When a solid dissolves in water, the solution may become hotter or colder. The dissolution enthalpy (dissolving) can be determined using a coffee cup calorimeter.In the laboratory, a general chemistry student finds that when 9.76 g K₂SO₄(s) is dissolved in 110.80 g water, the temperature of the solution drops from 24.45 to 21.22 °C.The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.60 J/°C.Based on the student's observation, calculate the dissolution enthalpy of K₂SO₄(s) in kJ/mol.Assume the specific heat capacity of the solution is equal to the specific heat capacity of water.Δ_disH = _____ kJ/mol When a solid dissolves in water, the solution may become hotter or colder. The **dissolution enthalpy** (dissolving) can be determined using a coffee cup calorimeter.In the laboratory, a general chemistry student finds that when **8.78 g CsCl(s)** is dissolved in **111.10 g** water, the temperature of the solution **drops from 25.41 to 23.19 °C**.The heat capacity of the calorimeter (sometimes referred to as the **calorimeter constant**) was determined in a separate experiment to be **1.57 J/°C**.Based on the student's observation, calculate the dissolution enthalpy of **CsCl(s)** in kJ/mol.Assume the specific heat capacity of the solution is equal to the specific heat capacity of water.\[ \Delta_{\text{dis}}H = \_\_\_\_ \text{ kJ/mol} \]

Since your question has multiple parts, we will answer the first question for you. If you want residual parts to be answered, then please resubmit the entire question and mention those parts you want us to answer. The total heat change of a system remains constant. The heat released or gained in the reaction is taken or given by the solution.qreaction=-(qsolution+qcalorimeter)qsolution=mc∆There, qreaction=-(110.80g×4.184JgC×21.22-24.25)+1.60JC×21.22-24.25=--1497.39J-5.17J=+1502.56Jmoles of salt=9.76g174.26g/mole0.056 moles∆Hrxn=qreactionmole=+1502.56J0.056 moles=+26831.43J/mole+26.83 KJ/mole

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When a solid dissolves in water, the solution may become hotter or colder. The dissolution enthalpy (dissolving) can be determined using a coffee cup calorimeter. In the laboratory a general chemistry student finds that when 9.76 g K2SO4(s) is dissolved in 110.8 the temperature of the solution drops from 24.45 to 21.22 °C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was detern separate experiment to be 1.60 J/ºC. Based on the student's observation, calculate the dissolution enthalpy of K2SO4(s) in k.J/mol. Assume the specific heat capacity of the solution is equal to the specific heat capacity of water. AdisH : kJ/mol

When a solid dissolves in water, the solution may become hotter or colder. The dissolution enthalpy (dissolving) can be determined using a coffee cup calorimeter. In the laboratory a general chemistry student finds that when 9.76 g K2SO4(s) is dissolved in 110.8 the temperature of the solution drops from 24.45 to 21.22 °C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was detern separate experiment to be 1.60 J/ºC. Based on the student's observation, calculate the dissolution enthalpy of K2SO4(s) in k.J/mol. Assume the specific heat capacity of the solution is equal to the specific heat capacity of water. AdisH : 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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