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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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
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Fructose, C6H12O6(s), is a sugar closely related to glucose.. A 0.755 g sample of fructose was combusted with excess oxygen in a bomb calorimeter, containing 500.0 g of water. The heat capacity of the empty calorimeter was 208 J/K. The temperature of the calorimeter and the water rose from 22.00°C to 27.12°C due to the combustion reaction, which formed CO2(g) and liquid water. What is the energy change, AU (in kJ), for the combustion of one mole of fructose under these conditions? -15600 -2810 +520 +254 -804
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
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