PQ-12. A 1.00 g sample of glucose, C H20. is burned in a bomb calorimeter, the...
When a 3.08 g sample of liquid octane (C8H18) is burned in a bomb calorimeter, the temperature of the calorimeter rises by 26.9 oC. The heat capacity of the calorimeter, measured in a separate experiment, is 6.22 kJ/∘C . The calorimeter also contains 3.00 kg of water, specific heat capacity of 4.18 J/g°C. Determine the heat of combustion of octane in units of kJ/mol octane.
A 0.44 mol sample of a substance is burned in a bomb calorimeter with a heat capacity of 8.87 kJ/C. The temperature increases by 8.36 C. What is ΔHrxn (in kJ/mol) for the combustion of the substance?
When a 3.80-g sample of liquid octane (C8H18) is burned in a bomb calorimeter, the temperature of the calorimeter rises by 26.5 ∘C. The heat capacity of the calorimeter, measured in a separate experiment, is 6.21 kJ/∘C . You may want to reference (Page 265) Section 6.5 while completing this problem. Part A Determine ΔE for octane combustion in units of kJ/mol octane. Express your answer using three significant figures.
A 1.764-g sample of heptanoic acid, C7H14O2 (130.19 g/mol) was burned in a bomb calorimeter with excess oxygen. The temperature of the calorimeter and the water before combustion was 23.68 °C; after combustion the calorimeter and the water had a temperature of 32.12 °C. The calorimeter had a heat capacity of 500 J/K, and contained 1.462 kg of water. Use these data to calculate the molar heat of combustion (in kJ) of heptanoic acid.
A 1.25-g sample of a compound is burned in a bomb calorimeter, producing a temperature change from 20.23 °C to 27.65 °C. The heat capacity of the calorimeter is determined to be 5.81 kJ/°C. What is ΔE (aka s ΔU, in kJ/g) for the combustion of this compound? Enter your answer as an integer.
7. A 2.548-9 sample of valine, CsH ,NO, (117.15 g/mol) was burned in a bomb calorimeter with excess oxygen. The temperature of the calorimeter and the water before combustion was 18.42 °C, after combustion the calorimeter and the water had a temperature of 29.13 °C. The calorimeter had a heat capacity of 633 J/K, and contained 1.255 kg of water. Use these data to calculate the molar heat of combustion (in kJ) of valine.
25. A 8,2 g sample of propane, C3H8, is burned inside a bomb calorimeter containing 2500 g of water initially at 20.6 °C. Calculate the final temperature of the bomb calorimeter system if AH comb for propane is -103.9 kJ/mol and the heat capacity of the bomb calorimeter is 2.25 kJ/°C. 1) 34.16°C 2) 22.12°C 3) 19.08°C 4) 17.61°C
Ignition wires heat sample Thermometer Stirrer A bomb calorimeter, or constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy content of 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 0.319-g sample of phenanthrene (C14H10 in a bomb calorimeter containing 1070. g of water....
A 0.559-g sample of 9,10-anthracenedione (C14H302) is burned in a bomb calorimeter and the temperature increases from 24.50 °C to 27.50 °C The calorimeter contains 1.15x10g of water and the bomb has a heat capacity of 876J/°C. Based on this experiment, calculate AE for the combustion reaction per mole of 9,10-anthracenedione burned (kJ/mol). C14H2O2() + 15 O2(g)— 14 CO2(g) + 4H2O(1) E k J/mol
7. A 2.053-g sample of ethylene glycol, CH.02 (62.07 g/mol) was burned in a bomb calorimeter with excess oxygen. The temperature of the calorimeter and the water before combustion was 16.49 °C; after combustion the calorimeter and the water had a temperature of 23.12 °C. The calorimeter had a heat capacity of 567 J/K, and contained 1.316 kg of water. Use these data to calculate the molar heat of combustion (in kJ) of ethylene glycol.