A 0.456 g (176.1 g/mol) sample of acid in question 11 is burned in a bomb...
A 0.456 g (176.1 g/mol) sample of acid in question 11 is burned in a bomb calorimeter.
Calculate the change in enthalpy if the temperature for 1350 g of water in the calorimeter changes from 21.5 oC to 30.4 oC. The heat capacity of the calorimeter is 564 kJ/oC.
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A 0.456 g (176.1 g/mol) sample of acid in question 11 is burned
in a bomb...
A 1.764-g sample of heptanoic acid, C7H14O2 (130.19 g/mol) was burned in a bomb calorimeter with...
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...
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.
A 0.375-g sample of 2-naphthylacetic acid (C12H1002) is burned in a bomb calorimeter and the temperature increases from...
A 0.375-g sample of 2-naphthylacetic acid (C12H1002) is burned in a bomb calorimeter and the temperature increases from 25.80 °C to 28.00 °C. The calorimeter contains 1.06x103 g of water and the bomb has a heat capacity of 903 J/°C. Based on this experiment, calculate AE for the combustion reaction per mole of 2-naphthylacetic acid burned (kJ/mol). C12H1002()+27/2 O2(g) —>12 CO2(g) +5 H2O(1) AE = kJ/mol
A 0.54 g sample of fructose (MW = 180. g/mol) is burned in a bomb calorimeter...
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 0.1785 g sample of magnesium was burned in an oxygen bomb calorimeter. The total heat...
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
When a 3.08 g sample of liquid octane (C8H18) 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 1.20-g sample of maleic acid (C4H4O4) is burned in a bomb calorimeter and the temperature...
A 1.20-g sample of maleic acid (C4H4O4) is burned in a bomb calorimeter and the temperature increases from 24.70 °C to 27.41 °C. The calorimeter contains 1000 g of water and the bomb has a heat capacity of 839 J/°C. The heat capacity of water is 4.184 J g-1°C-1. Based on this experiment, calculate ΔE for the combustion reaction per mole of maleic acid burned.
7. A 2.548-9 sample of valine, CsH ,NO, (117.15 g/mol) was burned in a bomb calorimeter...
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.
7. A 2.053-g sample of ethylene glycol, CH.02 (62.07 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.
5. (10 points) A 2.20 g sample of fructose (CoH12Os) is burned in a bomb calorimeter...
5. (10 points) A 2.20 g sample of fructose (CoH12Os) is burned in a bomb calorimeter containing 1350 g water at an initial temperature of 21.00 °c. After the reaction the temperature of the water is 23.52 °C. The heat capacity of the bomb is 450 J/°C. The specific heat capacity of water is 4.184 J/g. C. Calculate the quantity of heat released per mole of fructose in kJlmol.
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.
A 0.375-g sample of 2-naphthylacetic acid (C12H1002) is burned in a bomb calorimeter and the temperature increases from 25.80 °C to 28.00 °C. The calorimeter contains 1.06x103 g of water and the bomb has a heat capacity of 903 J/°C. Based on this experiment, calculate AE for the combustion reaction per mole of 2-naphthylacetic acid burned (kJ/mol). C12H1002()+27/2 O2(g) —>12 CO2(g) +5 H2O(1) AE = kJ/mol
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
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.
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.
5. (10 points) A 2.20 g sample of fructose (CoH12Os) is burned in a bomb calorimeter containing 1350 g water at an initial temperature of 21.00 °c. After the reaction the temperature of the water is 23.52 °C. The heat capacity of the bomb is 450 J/°C. The specific heat capacity of water is 4.184 J/g. C. Calculate the quantity of heat released per mole of fructose in kJlmol.
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