### Heat of Dissolution Experiment Using a Coffee Cup CalorimeterWhen a solid dissolves in water, heat may either be evolved or absorbed. This change in heat, known as the heat of dissolution (dissolving), can be determined using a coffee cup calorimeter.#### Student Experiment Overview:A general chemistry student conducted an experiment to determine the heat of dissolution for copper(II) chloride (CuCl₂). The following observations were noted during the experiment:- **Mass of CuCl₂:** 4.14 g- **Mass of water:** 106.80 g- **Initial temperature of water:** 23.05°C- **Final temperature of solution:** 26.46°CThe experiment also determined that the heat capacity of the calorimeter (often referred to as the calorimeter constant) is 1.65 J/°C in a separate calibration experiment.#### Calculation of Enthalpy of Dissolution (ΔH_dissolution):The enthalpy of dissolution of CuCl₂(s) in kJ/mol can be calculated from the observed temperature change, the mass of the solvent, and the known specific heat capacity of water. This allows us to find the heat absorbed or released during the dissolution process.##### Provided Formula:\[ \Delta H_{\text{dissolution}} = \text{__} \text{kJ/mol} \]#### Diagram Analysis:The accompanying diagram represents a coffee cup calorimeter used in the experiment. The components include:- A **thermometer** inserted through a **cardboard or Styrofoam lid** to monitor the temperature change.- **Nested Styrofoam cups** form the calorimeter, providing insulation to ensure minimal heat loss.- The **reaction occurs inside the solution** contained within these cups.This setup allows for a relatively simple and effective way to measure the heat involved in the dissolving process of solids in liquids, typical in a laboratory setting. The temperature changes recorded by the thermometer can be used to calculate the heat change associated with the dissolution reaction. **Understanding the Heat of Dissolution Using a Coffee Cup Calorimeter****Context:**When a solid dissolves in water, heat may either be evolved (released) or absorbed. This phenomenon, known as the heat of dissolution, can be determined using an apparatus called a coffee cup calorimeter.**Laboratory Experiment:**In an experiment conducted by a general chemistry student, 21.37 grams of BaBr₂(s) were dissolved in 103.30 grams of water. As a result, the temperature of the solution increased from 24.05°C to 27.39°C.The heat capacity of the calorimeter (often referred to as the calorimeter constant) was determined in a separate experiment and found to be 1.77 J/°C.**Objective:**Based on the student's observations, calculate the enthalpy of dissolution (ΔH_dissolution) of BaBr₂(s) in kJ/mol.**Assumptions:**- The specific heat of the solution is equal to the specific heat of water.**Calculation:**ΔH_dissolution = ____ kJ/mol**Apparatus Diagram:**The accompanying diagram illustrates a typical coffee cup calorimeter setup used for the experiment:- **Thermometer:** Used to measure the temperature change of the solution.- **Cardboard or Styrofoam lid:** Acts as an insulator to minimize heat exchange with the surroundings.- **Nested Styrofoam cups:** These cups provide additional insulation to help maintain a constant reaction temperature.- **Inner Cup (Solution):** This is where the reaction occurs. It contains water and the dissolved substance.By analyzing the temperature change and knowing the specific heat capacity, the enthalpy change for the dissolution process can be calculated.**Educational Note:**Such experiments are fundamental in thermochemistry for understanding energy changes associated with chemical reactions. By measuring how much heat is absorbed or released, chemists can infer important properties about the substances undergoing reaction.For a detailed step-by-step calculation and further theoretical background, students can refer to the thermochemistry section on our website.

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When a solid dissolves in water, heat may be evolved or absorbed. The heat of dissolution (dissolving) can be determined using a coffee cup calorimeter. Thermometer Cardboard or Styrofoam lid In the laboratory a general chemistry student finds that when 4.14 g of CuCl,(s) are dissolved in 106.80 g of water, the temperature of the solution increases from 23.05 to 26.46 °C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.65 J/°C. Nested Styrofoam cups Based on the student's observation, calculate the enthalpy of dissolution of CuCl2(s) in kJ/mol. Reaction Assume the specific heat of the solution is equal to the specific heat of water. occurs in solution. AHdissolution= kJ/mol

When a solid dissolves in water, heat may be evolved or absorbed. The heat of dissolution (dissolving) can be determined using a coffee cup calorimeter. Thermometer Cardboard or Styrofoam lid In the laboratory a general chemistry student finds that when 4.14 g of CuCl,(s) are dissolved in 106.80 g of water, the temperature of the solution increases from 23.05 to 26.46 °C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.65 J/°C. Nested Styrofoam cups Based on the student's observation, calculate the enthalpy of dissolution of CuCl2(s) in kJ/mol. Reaction Assume the specific heat of the solution is equal to the specific heat of water. occurs in solution. AHdissolution= kJ/mol

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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