In a calorimetry experiment 3.2 g of potassium hydroxide is dissolved in 400 mL water in a thermos flask. The temperature increase in the solution is 7 \deg C. The effective mass of the glass in the thermos flask ( mcal) is 0.040 kg. The heat capacity of the solution (Cs) is 4.04 kJkg-1K-1. The heat capacity of the calorimeter (Ccal) is 0.387 kJkg-1K-1. Remember to enter your answer using the specified number of significant figures, but keep the entire number in your calculator for use in further calculations. Part B - Calculating qsolution Calculate the heat absorbed by the solution (qsolution) Give your answer to four significant figures. Part C- Calculating qcalorimeter Calculate the heat absorbed by the glass in the calorimeter (qcalorimeter). Give your answer to four significant figures. Part D- Calculating qtotal Calculate the total heat transferred for the reaction (qtotal) Give your answer to four significant figures. Calculate the number of moles of KOH used in the experiment (n). Give your answer to four significant figures. View Available Hint(s) Calculate the enthalpy change (\Delta H) for the dissolution of one mole of KOH, that is, for the reaction: KOH(s) -> K+(aq) + OH-(aq) Remember to consider the sign of \Delta H. Give your answer to 2 significant figures.
In a calorimetry experiment 3.2 g of potassium hydroxide is dissolved in 400 mL water in a thermos flask. The temperature increase in the solution is 7 \deg C. The effective mass of the glass in the thermos flask ( mcal) is 0.040 kg. The heat capacity of the solution (Cs) is 4.04 kJkg-1K-1. The heat capacity of the calorimeter (Ccal) is 0.387 kJkg-1K-1. Remember to enter your answer using the specified number of significant figures, but keep the entire number in your calculator for use in further calculations. Part B - Calculating qsolution Calculate the heat absorbed by the solution (qsolution) Give your answer to four significant figures. Part C- Calculating qcalorimeter Calculate the heat absorbed by the glass in the calorimeter (qcalorimeter). Give your answer to four significant figures. Part D- Calculating qtotal Calculate the total heat transferred for the reaction (qtotal) Give your answer to four significant figures. Calculate the number of moles of KOH used in the experiment (n). Give your answer to four significant figures. View Available Hint(s) Calculate the enthalpy change (\Delta H) for the dissolution of one mole of KOH, that is, for the reaction: KOH(s) -> K+(aq) + OH-(aq) Remember to consider the sign of \Delta H. Give your answer to 2 significant figures.
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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Thermochemistry
Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.
Exergonic Reaction
The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.
Question
Transcribed Image Text:In a calorimetry experiment 3.2 g of potassium hydroxide is dissolved in 400 mL water in a thermos flask.
The temperature increase in the solution is 7 \deg C. The effective mass of the glass in the thermos flask (
mcal) is 0.040 kg. The heat capacity of the solution (Cs) is 4.04 kJkg-1K-1. The heat capacity of the
calorimeter (Ccal) is 0.387 kJkg-1K-1. Remember to enter your answer using the specified number of
significant figures, but keep the entire number in your calculator for use in further calculations. Part B -
Calculating qsolution Calculate the heat absorbed by the solution (qsolution) Give your answer to four
significant figures. Part C- Calculating qcalorimeter Calculate the heat absorbed by the glass in the
calorimeter (qcalorimeter). Give your answer to four significant figures. Part D - Calculating qtotal Calculate
the total heat transferred for the reaction (qtotal) Give your answer to four significant figures. Calculate the
number of moles of KOH used in the experiment (n). Give your answer to four significant figures. View
Available Hint(s) Calculate the enthalpy change (\Delta H) for the dissolution of one mole of KOH, that is, for
the reaction: KOH(s) -> K+(aq) + OH-(aq) Remember to consider the sign of \Delta H. Give your answer
to 2 significant figures.
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