b)Combustion reactionIn the same calorimeter, 1.04 g of benzoic acid were burnt completely (forming onlyCO2 and H2O) under oxygen atmosphere, which caused a temperature increase of8.8 K. Formulate the stoichiometrically correct reaction equation, calculate the molarenthalpy of combustion AcHm and the molar enthalpy of formation AfHm of benzoic acid.AHH20=-286.4 kJ mol-1A, Hoz =-393.509 kJ mol-1A Ho₂ = 0 kJ mol-1Benzoic acidC7H6O2OH

Step 1: The balanced chemical equation = combustion of…

Answered: b) Combustion reaction In the same…

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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5.000 g of Compound X with molecular formula C-H₂ are burned in a constant-pressure calorimeter containing 50.00 kg of water at 25 °C. The temperature of the water is observed to rise by 1.042 °C. (You may assume all the heat released by the reaction is absorbed by the water, and none by the calorimeter itself.) Calculate the standard heat of formation of Compound X at 25 °C. Be sure your answer has a unit symbol, if necessary, and round it to the correct number of significant digits. 1 00 x10
PCIS(s) can be prepared by the reaction PCl3(0) + Cl2(g) PCls(s). Calculate the enthalpy change (in kJ) that accompanies the production of 100.0 g of PCIs(s) by the above reaction, given the following data. Pals) + 6 Cl2(g) -4 PCI3(1) AH° = -1280 kJ per mole of P4(s) Pa(s) + 10 Cl2(g) -4 PCI5(s) AH = -1774 kJ per mole of P4(s) -124 O-258 O+124 O+59.3 O-59.3
2.000 g of Compound X with molecular formula C5H₁0 are burned in a constant-pressure calorimeter containing 45.00 kg of water at 25 °C. The temperature 10 of the water is observed to rise by 0.4696 °C. (You may assume all the heat released by the reaction is absorbed by the water, and none by the calorimeter itself.) Calculate the standard heat of formation of Compound X at 25 °C. Be sure your answer has a unit symbol, if necessary, and round it to 3 significant digits. 0 00 X Ś x10
Calculate the enthalpy of combustion (kJ/mol) of methyl linoleate (C₁₉H₃₄O₂), an important component of many biodiesel fuels made from corn oil and methanol, given the following standard enthalpies of formation: CO₂(g) = -393.5 kJ/mol H₂O(l) = -285.8 kJ/mol C₁₉H₃₄O₂(l) = -645.7 kJ/mol
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
2.000g of Compound X with molecular formula C4H6 are burned in a constant-pressure calorimeter containing 40.00kg of water at 25°C. The temperature of the water is observed to rise by 0.5325°C. (You may assume all the heat released by the reaction is absorbed by the water, and none by the calorimeter itself.) Calculate the standard heat of formation of Compound X at 25°C. Be sure your answer has a unit symbol, if necessary, and round it to 3 significant digits.
None
1 If the standard enthalpy of cembustion of gaseous cyclopropane, C3H6, is -2091.2 kJ mol- at 25 C, calculate the standard enthalpy of formation of the compound at 298 K. (The standard enthalpy of combustion is the heat of combustion of one mole of a compound to the most stable combustion products, which are CO2(g) and H20(1) in the case of hydrocarbons. The standard enthalpy of formation is the enthalpy of formation of one mole of a compound from its constituent elements, the compound and its constituent elements in their standard states.)

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