onmeter is an insulated device in which aical reaction is contained. By measuring theerature change, AT, we can calculate thereleased or absorbed during the reaction usingollowing equation:Part BConsider the reactionq = specific heat x mass x ATC12 H22011 (s) + 1202(g)→12CO2(g) + 11H20(1)if the calorimeter has a predetermined heatacity, C, the equation becomesin which 10.0 g of sucrose, C12 H22011, was burned in a bomb calorimeter with a heat capacity of 7.50kJ/°C. The temperature increase inside the calorimeter was found to be 22.0 °C. Calculate the change ininternal energy, AE, for this reaction per mole of sucrose.q = C x ATExpress the change in internal energy in kilojoules per mole to three significant figures.constant pressure, the enthalpy change for theaction, AH, is equal to the heat, qp; that is,• View Available Hint(s)AH = 9pVα ΑΣφut it is usually expressed per mole of reactant andwith a sign opposite to that of q for thesurroundings. The total internal energy change,AE (sometimes referred to as AU), is the sum ofheat, g, and work done, w.kJ/molAE =AE =q+ wSubmitHowever, at constant volume (as with a bombcalorimeter) w = 0 and so AE= g..Next >Provide FeedbackP PearsonCopyright © 2021 Pearson Education Inc. All rights reserved. Terms of Use | Privacy Policy I Permissions| Contact Us |VI 6:43 A calorimeter is an insulated device in which achemical reaction is contained. By measuring thetemperature change, AT, we can calculate theheat released or absorbed during the reaction usingthe following equation:Constants Periodic TablePart Aq = specific heat x mass x ATA calorimeter contains 30.0 mL of water at 14.0 °C. When 1.70 g of X (a substance with a molar mass of76.0 g/mol ) is added, it dissolves via the reactionOr, if the calorimeter has a predetermined heatcapacity, C, the equation becomesX(s) + H2O(1)→X(aq)q=C x ATand the temperature of the sblution increases to 30.0 °CAt constant pressure, the enthalpy change for thereaction, AH, is equal to the heat, qp; that is,Calculate the enthalpy change, AH, for this reaction per mole of X.Assume that the specific heat of the resulting solution is equal to that of water (4.18 J/(g. °C)J, that densityof water is 1.00 g/mL, and that no heat is lost to the calorimeter itself, nor to the suroundings.ΔΗpExpress the change in enthalpy in kilojoules per mole to three significant figures.but it is usually expressed per mole of reactant andwith a sign opposite to that of q for thesurroundings. The total internal energy change,AE (sometimes referred to as AU), is the sum ofheat, g. and work done, w:• View Available Hint(s)να ΑΣφ?AE=q+ uwkJ/molHowever, at constant volume (as with a bombcalorimeter) w = 0 and so AE = qu-ΔΗ-SubmitPearsonCopyright © 2021 Pearson Education Inc. All rights reserved. Terms of Use | Privacy Policy I Permissions I Contact Us /VI6 43

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Consider the reaction C12 H22O11 (s) + 1202(g)→12CO2 (g) + 11H,0(1) in which 10.0 g of sucrose, C12 H22O11, was burned in a bomb calorimeter with a heat capacity of 7.50 kJ/ C. The temperature increase inside the calorimeter was found to be 22.0°C. Calculate the change in internal energy, AE, for this reaction per mole of sucrose. Express the change in internal energy in kilojoules per mole to three significant figures. • View Available Hint(s) ? kJ/mol AE = Submit

Consider the reaction C12 H22O11 (s) + 1202(g)→12CO2 (g) + 11H,0(1) in which 10.0 g of sucrose, C12 H22O11, was burned in a bomb calorimeter with a heat capacity of 7.50 kJ/ C. The temperature increase inside the calorimeter was found to be 22.0°C. Calculate the change in internal energy, AE, for this reaction per mole of sucrose. Express the change in internal energy in kilojoules per mole to three significant figures. • View Available Hint(s) ? kJ/mol AE = Submit

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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A 3.971 g sample of a new organic material is combusted in a bomb calorimeter. The temperature of the calorimeter and its contents increase from 24.87 ∘C to 28.06 ∘C. The heat capacity (calorimeter constant) of the calorimeter is 36.35 kJ/ ∘C, what is the heat of combustion per gram of the material?
A chemist measures the enthalpy change AH during the following reaction: COC1₂(9) + 4 NH3(9)→ CO(NH₂),(s) + 2NH4Cl(s) Use this information to complete the table below. Round each of your answers to the nearest kJ/mol. esc COC₁₂ (8) + 2NH₂(g) → CO(NH₂), (s) + NH₂Cl(s) 1 1 ẩCO(NH,),() + ≈NH,C() → † COCI,(8) + NH, (8) CO(NH₂)₂ (s) + 2NH₂Cl(s) → COCL, (g) + 4NH, (g) Explanation THE Check reaction I > AH=-559. kJ Costa ΔΗ kJ ☐ kJ KJ MacBook Pro x10 X S © 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Acc You MOSISO L
Part B 2.0000 g of the unknown compound is burned in a bomb calorimeter. During the combustion, the temperature of the calorimeter increases from 23.125°C to 28.997 °C. During calibration, the heat capacity of the calorimeter was found to be 9.9897kJ °C-1. In the previous experiment, the molar mass of the substance was found to be 148.16 gmol-1. What is AcombU for the unknown compound? να ΑΣφ ? kJ mol1 Submit Request Answer
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Let's use our knowledge of constant volume (bomb) calorimetry to determine the heat energy in a given food sample, say a hamburger. A typical hamburger has a serving size of 105 g and consists of approximately 20% protein (21.0 g), 33% fat (34.7 g), and 47% carbohydrate (49.3 g). Assume that the heat capacity of the bomb calorimeter is 8.39 kJ K-¹, and the increase in water temperature was 13.2 K. Q5.38 Homework Unanswered How many Calories (Cal) are in the hamburger described above? Respond with the correct number of significant figures in scientific notation (Use E notation and only 1 digit before decimal e.g. 2.5E5 for 2.5 x 105) Type your numeric answer and submit Unanswered • 4 attempts left Submit
When 1.550 g of liquid hexane (C6H14) undergoes combustion in a bomb calorimeter, the temperature rises from 25.87 °C to 38.13 °C. Find AErxn for the reaction in kJ/mol hexane. The heat capacity of the bomb calorimeter, determined in a separate experiment, is 5.73 kJ/°C. Express your answer in kilojoules per mole to three significant figures. AErxn of hexane = Submit VE ΑΣΦ Request Answer ? kJ/mol
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The combustion of 1.880 g of sucrose, C,H,,O, (s), in a bomb calorimeter with a heat capacity of 4.30 kJ/°C results in an increase in the temperature of the calorimeter and its contents from 22.31 °C to 29.52 °C. What is the internal energy change, AU, for the combustion of 1.880 g of sucrose? AU = kJ Calculate the enthalpy of combustion, AHe, of sucrose in kilojoules per mole. kJ/mol AH. = A étv w MacBook Air DI DD 80 888 F12 F11 F9 F10 F7 FB 3 F4 F5 F6
A bomb calorimeter, or constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy available from 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 0.508-g sample of benzil (C14H1002) in a bomb calorimeter containing 1060. g water. The temperature increases from 24.70 °C to 27.80 °C. The specific heat capacity of water is 4.184 J gl°C1. The combustion enthalpy is -6784 k]/mol benzil. C14H1002(s) + 31/2 02(g) →14 CO2(g) + 5 H20(I) A,H° = -6784 kJ/mol %3D Calculate the heat capacity of the calorimeter. heat capacity of calorimeter = J/C
CH,,0, (s) + 60, (g) → 6CO, (g) + 6H,0(g) 12 The combustion of glucose was performed in a bomb calorimeter. Qwater= 14.52kJ. The heat capacity of the bomb is Ca = 2.273 kJ/C and the change in temperature was 28.49C. If 0.03255 moles of glucose was used in the bomb calorimeter, then what is AHmy in kJ/mol? a. ´cal rnx