Heat of Reaction
The Heat of Reaction is the change in the enthalpy of a chemical reaction that occurs at a constant pressure. It is a thermodynamic unit of measurement useful for calculating the amount of energy per mole either released or produced in a reaction. Since enthalpy is derived from pressure, volume, and internal energy, all of which are state functions, enthalpy is also a state function.
ΔH, or the change in enthalpy arose as a unit of measurement meant to calculate the change in energy of a system when it became too difficult to find the ΔU, or change in the internal energy of a system, by simultaneously measure the amount of heat and work exchanged. Given a constant pressure, the change in enthalpy can be measured as ΔH=q (See enthalpy for a more detailed explanation)
The notation ΔHº or ΔHºrxn then arises to explain the precise temperature and pressure of the heat of reaction ΔH. The standard enthalpy of reaction is symbolized by ΔHº or ΔHºrxn and can take on both positive and negative values. The units for ΔHº are kilojoules per mole, or kj/mol.
ΔH and ΔHºrxn
The Standard State: The standard state of a solid or liquid is the pure substance at a pressure of 1 bar ( 105 Pa) and at a relevant temperature.
The ΔHºrxn is the standard heat of reaction or standard enthalpy of a reaction, and like ΔH also measures the enthalpy of a reaction. However, ΔHºrxn takes place under "standard" conditions, meaning that the reaction takes place at 25º C and 1 atm. The benefit of a measuring ΔH under standard conditions lies in the ability to relate one value of ΔHº to another, since they occur under the same conditions.
How to Calculate ΔH Experimentally
Enthalpy can be measured experimentally through the use of a calorimeter. A calorimeter is an isolated system which has a constant pressure, so ΔH=q=cpsp x m x (ΔT)
How to calculate ΔH Numerically
In order to calculate the standard enthalpy of reaction the standard enthalpy of formation must be utilized. Another, more detailed, form of the standard enthalpy of reaction includes the use of the standard enthalpy of formation ΔHºf:
ΔHº = ∑ΔvpΔHºf(products) - ∑Δ vrΔHºf(reactants)
Since enthalpy is a state function, the heat of reaction depends only on the final and initial states, not on the path that the reaction takes. For example, the reaction A-->B goes through intermediate steps (ie C-->D), but A and B remain intact.
Therefore, one can measure the enthalpy of reaction as the sum of the ΔH of the three reactions by applying Hess' Law.
Since the ΔHº represents the total energy exchange in the reaction this value can be either positive or negative.
1. ΔH=q=cpsp x m x (ΔT) = (.98) x (2) x (+6o ) = 11.76 kJ
2. Since the heat gained by the calorimeter is equal to the heat lost by the system, then the substance inside must have lost the negative of +2001 J, which is -2001 J.
3. ΔHº = ∑ΔvpΔHºf(products) - ∑Δ vrΔHºf(reactants) so this means that you add up the sum of the ΔH's of the products and subtract away the ΔH of the products: (-275.2kJ) - (-393.509kJ + -241.83kJ) = (-275.2) - (-635.339) = +360.139 kJ.
4. ΔH=q=cpsp x m x (ΔT) = (.9) x (1.6) x (13) = 18.72 kJ
5. Endothermic, since a positive value indicates that the system GAINED heat.
This page viewed 82969 times