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41 Terms

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Calorimetry

The measurement and calculation of energy transferred as heat during a chemical reaction.

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Constant-Pressure Calorimetry

Also known as Coffee-Cup Calorimetry, ideal for reactions in aqueous solutions.

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qreaction

The heat exchanged by the reaction, calculated as -qsolution.

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qsolution

The heat absorbed or released by the solution, calculated using the formula qsolution=mcΔT.

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m (mass)

The mass of the solution, usually equal to the mass of water in grams.

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c (specific heat capacity)

The specific heat capacity for water is 4.18 J/g·°C.

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ΔT (temperature change)

The change in temperature, calculated as Tfinal - Tinitial.

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Heat exchange assumption

No heat is lost to the calorimeter or surroundings, implying an ideal situation.

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Limitations of Calorimetry

Imperfect insulation resulting in low precision; typically used for educational purposes.

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Constant-Volume Calorimetry

Also known as Bomb Calorimetry, where samples are combusted in a sealed bomb.

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ΔU

The change in internal energy measured in a constant-volume calorimeter.

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Energy measurement in Bomb Calorimetry

Measures the change in internal energy, not enthalpy.

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Uses of Bomb Calorimetry

Measuring caloric values of food and evaluating fuel efficiency.

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Accurate measurements

Bomb calorimeters provide more accurate measurements than coffee-cup calorimeters.

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Calorimeter’s heat capacity

Requires knowledge of this to make calculations in Bomb Calorimetry.

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Heat flow equation (Coffee-Cup)

qreaction = - (mcΔT) for constant-pressure calorimetry.

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Heat flow equation (Bomb)

qreaction = - (qwater + qbomb) for constant-volume calorimetry.

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Negative signs in calorimetry

Used to indicate the direction of heat flow.

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Specific heat of water

4.18 J/g·°C, essential for calorimetry calculations.

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Unit conversion

Ensure correct conversions between grams to kilograms and joules to kilojoules.

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Heat exchange equation

qreaction + qsolution = 0 in constant-pressure calorimetry.

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Ideal calorimetry

Assumes no heat exchange with surroundings, a rare occurrence.

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Reactions in aqueous solutions

Best measured using constant-pressure calorimetry.

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Insights from calorimetry

Helps in understanding heat exchanges during chemical reactions.

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Thermometer in calorimetry

Used to measure temperature changes in calorimetric experiments.

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Insulated system in Coffee-Cup Calorimetry

Reduces heat loss to the environment, improving measurement accuracy.

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Dynamic equilibrium in calorimetry

Heat exchanges can reach equilibrium within the solutions assessed.

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Calibration of calorimeters

Important for obtaining accurate measurements and results.

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Notables of calorimetry

Calorimetry serves as a foundational concept in thermodynamics.

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Basic lab work

Calorimetry is typically used for educational demonstrations rather than precise research.

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Heat capacity of a calorimeter

Crucial for interpreting data from a bomb calorimeter.

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Enthalpy changes

Difference between internal energy and heat capacity can influence outcomes.

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Potential errors in calorimetry

Imperfect insulation can skew results, leading to inaccuracies.

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Calorimetry in real-world applications

Critical for industries including food science and environmental studies.

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Caloric value measurement

Utilized in evaluating how much energy is released during combustion.

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Liquid vs. Solid measurements

Calorimetry can be applied to both states but is more common for liquids.

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Heat absorption

Essential concept in understanding thermal processes in calorimetry.

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Chemical reaction observations

Calorimetry provides insights into the energy dynamics of reactions.

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Thermal equilibrium

Condition where the temperature remains constant during a calorimetric experiment.

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Direct calorimetry

Measures heat produced directly by a chemical process.

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Calorimetry efficiency

Impact of calorimeter design on measurement reliability.