
Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
expand_more
expand_more
format_list_bulleted
Concept explainers
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.
Expert Solution

This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
This is a popular solution
Trending nowThis is a popular solution!
Step by stepSolved in 4 steps with 40 images

Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- 18) A 6.55 g sample of aniline (C6H5NH2, molar mass = calorimeter. If the temperature rose by 32.9°C, use the information below to determine the heat capacity of the calorimeter. 93.13 g/mol) was combusted in a bomb 4 C6H5NH2(1) + 35 02(g) 24 CO2(g) + 14 H2O(g) + 4 NO2(g) AH°r rxn=-1.28 x 104 kJ A) 97.3 kJ/°C B) 38.9 kJ/°C C) 5.94 kJ/°C D) 6.84 kJ/°C E) 12.8 kJ/°C Answer: D Diff: 3 Page Ref: 6.5arrow_forwardThe symbol AH represents enthalpy change Select one: O True False In a closed system, at 25°C and 1 atmosphere of pressure, a small sample of methane is combusted. All of the methane is reacted according to the following equation: CH4(9)+ 20₂(g) → CO₂(g) + 2H₂O(1) In order to determine the enthalpy change of the system, must be assumed that the products are also at 25°C and 1 atmosphere of pressure. Select one: O True O False In Question 11, the kinetic energy of the products will be the same as the kinetic energy of the reactants. Select one: O True Falsearrow_forwardA bomb calorimeter, or constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy content of foods. Since the "bomb" itself can absorb energy, a separate experiment is needed to determine the heat capacity of the calorimeter. This is known as calibrating the calorimeter. In the laboratory a student burns a 0.491 g sample of 9,10-anthracenedione (C_14H_8O_2) in a bomb calorimeter containing 1060 g of water. The temperature increases from 25.40°C to 28.30°C. The heat capacity of water is . 4.184 J/(g*C) The molar heat of combustion is −6464 kJ per mole of 9,10-anthracenedione. C_14H_8O_2(s) +150_2(g) ---> 14CO_2(g)+4H_2O(l) + Energy Calculate the heat capacity of the calorimeter. Heat capacity =arrow_forward
- Suppose 0.100 mol of a metal (M) is combusted in excess O2(g) in a bomb calorimeter. 4M(s) + 302 2M2O3(s) The heat capacity of the empty calorimeter is 458 J/°C and the calorimeter contains 450 mL of water. As a result of the reaction, the temperature of the water rises from 25.0°C to 40.8°C Calculate AE for the reaction in KJ/molxn: Assume, DH,0 = 1.00 8_ mL J SH,0 = 4.18 g.°C -1.48 X 103 KJ/mol +1.48 X 103 KJ/mol +3.35 X 103 KJ/mol -3.35 X 103 KJ/molarrow_forward11. An isomerization reaction is to be investigated involving the enthalpy of ring opening of cyclopropane to form propene: =CH2 H3C To determine the enthalpy change of this reaction the following calorimetric data were found for the combustion of cyclopropane and propene: Reaction I Reaction II mass of substance burned C.H. (g) + 3/2 0, (e) → 3C0, (E) + 3H,0 (8) C.H. (g) + 3/2 0,(g) → 3C0,(g) + 3H,O(8) 0.28g cyclopropane 0.37 g propene volume of water 300 ml 300 mL initial temperature 22.3 °C 22.0°C final temperature a) Find the AH for Reaction I and Reaction II using the above laboratory data. (Cwater = 4.18 J/g°c) Use the AH values for reactions I and Il to determine the enthalpy change for the ring opening of cyclopropane. 33.6 °C 36.4 °Carrow_forwardSuppose 0.100 mol of a metal (M) is combusted in excess O2(g) in a bomb calorimeter. 4M(s) + 302 2M203(s) > The heat capacity of the empty calorimeter is 458 J/°C and the calorimeter contains 450 mL of water. As a result of the reaction, the temperature of the water rises from 25.0°C to 40.8°C. Calculate AE for the reaction in KJ/molxn: Assume, DH20 = 1.00 8_ mL J SH20 = 4.18 g.°C O -1.48 X 103 KJ/mol +1.48 X 103 KJ/mol +3.35 X 103 KJ/mol -3.35 X 103 KJ/molarrow_forward
- Material: Heat Copper + Heating Duration: Reset Block Mass: 5.0 g 10.0 g 2 s 100 J has been transferred to the block. Experiment Complete Click Reset for a new experiment. 8= specific heat capacity (Jg¹ °C-¹) = Tinitial 20.0 °C Specific heat capacity is a measure of the quantity of heating required to raise 1 g of a substance 1 °C (1 K). Specific heat capacity can be calculated from the equation quantity heating (J) mass (g) x AT(°C) T final 71.9 °C 9 m x AT Use the following settings: Material: Copper Heating Duration: 2.0 s Block Mass: 5.0 g Run the experiment and calculate the value of the specific heat capacity for copper. * Jg-¹ °C-1 Cengage Learning Cengage Technical Support Previous Next Save and Exitarrow_forwardWhen 150.0 mL of a 0.500 M citric acid (H3C6H5O7) solution reacts with 50.0 mL of a 3.00 M KOH solution in a coffee cup calorimeter, the temperature of all components rises from 21.2°C to 28.7°C. Assume the density and heat capacity of the solutions are the same as that of water. H3 C6 H5 O 7 (aq) + 3 KOH(aq) -> K3 C6 H5 O 7 (aq) + 3 H2 O(l) 1.Calculate ΔHrxn for the reaction as it’s written. Make sure to account for the coefficient of the limiting reactant in determining ΔHrxn . The answer is: –1.3 x 102 kJarrow_forwardA 29.300 g piece of unknown metal was heated in a hot water bath at 99.20°C. The hot metal was then transferred to a coffee-cup calorimeter [Ccal = 21.0 J/°C] containing 50.0 mL of water. Time Temperature data was collected and plotted. From the plot, the initial and final temperatures for the water were determined to be 22.50°C and 26.89°C, respectively. Calculate the molar mass of the metal and identify it using the periodic table.arrow_forward
- 4.38 g of a gas (28.1 g mol–1) was dissolved in liquid water in a calorimeter with a calorimeter constant of 76.0 J K–1. Prior to mixing everything was equilibrated to 21.2 °C. The resulting solution with a mass of 23.4 g was observed to be at a temperature of -6.8 °C and have a specific heat capacity of 4.61 J g–1 K–1. Determine q per mole for this dissolution process. a. -5150 J/mol b. -1.94 × 104 J/mol c. 2.89 × 105 J/mol d. -3.39 × 105 J/mol e. 3.30 × 104 J/molarrow_forwardA student poured 100 ml of water (density = 1.00 g / mL) into a coffee calorimeter, noted that the temperature of the water was 18.8oC, then added 5.33 g KOH. With the lid on, the mixture was stirred, temperature increased and the maximum temperature reached at the time of mixing 31.6 oC. Calculate the heat of the system in this dissolution reaction (qsys). ( Approximate the specific heat capacity, cp as 4.18 J g-1 K-1. Do not consider the contribution to the heat generated from the calorimeter; assume that this is zero. Only calculate the heat from the heat capacity of the solution. make sure you consider the sign of qsys qsys for dissolution of KOH = Jarrow_forwardConsider the following reactions: W(s) + C(graphite) ---> WC(s) What is the enthalpy of reaction (in units of kJ) of the reaction above? 2W(s) + 302lg) ---> C(graphite) + O2(g) 2WC(s) + 502(g) ---> 2WO3(s) + 2CO2(g); AH = -1685.8 kJ 2WO3(s); ---> CO2(g); AH = -393.5 kJ %3D ΔΗ--239 1.8 kJarrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistryChemistryISBN:9781259911156Author:Raymond Chang Dr., Jason Overby ProfessorPublisher:McGraw-Hill EducationPrinciples of Instrumental AnalysisChemistryISBN:9781305577213Author:Douglas A. Skoog, F. James Holler, Stanley R. CrouchPublisher:Cengage Learning
- Organic ChemistryChemistryISBN:9780078021558Author:Janice Gorzynski Smith Dr.Publisher:McGraw-Hill EducationChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningElementary Principles of Chemical Processes, Bind...ChemistryISBN:9781118431221Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. BullardPublisher:WILEY

Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning

Chemistry
Chemistry
ISBN:9781259911156
Author:Raymond Chang Dr., Jason Overby Professor
Publisher:McGraw-Hill Education

Principles of Instrumental Analysis
Chemistry
ISBN:9781305577213
Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:Cengage Learning

Organic Chemistry
Chemistry
ISBN:9780078021558
Author:Janice Gorzynski Smith Dr.
Publisher:McGraw-Hill Education

Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning

Elementary Principles of Chemical Processes, Bind...
Chemistry
ISBN:9781118431221
Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:WILEY