If a student performs an endothermic reaction in a...

If a student performs an endothermic reaction in a calorimeter, how does the calculated value of $\Delta H$ differ from the actual value if the heat exchanged with the calorimeter is not taken into account?

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Key Concepts

Endothermic Reactions

Endothermic reactions absorb heat from their surroundings, resulting in a positive ?H value. When performing such reactions in a calorimeter, it is crucial to include all sources of heat absorption, including the calorimeter’s heat capacity, to accurately determine the true enthalpy change.

Heat Exchange and Energy Conservation

The principle of energy conservation in thermodynamics asserts that energy cannot be created or destroyed, only transferred or transformed. In calorimetric experiments, this means that both the reaction and the calorimeter absorb or release heat. Neglecting the heat absorbed by the calorimeter results in an incomplete energy balance, leading to errors in the calculated ?H.

Calorimetry

Calorimetry is the technique used to measure the amount of heat involved in chemical reactions or physical changes. It relies on a calorimeter to capture the heat released or absorbed, ensuring that all aspects of energy transfer within the system are accounted for.

Enthalpy Change (?H)

Enthalpy change, symbolized as ?H, represents the heat change at constant pressure during a reaction. Accurate determination of ?H is essential for understanding the energy profile of a reaction, particularly when distinguishing between endothermic and exothermic processes.

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