Homework Answers
Calorimetric experiment is used to calculate the energy changes in chemical reaction. In a calorimeter, when a chemical reaction releases or absorbs energy, it results in change in temperature of calorimeter as well. So, the total energy released or absorbed during the reaction includes the energy absorbed or released by calorimer.
Energy absorbed by calorimeter= heat capacity of calorimeter× increase in temperature of calorimeter= energy released by the reaction
Hence, to calculate the energy changes of the reaction, we need to determine heat capacity of calorimeter.
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b. In a calorimetric experiment, why is it important to determine the heat capacity of the...
b. In a calorimetric exp periment, why is it important to determine the heat capacity of...
b. In a calorimetric exp periment, why is it important to determine the heat capacity of the -calorimeter? be able No losorbe a lot af h ea 2. Two solutions namely, 500 mL of 0.50 M HCl and 500 mL of 0.50 M NaOH at the same temperature of 2L6C are mixed in a constant-pressure calorimeter. The heat capacity of the calorimeter was450 J/oC. Given thatthe-specific heat of the solution is 4.184 J/g C, the density of the solution is...
#14 A bomb calorimetric experiment was run to determine the enthalpy of combustion of ethanol. The...
#14 A bomb calorimetric experiment was run to determine the enthalpy of combustion of ethanol. The reaction is The bomb had a heat capacity of 540 J/K, and the calorimeter contained 690 g of water. Burning 4.50 g of ethanol, resulted in a rise in temperature from 16.7 °C to 20.6 °C. Calculate the enthalpy of combustion of ethanol, in kJ/mol. (The specific heat capacity of liquid water is 4.184 J/g ⋅ K.) Enthalpy of combustion = _____ kJ/mol
A bomb calorimetric experiment was run to determine the enthalpy of combustion of ethanol. The reaction...
A bomb calorimetric experiment was run to determine the enthalpy of combustion of ethanol. The reaction is C2H5OH(l) + 3 O2(g) → 2 CO2(g) + 3 H2O(l) The bomb had a heat capacity of 500 J/K, and the calorimeter contained 610 g of water. Burning 4.50 g of ethanol, C2H5OH(L) resulted in a rise in temperature from 16.5 °C to 20.9 °C. Calculate the enthalpy of combustion of ethanol, in kJ/mol. (The specific heat capacity of liquid water is 4.184...
1. Briefly explain why the heat capacity of the calorimeter must be calculated in this experiment....
1. Briefly explain why the heat capacity of the calorimeter must be calculated in this experiment. The experiment includes the calibration of the calorimeter, the measurement of temperatures to determine enthalpy change. Chemicals include ammonium hydroxide, hydrochloric acid and ammonium chloride.
Two experiments were conducted in a bomb calorimeter. The first one to determine the heat capacity...
Two experiments were conducted in a bomb calorimeter. The first one to determine the heat capacity of the calorimeter, the second to determine the heat of combustion of the carcinogenic substance benzene (C6H6). In the first experiment, the temperature rises from 22.37degrees C to 24.68degrees C when the calorimeter absorbs 5682 J of heat. the second experiment, the comustion of 0.258g of benzene increases the temperature from 22.37degreesC to 26.77degreesC. Determine the heat of combustion for 1 mol of benzene.
In the specific heat capacity experiment, the unknown object was cooled, then placed in a calorimeter...
In the specific heat capacity experiment, the unknown object was cooled, then placed in a calorimeter that contains water. The temperature of the calorimeter and water was measured using a temperature probe. The data was fitted using natural exponent function: 20.9+(22.9-20.9) exp(-t/0.66) Determine the initial temperature of the calorimeter and water mixture.
what is the heat lost by copper snd the heat capacity of calorimeter? EXPERIMENT 7 Thermochemistry:...
what is the heat lost by copper snd the heat capacity of
calorimeter?
EXPERIMENT 7 Thermochemistry: Calorimetry and Hess's Law Data Sheet Part A-Calibration of the Calorimeter Mass of copper Mass of empty, dry calorimeter Mass of calorimeter plus water 172.1146 168.602g 229.0189 60.416g 72.005 23.6 °C Mass of water 39.0°C Temperature of copper (boiling water, T) Initial temperature of calorimeter and water, T. Final temperature of metal/water mixture, T, AT for copper T AD AT for water Heat lost...
In the specific heat capacity experiment, the unknown object was cooled, then placed in a calorimeter...
In the specific heat capacity experiment, the unknown object was cooled, then placed in a calorimeter that contain water. The temperature of the calorimeter and water was measured using a temperature probe. The data was fitted using natural exponent function: 20.3+(24.7-20.3) exp(-t/0.51) Determine the ambient temperature.
A bomb calorimeter, or constant volume calorimeter, is a device often used to determine the heat...
A bomb calorimeter, or constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy sontent of foods. lastered 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 0.500-g sample of benzoic acid (C H02) in a bomb calorimeter containing 1030. g of water. The temperature increases...
In the specific heat capacity experiment, the unknown object has a mass of 0.085 kg and...
In the specific heat capacity experiment, the unknown object has a mass of 0.085 kg and was cooled to -6C. Then, it was placed in a calorimeter (mcalorimeter = 0.12 kg) that contain water (mwarter = 0.27 kg) at a temperature of 28 oC. After 5 minutes the temperature dropped to 23C. Determine the heat lost by the calorimeter. (cwater = 4186 J/kg. oC and ccalorimeter = 900 J/kg. oC)
b. In a calorimetric exp periment, why is it important to determine the heat capacity of the -calorimeter? be able No losorbe a lot af h ea 2. Two solutions namely, 500 mL of 0.50 M HCl and 500 mL of 0.50 M NaOH at the same temperature of 2L6C are mixed in a constant-pressure calorimeter. The heat capacity of the calorimeter was450 J/oC. Given thatthe-specific heat of the solution is 4.184 J/g C, the density of the solution is...
A bomb calorimetric experiment was run to determine the enthalpy of combustion of ethanol. The reaction is C2H5OH(l) + 3 O2(g) → 2 CO2(g) + 3 H2O(l) The bomb had a heat capacity of 500 J/K, and the calorimeter contained 610 g of water. Burning 4.50 g of ethanol, C2H5OH(L) resulted in a rise in temperature from 16.5 °C to 20.9 °C. Calculate the enthalpy of combustion of ethanol, in kJ/mol. (The specific heat capacity of liquid water is 4.184...
what is the heat lost by copper snd the heat capacity of
calorimeter?
EXPERIMENT 7 Thermochemistry: Calorimetry and Hess's Law Data Sheet Part A-Calibration of the Calorimeter Mass of copper Mass of empty, dry calorimeter Mass of calorimeter plus water 172.1146 168.602g 229.0189 60.416g 72.005 23.6 °C Mass of water 39.0°C Temperature of copper (boiling water, T) Initial temperature of calorimeter and water, T. Final temperature of metal/water mixture, T, AT for copper T AD AT for water Heat lost...
A bomb calorimeter, or constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy sontent of foods. lastered 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 0.500-g sample of benzoic acid (C H02) in a bomb calorimeter containing 1030. g of water. The temperature increases...
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