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青州's Question
Posted 3 months ago

The addition of 115.0 g115.0 \mathrm{~g} potassium fluoride to 609.0 mL609.0 \mathrm{~mL} of water (d=1.00 g/mL)(\mathrm{d}=1.00 \mathrm{~g} / \mathrm{mL}) causes the temperature to rise 3.81\degC3.81 \backslash \operatorname{deg} \mathrm{C}. What is the \\backslash Delta Hrxn for KF? (Assume cs=4.18 J/g\mathrm{cs}=4.18 \mathrm{~J} / \mathrm{g} oC.)
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Answer from Sia
Posted 3 months ago
Calculate the heat absorbed by the water: To find the enthalpy change of the reaction, we first need to calculate the heat absorbed by the water using the formula q=mCsΔTq = m \cdot Cs \cdot \Delta T
Convert heat to kilojoules: The heat absorbed by the water needs to be converted from joules to kilojoules since the enthalpy change is asked in kJ
Calculate the enthalpy change for KF: The enthalpy change for the reaction involving KF is the negative of the heat absorbed by the water per mole of KF
The ΔHrxn\Delta H_{rxn} for KF is -57.2 kJ/mol
Key Concept
Enthalpy change of a reaction
The enthalpy change of a reaction is the heat absorbed or released during the reaction, which can be calculated from the temperature change of the solution and the amount of substance involved.

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