`=>` For chemical reactions, heat absorbed at constant volume, is measured in a `color{red}("bomb calorimeter")` (Fig. 6.7).

● Here, a steel vessel (the bomb) is immersed in a water bath. The whole device is called calorimeter.

● The steel vessel is immersed in water bath to ensure that no heat is lost to the surroundings.

● A combustible substance is burnt in pure dioxygen supplied in the steel bomb. Heat evolved during the reaction is transferred to the water around the bomb and its temperature is monitored.

● Since the bomb calorimeter is sealed, its volume does not change i.e., the energy changes associated with reactions are measured at constant volume.

● Under these conditions, no work is done as the reaction is carried out at constant volume in the bomb calorimeter. Even for reactions involving gases, there is no work done as `color{purple}(ΔV = 0)`.

● Temperature change of the calorimeter produced by the completed reaction is then converted to `q_V`, by using the known heat capacity of the calorimeter with the help of equation 6.11(`color{purple}(q = c ×m × DeltaT =C DeltaT)`).

`=>` Measurement of heat change at constant pressure (generally under atmospheric pressure) can be done in a calorimeter shown in Fig.6.8.

`=>` We know that `color{pu(rple}ΔH = q_p)` (at constant p) and, therefore, heat absorbed or evolved, `q_p` at constant pressure is also called the heat of reaction or enthalpy of reaction, `color{purple}(Δ_r H)`.

● In an exothermic reaction, heat is evolved, and system loses heat to the surroundings. Therefore, `color{purple}(q_p)` will be negative and `color{purple}(Δ_r H)` will also be negative.

● Similarly in an endothermic reaction, heat is absorbed, `color{purple}(q_p)` is positive and `color{purple}(Δ_r H)` will be positive.