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Enthalpy change of reaction
Product - reactant
Endothermic
∆H = +
Endothermic
∆H = +
Exothermic
∆H = -
Enthalpy change of formation
Element to 1 mol of compound
∆H = ∆H of product - ∆H of reactant
Enthalpy change of combustion
1 mol of substance + nO2 = oxides + water
∆H = ∆H of reactant - ∆H of product
Enthalpy change of neutralisation
Acid + alkali = 1 mol of water + salt
bond enthalpy change
Bond enthalpy of reactant - Bond enthalpy of product
Enthalpy change of calorimetry
Calorimetry: q = m ∆ T
Enthalpy = q / number of mole reacting
Homogenous catalyst
Catalyst is in the same state of as the reactant
Heterogenous catalyst
Catalyst is in a different state from the reactant
Note
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