When 125 mL of 0.210 M NaCl(aq) and 125 mL of 0.210 M AgNO3(aq), both at 21.0°C, are mixed in a coffee cup calorimeter, the temperature of the mixture increases to 23.6°C as solid AgCl forms. NaCl(aq) + AgNO3(aq) → AgCl(s) + NaNO3(aq) This precipitation reaction produces 2.71 x 10³ J of heat, assuming no heat is absorbed by the calorimeter, no heat is exchanged between the calorimeter and its surroundings, and that the specific heat and density of the solutions are the same as those for water (4.18 J/g °C, and 0.997 g/mL, respectively). Using this data, calculate AH in kJ/mol of AgNO3(aq) for the given reaction. 4.0✔ kJ/mol

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**Transcription for Educational Website**

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When 125 mL of 0.210 M NaCl(aq) and 125 mL of 0.210 M AgNO₃(aq), both at 21.0°C, are mixed in a coffee cup calorimeter, the temperature of the mixture increases to 23.6°C as solid AgCl forms.

\[ \text{NaCl(aq) + AgNO}_3\text{(aq) → AgCl(s) + NaNO}_3\text{(aq)} \]

This precipitation reaction produces \( 2.71 \times 10^3 \) J of heat, assuming no heat is absorbed by the calorimeter, no heat is exchanged between the calorimeter and its surroundings, and that the specific heat and density of the solutions are the same as those for water (4.18 J/g°C, and 0.997 g/mL, respectively). Using this data, calculate \( \Delta H \) in kJ/mol of AgNO₃(aq) for the given reaction.

[Input box appears here]
\( \Delta H \) = _______ kJ/mol

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Note that the experiment uses a coffee cup calorimeter to measure the heat change during the reaction, and all assumptions are made to simplify calculations, assuming ideal conditions.
Transcribed Image Text:**Transcription for Educational Website** --- When 125 mL of 0.210 M NaCl(aq) and 125 mL of 0.210 M AgNO₃(aq), both at 21.0°C, are mixed in a coffee cup calorimeter, the temperature of the mixture increases to 23.6°C as solid AgCl forms. \[ \text{NaCl(aq) + AgNO}_3\text{(aq) → AgCl(s) + NaNO}_3\text{(aq)} \] This precipitation reaction produces \( 2.71 \times 10^3 \) J of heat, assuming no heat is absorbed by the calorimeter, no heat is exchanged between the calorimeter and its surroundings, and that the specific heat and density of the solutions are the same as those for water (4.18 J/g°C, and 0.997 g/mL, respectively). Using this data, calculate \( \Delta H \) in kJ/mol of AgNO₃(aq) for the given reaction. [Input box appears here] \( \Delta H \) = _______ kJ/mol --- Note that the experiment uses a coffee cup calorimeter to measure the heat change during the reaction, and all assumptions are made to simplify calculations, assuming ideal conditions.
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