Use the References to access important values if needed for this question. Thermometer 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 Cardboard or Styrofoam lid In the laboratory a general chemistry student finds that when 7.38 g of NH4Br(s) are dissolved in 114.50 g of water, the temperature of the solution drops from 24.05 to 21.15 °C The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.73 J/eC. Nested Styrofoam cups Based on the student's observation, calculate the enthalpy of dissolution of NH4Br(s) in kJ/mol Reaction occurs in Assume the specific heat of the solution is equal to the specific heat of water solution kJ/mol AHdissolution etro CangL Submit Answer Retry Entire Group 9 more group attempts remaining

Use the References to access important values if needed for this question. Thermometer 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 Cardboard or Styrofoam lid In the laboratory a general chemistry student finds that when 7.38 g of NH4Br(s) are dissolved in 114.50 g of water, the temperature of the solution drops from 24.05 to 21.15 °C The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.73 J/eC. Nested Styrofoam cups Based on the student's observation, calculate the enthalpy of dissolution of NH4Br(s) in kJ/mol Reaction occurs in Assume the specific heat of the solution is equal to the specific heat of water solution kJ/mol AHdissolution etro CangL Submit Answer Retry Entire Group 9 more group attempts remaining

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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23. Salt A and salt B were dissolved separately in 100-milliliter beakers of water. The water temperatures were méasured and recorded as shown in the table below: Salt A Salt B Initial water temperature: 25.1°C Final water temperature: 25.1°C 20.0°C 30.2°C Which statement is a correct interpretation of these data? a) The dissolving of only salt A was endothermic b) The dissolving of only salt B was exothermic c) The dissolving of both salt A and salt B was endothermic đ) The dissolving of salt A was exothermic and the dissolving of salt B was endothermic 24. The graph to the right represents the uniform cooling of a substance, starting with the substance as a gas above its boiling point. How much time passes between the first appearance of the liquid phase of the substance and the presence of the substance completely in its solid phase? a) 5 minutes b) 2 minutes c) 7 minutes d) 4 minutes e) impossible to tell from the information given 150- 100- 50- 01+23 4 5 6 7 8 9 10 11 12 13 14 25.…
A 6.61g sample of an unknown salt (MM=116.82g//mol) is dissolved in 150.00g 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 total heat for the dissolution reaction of the 6.61 g of salt
A 6.61g sample of an unknown salt (MM=116.82g//mol) is dissolved in 150.00g 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. Given that 156.61 g of solution increased in temperature by 4.82 °C, what quantity of heat, in J, was gained by the solution? Assume the specific heat of the solution is the same as water, 4.184 J/g• °C.
The heat released when one mole of water is formed from the elements is 1,198 kJ. An experiment was conducted that permitted water to form in this manner, and the heat was contained in 2.0 liters of water. The water temperature before the reaction was 34.5°C, and after the reaction it had risen to 52.0°C. How many moles of water were formed? (The specific heat of water is 4.184 J/g·°C.)Answer: 0.12 mole (Can you explain how?)
A 5.71 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. What quantity in moles of the unknown salt were used in the reaction?
When 26.6 g of potassium chloride dissolves in 300.0g of water, the temperature drops from 26.1 degrees Celcius to 11.7 degrees C. The Ccal of the calorimeter is 22.0 J/(degrees C). Write an equation for solid potassium chloride dissociating into ions when it dissolves in water.
25. Dissolving 3.0 g of CaCl2(s) in 150.0 g of water in a calorimeter at 22.4 °C causes the temperature to rise to 25.8 °C. What is the approximate amount of heat involved in the dissolution, assuming the specific heat of the resulting solution is 4.18 J/g °C? Is the reaction exothermic or endothermic?
1) A 0.416 g sample of KCl is added to 56.5 g of water in a calorimeter. If the temperature decreases by 1.24°C, what is the approximate amount of heat (in J) involved in the dissolution of the KCl, assuming the heat capacity of the resulting solution is 4.18 J/g°C? _____ J 2) Is the reaction exothermic or endothermic?
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