A 1.800-g sample of solid phenol (C6H5OH(s)) was burned in a bomb calorimeter, which has a total heat capacity of 11.66...
A 1.800-g sample of solid phenol (C6H5OH(s)) was burned in a bomb calorimeter, which has a total heat capacity of 11.66 kJ/∘C. The temperature of the calorimeter plus its contents increased from 21.36∘C to 26.37∘C
1.Write a balanced chemical equation for the reaction that takes place in the bomb calorimeter.(Identify all phases)
2.What is the heat of combustion per gram of phenol?
3.What is the enthalpy per mole of phenol?
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A 1.800-g sample of solid phenol (C6H5OH(s)) was burned in a bomb calorimeter, which has a total heat capacity of 11.66...
A 1.800-g sample of solid phenol (C6H5OH(s)) was burned in a bomb calorimeter, which has a...
A 1.800-g sample of solid phenol (C6H5OH(s)) was burned in a bomb calorimeter, which has a total heat capacity of 11.66 kJ/∘C. The temperature of the calorimeter plus its contents increased from 21.36∘C to 26.37∘C. A. Write a balanced chemical equation for the reaction that takes place in the bomb calorimeter. Express you answer as a chemical equation including phases. B. What is the heat of combustion per gram of phenol? Express the heat in kilojoules per gram to three...
A 2.300 −g sample of quinone (C6H4O2) is burned in a bomb calorimeter whose total heat...
A 2.300 −g sample of quinone (C6H4O2) is burned in a bomb calorimeter whose total heat capacity is 7.854kJ/∘C. The temperature of the calorimeter increases from 23.84 ∘C to 31.29 ∘C Part A What is the heat of combustion per gram of quinone? Part B What is the heat of combustion per mole of quinone?
3. A 2.200 g sample of quinone (CH,02) is burned in a bomb calorimeter whose total...
3. A 2.200 g sample of quinone (CH,02) is burned in a bomb calorimeter whose total heat capacity is 7.854 kJ/°C. The temperature of the calorimeter increases from 23.44 to 30.57°C. a. What quantity of heat was produced by the combustion of the quinone? b. What is the heat of combustion per gram of quinone? c. What is the heat of combustion per mole of quinone?
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
. (15. A 1.600g sample of quinone (C6H,02) was burned in a bomb calorimeter whose total...
. (15. A 1.600g sample of quinone (C6H,02) was burned in a bomb calorimeter whose total heat capacity is 7.854 kJ/°C. The temperature of the calorimeter increases from 21.34 °C to 32.57 °C. What is the heat of combustion per gram of quinone? Per mole of quinone? (10 pts.)
Thermometer A sample of solid bianthracene (C28H18) that weighs 0.5254 g is burned in an excess...
Thermometer A sample of solid bianthracene (C28H18) that weighs 0.5254 g is burned in an excess of oxygen to CO2(g) and H2O() in a constant-volume calorimeter at 25.00 °C. The temperature rise is observed to be 2.190 °C. The heat capacity of the calorimeter and its contents is known to be 9.405x103 JK. Ignition wires heat sample Stirrer (a) Write and balance the chemical equation for the combustion reaction. Use the lowest possible coefficients. Use the pull-down boxes to specify...
A 0.559-g sample of 9,10-anthracenedione (C14H302) is burned in a bomb calorimeter and the temperature increases...
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
A 2.991 g sample of a new organic material is combusted in a bomb calorimeter. The temperature of the calorimeter and i...
A 2.991 g sample of a new organic material is combusted in a bomb calorimeter. The temperature of the calorimeter and its contents increase from 23.95 °C to 27.24 °C. The heat capacity (calorimeter constant) of the calorimeter is 28.85 kJ/°C, what is the heat of combustion per gram of the material? heat of combustion: kJ/g
A 0.44 mol sample of a substance is burned in a bomb calorimeter with a heat...
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?
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.
3. A 2.200 g sample of quinone (CH,02) is burned in a bomb calorimeter whose total heat capacity is 7.854 kJ/°C. The temperature of the calorimeter increases from 23.44 to 30.57°C. a. What quantity of heat was produced by the combustion of the quinone? b. What is the heat of combustion per gram of quinone? c. What is the heat of combustion per mole of quinone?
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
. (15. A 1.600g sample of quinone (C6H,02) was burned in a bomb calorimeter whose total heat capacity is 7.854 kJ/°C. The temperature of the calorimeter increases from 21.34 °C to 32.57 °C. What is the heat of combustion per gram of quinone? Per mole of quinone? (10 pts.)
Thermometer A sample of solid bianthracene (C28H18) that weighs 0.5254 g is burned in an excess of oxygen to CO2(g) and H2O() in a constant-volume calorimeter at 25.00 °C. The temperature rise is observed to be 2.190 °C. The heat capacity of the calorimeter and its contents is known to be 9.405x103 JK. Ignition wires heat sample Stirrer (a) Write and balance the chemical equation for the combustion reaction. Use the lowest possible coefficients. Use the pull-down boxes to specify...
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
A 2.991 g sample of a new organic material is combusted in a bomb calorimeter. The temperature of the calorimeter and its contents increase from 23.95 °C to 27.24 °C. The heat capacity (calorimeter constant) of the calorimeter is 28.85 kJ/°C, what is the heat of combustion per gram of the material? heat of combustion: kJ/g
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