The combustion of 1.516 g of fructose, C, H, O,(s), in a bomb calorimeter with a heat capacity of 5.10 kJ/C results in an increase in the temperature of the calorimeter and its contents from 22.71 °C to 27.35 °C. What is the internal energy change, AU, for the combustion of 1.516 g of fructose? Remember that under constant pressure AU is equal to q reaction. AU = 2983.3 Incorrect Calculate the enthalpy of combustion, AH., of fructose in kilojoules per mole. AH, = 2983.3 kJ kJ/mol

The combustion of 1.516 g of fructose, C, H, O,(s), in a bomb calorimeter with a heat capacity of 5.10 kJ/C results in an increase in the temperature of the calorimeter and its contents from 22.71 °C to 27.35 °C. What is the internal energy change, AU, for the combustion of 1.516 g of fructose? Remember that under constant pressure AU is equal to q reaction. AU = 2983.3 Incorrect Calculate the enthalpy of combustion, AH., of fructose in kilojoules per mole. AH, = 2983.3 kJ kJ/mol

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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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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In the following experiment, solid CaCl2 (M = 110.98 g/mol) is dissolved in water:CaCl2(s) → Ca2+(aq) + 2Cl-(aq) ΔsolnH = ? kJ mol−1A 4.00 g sample of CaCl2 is added to a coffee-cup calorimeter containing 125 g of H2O. The initial temperature of water in the calorimeter is 22.0°C and the final temperature is 27.5°C. What is the enthalpy change for the dissolution reaction (ΔsolnH) in kJ per mole of CaCl2? Assume the specific heat capacity of the solution is the same as water (Cs=4.18 J g-1 °C-1) and that no heat is lost to the calorimeter.
4. A copper flame calorimeter has a mass of 305 g and contains 255 g of water. When 1.01g of propanol, C,H,O, is burned in the calorimeter, the calorimeter and contents increase in temperature by 28.8 °C. Calculate the enthalpy of combustion of propanol.
A 0.576 g sample of liquid C5H12 was combusted using excess oxygen gas inside a bomb calorimeter, with the products being carbon dioxide gas and liquid water. The calorimeter's heat capacity is 4.957 kJ °C^-1. If the temperature inside the calorimeter increased from 25.0 °C to 35.1 °C, determine A,U for this reaction in kl mol (with respect to C3H12). Do not worry about how realistic the final answer is.
When 50.4 mL of 0.28 M AgNO3 and 20.8 mL of 0.28 M NaCI, both at 25.26°C, are mixed in a coffee-cup calorimeter, AgCl precipitates and the temperature of the mixture increases to 31.25°C. Calculate A H in kJ/mole of AgCl (s) produced during the reaction. (Assume that the total volume is the sum of the volumes and that the density and specific heat capacity of the solution are the same as for water: d 1.00 g/mL and c = 4.18 J/g°C). Enter AH in kJ/mol to 1 decimal place and without units.
A bomb calorimeter has a heat capacity of 4.66 kJ/°C. When 1.772 g of glucose, C6H₁2O6(s), is combusted in the bomb calorimeter, the temperature of the calorimeter and its contents increased from 22.32 °C to 28.24 °C. Calculate the change in internal energy, AU, for the combustion of 1.772 g of glucose in the bomb calorimeter. AU = -716.36 kJ
Phthalates used as plasticizers in rubber and plastic products are believed to act as hormone mimics in humans. The value of ΔHcomb for dimethylphthalate (C10H10O4) is –4685 kJ/mol. Assume 1.16 g of dimethylphthalate is combusted in a calorimeter whose heat capacity (Ccalorimeter) is 7.85 kJ/°C at 20.0 °C. What is the final temperature of the calorimeter?
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
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1. Methanol CH3OH is a potential source of fuel. An experiment was conducted to determine the enthalpy of combustion of methanol. 2.00 g of methanol was used to heat 150 g of water. The temperature of the water increased from 25°C to 87 °C. (Given that the specific heat capacity of water is 4.18 J K-1 g-1) Define the term standard enthalpy of combustion with reference to methanol. Use the data above to determine the enthalpy of combustion of methanol (show solutions). 2. Calculate the e.m.f of the following cell in the image (show solutions).
The experimental enthalpy of decomposition of H2O2 was determined using another coffee-cup calorimetry. A sample of H202 solution was placed in the calorimeter and the initial temperature of H202 solution and the calorimeter was measured. Then, KI solution was added to the solution to catalyze the decomposition of H202 to H20. This resulted to an increase of 16.9°C in the temperature. Determine the experimental enthalpy of decomposition per mole of H2O2 given the following additional information. Express your answer in kJ/mol and in 2 decimalplaces. moles H202: 0.018 mol Ccal: 54.56 J/°C mass of the solution (mainly water): 33.9 g C, of water: 4.184 J/g°C