Thermometer Ignition wires heat Stirrer sample A bomb calorimeter, or a constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy content of foods. In an experiment, a 0.4241 g sample of diphenylacetylene (C14H10) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.158×10 g of water. During the combustion Water the temperature increases from 21.80 to 24.74 °C. The heat capacity of water is 4.184 J gl°c-!. The heat capacity of the calorimeter was determined in a previous experiment to be 785.1 J/°C. Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of diphenylacetylene based on these data. C14H10(s) + (33/2) O2(g) 5 H2O(1) + 14 CO2(g) + Energy Insulated outside chamber Sample dish Burning sample Steel bomb Molar Heat of Combustion = kJ/mol animate

Thermometer Ignition wires heat Stirrer sample A bomb calorimeter, or a constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy content of foods. In an experiment, a 0.4241 g sample of diphenylacetylene (C14H10) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.158×10 g of water. During the combustion Water the temperature increases from 21.80 to 24.74 °C. The heat capacity of water is 4.184 J gl°c-!. The heat capacity of the calorimeter was determined in a previous experiment to be 785.1 J/°C. Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of diphenylacetylene based on these data. C14H10(s) + (33/2) O2(g) 5 H2O(1) + 14 CO2(g) + Energy Insulated outside chamber Sample dish Burning sample Steel bomb Molar Heat of Combustion = kJ/mol animate

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter7: Chemical Energy

Section: Chapter Questions

Problem 110AE: Quinone is an important type of molecule that is involved in photosynthesis. The transport of...

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Nitroglycerin, C3H5(NO3)3(l), is an explosive most often used in mine or quarry blasting. It is a powerful explosive because four gases (N2, O2, CO2, and steam) are formed when nitroglycerin is detonated. In addition, 6.26 kJ of heat are given off per gram of nitroglycerin detonated. (a) Write a balanced thermochemical equation for the reaction. (b) What is H when 4.65 mol of products are formed?
Salicylic acid, C7H6O3, is one of the starting materials in the manufacture of aspirin. When 1.00 g of salicylic acid burns in a bomb calorimeter, the temperature of the bomb and water goes from 23.11C to 28.91C. The calorimeter and water absorb 21.9 kJ of heat. How much heat is given off when one mole of salicylic acid burns?
Microwave ovens convert radiation to energy. A microwave oven uses radiation with a wavelength of 12.5 cm. Assuming that all the energy from the radiation is converted to heat without loss, how many moles of photons are required to raise the temperature of a cup of water (350.0 g, specific heat =4.18J/gC) from 23.0C to 99.0C?
A 0.470-g sample of magnesium reacts with 200 g dilute HCl in a coffee-cup calorimeter to form MgCl2(aq) and H2(g). The temperature increases by 10.9 C as the magnesium reacts. Assume that the mixture has the same specific heat as water and a mass of 200 g. (a) Calculate the enthalpy change for the reaction. Is the process exothermic or endothermic? (b) Write the chemical equation and evaluate H.
Quinone is an important type of molecule that is involved in photosynthesis. The transport of electrons mediated by quinone in certain enzymes allows plants to take water, carbondioxide, and the energy of sunlight to create glucose. A 0.1964-g sample of quinone (C6H4O2) is burned in a bomb calorimeter with a heat capacity of 1.56 kJ/C. The temperature of the calorimeter increases by 3.2C. Calculate the energy of combustion of quinone per gram and per mole.
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?
The value of U for the decomposition of 7.647 g of ammonium nitrate can be measured in a bomb calorimeter. The reaction that occurs is NH4NO3(s) N2O(g) + 2 H2O(g) The temperature of the calorimeter, which contains 415 g of water, increases from 18.90 C to 20.72 C. The heat capacity of the bomb is 155 J/K. What is the value of U for this reaction, in kl/mol?
When a 0.740-g sample of trinitrotoluene (TNT), C7H5N2O6, is burned in a bomb calorimeter, the temperature increases from 23.4 C to 26.9 C. The heat capacity of the calorimeter is 534 J/C, and it contains 675 mL of water. How much heat was produced by the combustion of the TNT sample?
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?
Assume 200. mL of 0.400 M HCl is mixed with 200. mL of 0.400 M NaOH in a coffee-cup calorimeter The temperature of the solutions before mixing was 25.10 C; after mixing and allowing the reaction to occur, the temperature is 27.78 C. What is the enthalpy change when one mole of acid is neutralized? (Assume that the densities of all solutions are 1.00 g/mL and their specific heat capacities are 4.20 J/g K.)
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.
The heat of neutralization, Hneut, can be defined as the amount of heat released (or absorbed), q, per mole of acid (or base) neutralized. Hneut for nitric acid is -52 kJ/mol HNO3. At 27.3C, 50.00 mL of 0.743M HNO3 is neutralized by 1.00 M Sr(OH)2 in a coffee-cup calorimeter. (a) How many mL of Sr(OH)2 were used in the neutralization? (b) What is the final temperature of the resulting solution? (Use the assumptions in Question 11.)