When 1.045 g of CaO is added to 50.0 mL of water at 25.0^∘ C in a calorimeter, the temperature o

step 1 We know the density of water is 1. So 50 ml of water will be equivalent to 50 grams of water. No

When 1.045 g of CaO is added to 50.0 mL of water at 25.0^∘ C...

When 1.045 g of CaO is added to 50.0 $\mathrm{mL}$ of water at $25.0^{\circ} \mathrm{C}$ in a calorimeter, the temperature of the water increases to $32.3^{\circ} \mathrm{C}$ . Assuming that the specific heat of the solution is 4.18 J/(g. $^{\circ} \mathrm{C} )$ and that the calorimeter itself absorbs a negligible amount of heat, calculate $\Delta H$ in kilojoules for the reaction

When 1.045 g of CaO is added to 50.0 $\mathrm{mL}$ of water at $25.0^{\circ} \mathrm{C}$ in a calorimeter, the temperature of the water increases to $32.3^{\circ} \mathrm{C}$ . Assuming that the specific heat of the solution is 4.18 J/(g. $^{\circ} \mathrm{C} )$ and that the calorimeter itself absorbs a
negligible amount of heat, calculate $\Delta H$ in kilojoules for the reaction

Key Concepts

Calorimetry

Calorimetry is the experimental technique used to measure the amount of heat transferred to or from a substance during a physical or chemical process. This method typically involves using a calorimeter, an insulated device that minimizes heat exchange with the surroundings, ensuring that the measured temperature changes accurately reflect the heat released or absorbed by the reaction.

Specific Heat Capacity

Specific heat capacity is a physical property that indicates the amount of heat required to raise the temperature of a unit mass of a substance by one degree Celsius. It is a crucial parameter in calorimetric calculations because it allows for the determination of the energy change associated with a given temperature change when the mass of the substance is known.

Heat Transfer Equation

The heat transfer equation, q = m × c × ?T, relates the amount of heat (q) absorbed or released by a substance to its mass (m), its specific heat capacity (c), and the change in temperature (?T). This fundamental equation is at the heart of calorimetric calculations, enabling the conversion of temperature changes into quantifiable energy changes.

Enthalpy Change (?H)

Enthalpy change (?H) is a thermodynamic quantity that represents the heat absorbed or released during a chemical reaction at constant pressure. It provides insight into whether a reaction is exothermic (releases heat) or endothermic (absorbs heat) and is essential for understanding the energy profile of reactions.

Stoichiometry

Stoichiometry involves the quantitative relationship between reactants and products in a chemical reaction. In the context of calorimetry, it is used to convert the measured energy change, derived from calorimetric data, into a per mole basis, which is essential for comparing the reaction’s heat change to standard thermodynamic values.

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