimate the Average molar bond enthalpies. (Hd value of AHn for the equation kJ mol Bond Воnd kJ mol CH)+HBrig)C,H,Brig) O-H 464 CEN 890 O-O The bonding in the molecules is shown. 142 N-H 390 C-O 351 N-N 159 H Br O-O 502 N-N 418 H-Br NEN C-O 730 945 C-C 347 F-F 155 Enter numeric value С-С 615 CI-CI 243 AH = C C Br-Br I kJ 811 192...
The enthalpy for the equation OF2 ==> O + 2F is 384 kJ/mol. Calculate the average molar bond enthalpy of an oxygen -fluorine bond in an OF2 molecule
5. Calculate the heat (in kJ) required to transform 70.80 g of bromine from a solid at a temperature of -7.2 °C to a gas at 92 °C. Report your answer to one decimal place. Data: Molar mass of bromine, Br 2 = 159.808 g/mol Melting point = -7.2 °C Boiling point = 59°C. Enthalpy of fus ion = 10.57 kJ/mol Enthalpy of vaporization = 29.96 kJ/mol. Molar heat capacity of the liquid phase = 75.7 J/mol • K Molar...
Use the molar bond enthalpy data in the table to estimate the value of AHixn for the equation Average molar bond enthalpies. (Hbond) kJ · mol-1 NH2(g) + 2O2(g) — HNO2(g) + H2O(g) Bond CON 464 Bond 0-H 0-0 C-O kJ mol-1 890 390 201 N-H The bonding in the molecules is shown. N-O O=O 142 351 502 730 418 + + C=O N=N N=0 F-F 607 347 155 615 243 A Hinc C-C C=C CEC C-H AHxn = C1-C1...
Question 18 of 29 > Use the molar bond enthalpy data in the table to estimate the value of AH, for the equation CCI (8) + 2F,(g) CF (B) + 2C,®) The bonding in the molecules is shown. kJ. mol-1 890 390 159 418 945 Average molar bond enthalpies. (Hond) Bond kJ. mol-' Bond O-H 464 CEN 0-0 142 N-H N-N N=N NEN F-F CI-CI СС 811 Br-Br C-H H -H C-F H-F C-C H-CI C-B H-BE C-N 293 H-S...