3. When 21.45 g of potassium nitrate was dissolved in water in a calorimeter, the temperature fell from 25.00°C to 14.14°C. If the heat capacity of the calorimeter and its contents is 682 J/°C, what is AH for the dissolution of potassium nitrate, in kJ/mol? rxn Write the equation for this reaction: Is it exothermic or endothermic? Draw the enthalpy diagram for the dissolution of KNO3

3. When 21.45 g of potassium nitrate was dissolved in water in a calorimeter, the temperature fell from 25.00°C to 14.14°C. If the heat capacity of the calorimeter and its contents is 682 J/°C, what is AH for the dissolution of potassium nitrate, in kJ/mol? rxn Write the equation for this reaction: Is it exothermic or endothermic? Draw the enthalpy diagram for the dissolution of KNO3

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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Section 5.6 You place 0.0750 g of magnesium chips in a coffee-cup calorimeter and then add 100.0 mL of 1.00 M HCI. The reaction that occurs is: -> Mg (s) + 2 HCI (aq) → H2 (g) + MgCl2 (aq) The temperature of the solution raises from 20.15 °C to 23.29 °C. What is the enthalpy change or the reaction per mole of Mg? Assume that the specific heat capacity of the solution is 4.20 J/g K and the density of the solution is 1.00 g/mL. 412 kJ/mol 428 kJ/mol -412 kJ/mol -428 kJ/mol
The answer in the box is wrong.
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You have 8.99 g sample of an unknown salt (MM = 116.82 g/mol). It is dissolved in 150.00 g water in a coffee cup calorimeter. Before placing the sample in the water, the temperature of the salt and water is 23.72°C. After the salt has completely dissolved, the temperature of the solution is 28.54°C. What is the Mass inside calorimeter (g)? Change in Temp inside calorimeter (C)? How much Heat gained (J)? Total Heat? How many mols of the unknown salt? What is the change in empalthy?
A 6.55 g sample of an unknown salt (MM = 116.82 g/mol) is dissolved in 150.00 g water in a coffee cup calorimeter. Before placing the sample in the water, the temperature of the salt and water is 23.72°C. After the salt has completely dissolved, the temperature of the solution is 28.54°C. Wht is the change in teperature in celcios inside the calometer? was the dissolution process endothermic or exothermic? how much heat, in J, was hained b the solution? assume the specific heat of the solution is the same as water, 4.184 J/g. celcius
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. In the laboratory a general chemistry student finds that when 3.95 g of CuCl2(s) are dissolved in 108.60 g of water, the temperature of the solution increases from 23.05 to 26.27 °C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.86 J/°C. Based on the student's observation, calculate the enthalpy of dissolution of CuCl,(s) in kJ/mol. Assume the specific heat of the solution is equal to the specific heat of water. AHdissolution kJ/mol