IgnitionwiresheatsampleThermometerStirrerA bomb calorimeter, or constant volume calorimeter, is a device often used to determine the heat ofcombustion of fuels and the energy content of foods.Since the "bomb" itself can absorb energy, a separate experiment is needed to determine the heatcapacity of the calorimeter. This is known as calibrating the calorimeter.In the laboratory a student burns a 0.429-g sample of biphenyl (C12H10) in a bomb calorimetercontaining 1170. g of water. The temperature increases from 26.00 °C to 29.00 °C. The heat capacityof water is 4.184 J gl°C-1.WaterThe molar heat of combustion is -6251 kJ per mole of biphenyl.C12H10(s) + 29/2 O2(g) →12 CO2(g) + 5 H20(1) + EnergyCalculate the heat capacity of the calorimeter.InsulatedoutsidechamberSampledishBurningsampleheat capacity of calorimeter =J/°CSteelbombCombustion (bomb) calorimeter. IgnitionwiresheatsampleThermometerStirrerA bomb calorimeter, or constant volume calorimeter, is a device often used to determine the heat ofcombustion of fuels and the energy content of foods.Since the "bomb" itself can absorb energy, a separate experiment is needed to determine the heatcapacity of the calorimeter. This is known as calibrating the calorimeter.WaterIn the laboratory a student burns a 0.434-g sample of bisphenol A (C15H1602) in a bombcalorimeter containing 1010. g of water. The temperature increases from 24.20 °C to 27.10 °C. Theheat capacity of water is 4.184 J gl°C-1.The molar heat of combustion is –7821 kJ per mole of bisphenol A.C15H1602(s) + 18 O2(g)15 CO2(g) + 8 H2O(1) + EnergyCalculate the heat capacity of the calorimeter.InsulatedoutsidechamberSampledishBurningsampleSteelbombheat capacity of calorimeter =J/°CCombustion (bomb) calorimeter.

"Since you have asked multiple question, we will solve the first question for you. If you want any…

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 0.429-g sample of biphenyl (C12H10) in a bomb calorimeter containing 1170. g of water. The temperature increases from 26.00 °C to 29.00 °C. The heat capacity of water is 4.184 Jgl°C-1. Water The molar heat of combustion is -6251 kJ per mole of biphenyl. C12H10(s) + 29/2 O2(g) →12 CO2(g) + 5 H2O(1) + Energy Calculate the heat capacity of the calorimeter. Insulated outside Sample dish Burning sample heat capacity of calorimeter J/°C Steel bomb nhomber

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 0.429-g sample of biphenyl (C12H10) in a bomb calorimeter containing 1170. g of water. The temperature increases from 26.00 °C to 29.00 °C. The heat capacity of water is 4.184 Jgl°C-1. Water The molar heat of combustion is -6251 kJ per mole of biphenyl. C12H10(s) + 29/2 O2(g) →12 CO2(g) + 5 H2O(1) + Energy Calculate the heat capacity of the calorimeter. Insulated outside Sample dish Burning sample heat capacity of calorimeter J/°C Steel bomb nhomber

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter6: Thermochemistry

Section: Chapter Questions

Problem 112AE: In a bomb calorimeter, the reaction vessel is surrounded by water that must be added for each...

See similar textbooks

Similar questions

Isooctane is a primary component of gasoline and gives gasoline its octane rating. Burning 1.00 mL of isooctane (d=0.688g/mL) releases 33.0 kJ of heat. When 10.00 mL of isooctane are burned in a bomb calorimeter, the temperature in the bomb and water rises from 23.2C to 66.5C. The bomb contains 1.00 kg of water. What is the heat capacity of the calorimeter?
Chlorine trifluoride is a toxic, intensely reactive gas. It was used in World War II to make incendiary bombs. It reacts with ammonia and forms nitrogen, chlorine, and hydrogen fluoride gases. When two moles of chlorine trifluoride react, 1196 kJ of heat are evolved. (a) Write a thermochemical equation for the reaction. (b) What is Hf for ClF3?
In the 1880s, Frederick Trouton noted that the enthalpy of vaporization of 1 mol pure liquid is approximately 88 times the boiling point, Tb, of the liquid on the Kelvin scale. This relationship is called Troutons rule and is represented by the thermochemical equation liquid gas H = 88 Tb, joules Combined with an empirical formula from chemical analysis, Troutons rule can be used to find the molecular formula of a compound, as illustrated here. A compound that contains only carbon and hydrogen is 85.6% C and 14.4% H. Its enthalpy of vaporization is 389 J/g, and it boils at a temperature of 322 K. (a) What is the empirical formula of this compound? (b) Use Troutons rule to calculate the approximate enthalpy or vaporization or one mole of the compound. Combine the enthalpy of vaporization per mole with that same quantity per gram to obtain an approximate molar mass of the compound. (c) Use the results of parts (a) and (b) to find the molecular formula of this compound. Remember that the molecular mass must be exactly a whole-number multiple of the empirical formula mass, so considerable rounding may be needed.
In a coffee-cup calorimeter, 100.0 mL of 1.0 M NaOH and 100.0 mL of 1.0 M HCI are mixed. Both solutions were originally at 24.6C. After the reaction, the final temperature is 31.3C. Assuming that all the solutions have a density of 1.0 g/cm3 and a specific heat capacity of 4.18 J/Cg, calculate the enthalpy change for the neutralization of HCl by NaOH. Assume that no heat is lost to the surroundings or to the calorimeter.
A sample of sucrose, C12H22O11, is contaminated by sodium chloride. When the contaminated sample is burned in a bomb calorimeter, sodium chloride does not burn. What is the percentage of sucrose in the sample if a temperature increase of 1.67C is observed when 3.000 g of the sample are burned in the calorimeter? Sucrose gives off 5.64103kJ/mol when burned. The heat capacity of the calorimeter and water is 22.51 kJ/C.
Fructose is a sugar commonly found in fruit. A sample of fructose, C6H12O6, weighing 4.50 g is burned in a bomb calorimeter that contains 1.00 L of water (d=1.00g/mL). The heat capacity of the calorimeter is 16.97 kJ/PC. The temperature of the calorimeter and water rise from 23.49C to 27.72C. (a) What is q for the calorimeter? (b) What is q for water in the calorimeter? (c) What is q when 4.50 g of fructose are burned in the calorimeter? (d) What is q for the combustion of one mole of fructose?
9.102 A runner generates 418 kJ of energy per kilometer from the cellular oxidation of food. The runner's body must dissipate this heat or the body will overheat. Suppose that sweat evaporation is the only important cooling mechanism. If you estimate the enthalpy of evaporation of water as 44 kJ/mol and assume that sweat can he treated as water, describe how you would estimate the volume of sweat that would have to be evaporated if the runner runs a 10-km race.
A bomb calorimetric experiment was run to determine the enthalpy of combustion of ethanol. The reaction is C2H5OH() + 3 O2(g) 2 CO2(g) + 3 H2O() The bomb had a heat capacity of 550 J/K, and the calorimeter contained 650 g of water. Burning 4.20 g of ethanol, C2HsOH() resulted in a rise in temperature from 18.5 C to 22.3 C. Calculate U for the combustion of ethanol, in kJ/mosl.
In a constant-pressure calorimeter that is, one that expands or contracts if the volume of the system changes, 0.145 mole of an ideal gas contracts slowly from 5.00 L to 3.92 L. If the initial temperature of the gas is 0.0 C, calculate the U and w for the process.
In earlier times, ethyl ether was commonly used as an anesthetic. It is, however, highly flammable. When five milliliters of ethyl ether, C4H10O(l)(d=0.714g/mL), are burned in a bomb calorimeter, the temperature rises from 23.5C to 39.7C. The calorimeter contains 1.200 kg of water and has a heat capacity of 5.32 kJ/C. (a) What is qH2o? (b) What is qcal? (c) What is q for the combustion of 5.00 mL of ethyl ether? (d) What is q for the combustion of one mole of ethyl ether?
9.104 An engineer is using sodium metal as a cooling agent in a design because it has useful thermal properties. Looting up the heat capacity, the engineer finds a value of 28.2 J mol-l °C-l. Carelessly, he wrote this number down without units. As a result, it was later taken as specific heat. (a) What would he the difference between these two values? (b) Would the engineer overestimate the ability of sodium to remove heat from the system or underestimate it because of this error? Be sure to explain your reasoning.
9.91 You want to heat the air in your house with natural gas (CH4). Assume your house has 275 m2(ahout 2800 ft2) of floor area and that the ceilings are 2.50 m from the floors. The air in the house has a molar heat capacity of 29.1 J mol-l K-l. (The number of moles of air in the house may he found by assuming that the average molar mass of air is 28.9 g/mol and that the density of air at these temperatures is 1.22 g/L.) What mass of methane do you have to burn to heat the air from 15.0 to 22.0°C?