7. A 2.548-9 sample of valine, CsH ,NO, (117.15 g/mol) was burned in a bomb calorimeter...
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.
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.
7. A 2.529-g sample of glutaric acid, CsH.O.(132.12 g/mol) was burned in a bomb calorimeter with excess oxygen. The temperature of the calorimeter and the water before combustion was 23.63 °Cafter combustion the calorimeter and the water had a temperature of 32.48 °C. The calorimeter had a heat capacity of 747 J/K, and contained 0.926 kg of water. Use these data to calculate the molar heat of combustion (in kJ) of glutaric acid.
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 0.1785 g sample of magnesium was burned in an oxygen bomb calorimeter. The total heat capacity of the calorimeter plus water was 5,760 J/C. If the temperature rise of the calorimeter with water was 1.25*C, calculate the enthalpy of combustion(in kJ/mol) of magnesium. Mg(s) + 1/2O2(g) -> MgO(s) Write answer to three significant figures. Numeric Response
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 1.986 grams of sucrose (Molar mass 342.3 g/mol) is burned in a bomb calorimeter, the temperature of the calorimeter increases from 22.41°C to 26.63°C. If the heat capacity of the calorimeter is 4.900 kJ/°C, what is the heat of combustion of sucrose?
A 0.54 g sample of fructose (MW = 180. g/mol) is burned in a bomb calorimeter that has a heat capacity of 2.69 kJ/oC. The temperature of the calorimeter increases by 3.16oC. Calculate the molar heat of combustion of fructose using the data from this experiment. Since this experiment is carried out under conditions of constant volume, we are measuring ∆E. Your answer should be in kJ/mol and entered to 3 sig. fig. ∆E=?
A 1.0422 g sample of powdered aluminum is burned in a constant volume bomb calorimeter containing excess oxygen to form Al_2 O_3 (s) The calorimeter has a heat capacity of 8.775 kJ degree C^-1. The temperature of the calorimeter increases by 3.680 degree C. Determine the molar internal energy of combustion delta U and the molar enthalpy of combustion delta H for aluminum at 25 degree C. 4 Al (s) + 3 O_2 (g) middot 2 Al_2 O_3 (s)
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