The heat of combustion (AHºJ is:an experimental value for the energy released when ahydrocarbon is burned in aira theoretical value for the energy released when a molecule isformed from its component elements in their standard atomicstatesO an experimental value for the energy released when ahydrocarbon is treated with H2 and Pdan experimental value for the energy released when a molecule isformed from its component elements in their standard atomicstates

Heat of combustion is also known as enthalpy of combustion. It is the amount of heat energy released…

The heat of combustion (AHºJ is: an experimental value for the energy released when a hydrocarbon is burned in air a theoretical value for the energy released when a molecule is formed from its component elements in their standard atomic states an experimental value for the energy released when a hydrocarbon is treated with H2 and Pd an experimental value for the energy released when a molecule is formed from its component elements in their standard atomic states

The heat of combustion (AHºJ is: an experimental value for the energy released when a hydrocarbon is burned in air a theoretical value for the energy released when a molecule is formed from its component elements in their standard atomic states an experimental value for the energy released when a hydrocarbon is treated with H2 and Pd an experimental value for the energy released when a molecule is formed from its component elements in their standard atomic states

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

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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A 34.3 g sample of ethanol (C2H5OH) is burned in a bomb calorimeter containing a certain mass of water. If the temperature rose from 35.0 to 76.7°C, how much water, in kg, must the bomb calorimeter have contained? The molar mass of ethanol is 46.07 g/mol. Assume that the calorimeter doesn't absorb any heat. The specific heat of water is 4.184 J/g °C. C2H5OH(l) + 3 O2(g) → 2 CO2(g) + 3 H2O(g) ΔH°rxn = -1.24 x 103 kJ/mol
A 33.4 g sample of ethanol (C2H5OH) is burned in a bomb calorimeter containing a certain mass of water. If the temperature rose from 35.0 to 74.8°C, how much water, in kg, must the bomb calorimeter have contained? The molar mass of ethanol is 46.07 g/mol. Assume that the calorimeter doesn't absorb any heat. The specific heat of water is 4.184 J/g °C. C2H5OH(l) + 3 O2(g) → 2 CO2(g) + 3 H2O(g) ΔH°rxn = -1.24 x 103 kJ/mol
A 36.7 g sample of ethanol (C2H5OH) is burned in a bomb calorimeter containing a certain mass of water. If the temperature rose from 35.0 to 75.2°C, how much water, in kg, must the bomb calorimeter have contained? The molar mass of ethanol is 46.07 g/mol. Assume that the calorimeter doesn't absorb any heat. The specific heat of water is 4.184 J/g °C. C2H5OH() + 3 O2(g) → 2 CO2(s) +3 H20(g) AH°rxn 1.24 x 103 kJ/mol Please do not include units in your answer. Assume all numbers have at least 3 sig figs.
▾ Part A For a hypothetical reaction X(g) → Y(g), you are told that the enthalpy of Y(g) is greater than that of X(g). Which of the following statements is false? O The enthalpies of X(g) and Y(g) could both have negative values. O AH for the reaction is positive. O The reaction is endothermic. O On an enthalpy diagram, the line for Y(g) is below the line for X(g). Submit Provide Feedback Request Answer Next >
The burning of 28g of vegetable cause the temperature of 58.18 g of water in a soda can calorimeter to increase from 21.5°C to 28.1 Calculate the amount of heat absorbed by the water using the specific heat of water at 4.18 J/gºC.
Food contains three main categories of compounds: carbohydrate, protein, and fat. Arctic explorers often eat a high-fat diet because fats have a high food value. The average food values for carbohydrate, protein, and fat are 4 Cal/g, 4 Cal/g, and 9 Cal/g, respectively. Consider a typical fat to have the chemical formula C18H36O2, glucose (C6H12O6) to be a representative carbohydrate, and the amino acid alanine (C3H6NO2) a building block of proteins. Express the food values given above in kJ/mol.
Use the following information to answer Questions 6-9: A sample of NH4NO3 with a mass of 5.0 g is dissolved in 40.1 g of deoinized water in a calorimeter. The initial temperature of the water is 21.2 oC. The final temperature of the solution is 15.4 oC. The calorimeter constant = 25.2 J/oC. Is the following statement true or false? This process is exothermic. True False
A 3.59°C increase in temperature occurs when a 0.232 g sample of benzoic acid (C7H6O2) is combusted in a bomb calorimeter. A 1.81 °C increase in temperature occurs when a 0.303 g sample of citric acid (C6H8O7) is combusted in the same bomb calorimeter. The heat of combustion of benzoic acid is -26.37 kJ/g. What is the molar heat of combustion of citric acid? Reminder: Any heats of combustion will be negative since these are exothermic reactions.
The flame in a torch used to cut metal is produced by burning acetylene (C2H2)(26.04 g/mol) in pure oxygen. Assuming the combustion of 1 mole of acetylene releases 1251 kJ of heat, what mass of acetylene is needed to cut through a piece of steel if the process requires 22.5 × 104 kJ of heat? 2 C2H2(g) + 5 O2(g) → 4 CO2(g) + 2 H2O(g) ΔH = –2502 kJ
The combustion of 0.1566 g benzoic acid increases the temperature of a bomb calorimeter by 2.51°C. Calculate the heat capacity of this calorimeter. (The energy released by combustion of benzoic acid is 26.42 kJ/g.) Heat capacity = kJ/°C A 0.2195-g sample of vanillin (Cg H3 O3) is then burned in the same calorimeter, and the temperature increases by 3.21°C. What is the energy of combustion per gram of vanillin? Energy = kJ/g Per mole of vanillin? Energy = kJ/mol
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