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Chemistry

Energetics

QuestionAnswer
Define endothermic process Energy is absorbed into the system which results in bond breaking
Define exothermic process Energy is released from the system which results in bond making
Why is enthalpy +ve in endothermic reactions The heat change in product is greater than heat change in reactant Hp>Hr
Why is enthalpy -ve in exothermic reactions The heat change in reactant is greater than heat change in product Hr>Hp
Does temp of surroundings increase/decrease in endothermic reactions Decrease due to heat being absorbed
Does temp of surroundings increase/decrease in exothermic reactions Increase due to heat being released
Why is Ea higher in endothermic reactions Great amount of energy needs to be absorbed to allow for bond breaking hence there are fewer endothermic reactions
Definition of bond energy and its unit The amount of energy needed to break 1 mole of a particular bond in 1 mole of a gaseous molecule KJ/mol
What effect does the type of bond have on bond energy As the bonds between atoms increase, bond energy increases single bond<double bond<triple bond
What effect does the bond length have on bond energy If bond length increase, bond energy decreases
T/F. Bond length increases because atomic radius increases T
Formula for enthalpy change delta h = sum of reactants - sum of formed
How does ionic charge affect magnitude of lattice energy The higher the ionic charge of the ions the more attraction between the ions in the compound therefore latt energy is greater
State Hess' Law The total enthalpy change of a reaction is independent of the route the reaction proceeds.
Created by: Dia_white
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