Reactivity 1.2
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What sort of process is bond breaking?
Endothermic
What sort of process is bond forming?
Exothermic
In terms of bond breaking and forming, describe when a reaction would be exothermic.
The energy released from forming new bonds is greater than the energy needed to break existing bonds
In terms of bond breaking and forming, describe when a reaction would be endothermic.
The energy needed to break existing bonds is greater than the energy released from forming new bonds
To use average bond enthalpies to determine an enthalpy change of reaction, which state must all reactants and products be
Gas
Describe how to calculate the enthalpy of reaction using bond enthalpy values
The sum of the energies needed to break bonds in the reactants minus the energy released when the new bond are formed in the products
Define bond enthalpy
The enthalpy change needed to break one mole of bonds in a gaseous molecule averaged over similar compounds
Explain why experimentally determined enthalpy of reaction values are always different from theoretical enthalpy of reaction values calculated using bond enthalpy data
Bond enthalpy values in the data booklet are averages of that bond in many different molecules, whilst the experimental data will be determined using a specific molecules.
Explain why the bond enthalpy values in the data booklet are averages
They are an average value of the bond enthalpy for the same bond in different environments or molecules
Determine the enthalpy required to break all the bonds in 1.00 mol of nitrogen molecules
(+) 945 kJ mol⁻
Determine the enthalpy released when forming all the bonds in 1.00 mol of nitrogen molecules
(-) 945 kJ mol⁻
Determine the enthalpy required to break all the bonds in 1.00 mol of oxygen molecules
(+) 498 kJ mol⁻
Determine the enthalpy released when forming all the bonds in 1.00 mol of oxygen molecules
(-) 498 kJ mol⁻
Determine the enthalpy required to break all the bonds in 1.00 mol of carbon dioxide molecules
(+) 1608 kJ mol⁻
Determine the enthalpy released when forming all the bonds in 1.00 mol of carbon dioxide molecules
(-) 1608 kJ mol⁻
Determine the enthalpy required to break all the bonds in 1.00 mol of methane molecules
(+) 1656 kJ mol⁻
Determine the enthalpy released when forming all the bonds in 1.00 mol of methane molecules
(-) 1656 kJ mol⁻
Determine the enthalpy required to break all the bonds in 1.00 mol of propene molecules
(+) 3444 kJ mol⁻
Determine the enthalpy released when forming all the bonds in 1.00 mol of propene molecules
(-) 3444 kJ mol⁻
Using section 12 of the data booklet, determine the total enthalpy required to break all the bonds in the following reactants
(+) 1898 kJ mol⁻
Using section 12 of the data booklet, determine the total enthalpy required to break all the bonds in the following reactants
(+) 2582 kJ mol⁻
Using section 12 of the data booklet, determine the total enthalpy required to break all the bonds in the following reactants
(+) 6494 kJ mol⁻
Using section 12 of the data booklet, determine the total enthalpy released to form all of the bonds in the following products
(-) 1997 kJ mol⁻
Using section 12 of the data booklet, determine the total enthalpy released to form all of the bonds in the following products
(-) 2385 kJ mol⁻