In an experiment, a 0.5002 g sample of tridecanedioic acid (C13 H24 O4) is burned completely in a bomb calorimeter. Thecalorimeter is surrounded by 1.165 × 10³ g of water. Duringthe combustion the temperature increases from 21.99 to 24.52°C. The heat capacity of water is 4.184 J·g¯¹. °C-¹.The heat capacity of the calorimeter was determined in aprevious experiment to be 904.0 J. °C¯¹.Assuming that no energy is lost to the surroundings, calculatethe molar heat of combustion of tridecanedioic acid based onthese data.C13H24 O4(s) + 17O2 (g) → 12H₂O(l) + 13CO2 (g) + EnergykJ/molMolar Heat of Combustion =

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13 H24 O4) is burned completely in calorimeter is surrounded by 1.165 che combustion the temperature incr C. The heat capacity of water is 4.1 The heat capacity of the calorimeter previous experiment to be 904.0 J · Assuming that no energy is lost to th the molar heat of combustion of trid

13 H24 O4) is burned completely in calorimeter is surrounded by 1.165 che combustion the temperature incr C. The heat capacity of water is 4.1 The heat capacity of the calorimeter previous experiment to be 904.0 J · Assuming that no energy is lost to th the molar heat of combustion of trid

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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