1. The enthalpy of combustion (AH") of 3-ethyl-2-methylpentane (CgH18) is -5471.00 kJ/mol. Using the appropriate information given below, calculate the enthalpy of formation (AH";), in kl/mol, for 3-ethyl-2-methylpentane.Report your answer to two decimal places.AH", (CO, (9)) = -393.51 k)/molAH°, (H20 (1)) = -285.83 kl/molSubmit Answer Tries 0/52. Determine the mass (in g) of 3-ethyl-2-methylpentane produced, if AH° was determined to be -159.71 k during an experiment in which 3-ethyl-2-methylpentane was formed.Report your answerthree significant figures.

Given: ΔHo rxn = -5471.00 KJ/mol Hof(O2(g)) = 0.0 KJ/mol Hof(CO2(l)) = -393.51 KJ/mol Hof(H2O(g)) =…

1. The enthalpy of combustion (AH") of 3-ethyl-2-methylpentane (CeHs) is -5471.00 k3/mol. Using the appropriate information given below, calculate the enthalpy of formation (AH"), in k/mol, for 3-ethyl-2-methylpentane. Report your answer to two decimal places. AH", (CO, (9))- -393.51 k/mol AH", (H,0 (1)) -285.83 k/mol Submit Answer Tries 0/s 2. Determine the mass (in g) of 3-ethyl-2-methylpentane produced, if AH° was determined to be -159.71 ka during an experiment in which 3-ethyl-2-methylpentane was formed. Report your answer to three significant figures.

1. The enthalpy of combustion (AH") of 3-ethyl-2-methylpentane (CeHs) is -5471.00 k3/mol. Using the appropriate information given below, calculate the enthalpy of formation (AH"), in k/mol, for 3-ethyl-2-methylpentane. Report your answer to two decimal places. AH", (CO, (9))- -393.51 k/mol AH", (H,0 (1)) -285.83 k/mol Submit Answer Tries 0/s 2. Determine the mass (in g) of 3-ethyl-2-methylpentane produced, if AH° was determined to be -159.71 ka during an experiment in which 3-ethyl-2-methylpentane was formed. Report your answer to three significant figures.

Physical Chemistry

2nd Edition

ISBN:9781133958437

Author:Ball, David W. (david Warren), BAER, Tomas

Publisher:Ball, David W. (david Warren), BAER, Tomas

Chapter2: The First Law Of Thermodynamics

Section: Chapter Questions

Problem 2.83E: Benzoic acid, C6H5COOH, is a common standard used in bomb calorimeters, which maintain a constant...

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The enthalpy of reaction for the combustion of C to CO2 is -393.5 kJ>mol C, and the enthalpy for the combustion of CO to CO2is -283.0 kJ>mol CO:(1) C1s2 + O21g2 ---> CO21g2 ΔH = -393.5 kJ(2) CO1g2 + 12O21g2 ----> CO21g2 ΔH = -283.0 kJUsing these data, calculate the enthalpy for the combustion of C to CO:(3) C1s2 + 12 O21g2 ---->CO1g2 ΔH = ?
For the following combustion reaction of benzoic acid (HC7H5O2; molar mass = 122.1 g/mol) HC7H5O2(s) + 15/2 O2(g) --> 7CO2(g) + 3H2O(l); DHcomb = -3226 kJ 1.00 g of benzoic acid is combusted in a bomb calorimeter, which contains 1.00 kg of water (specific heat = 4.184 J/g.oC) and the bomb has a heat capacity of 890 J/oC. If the initial temperature of the calorimeter is 25.0oC, what is the final temperature of the calorimeter when the combustion is completed? (A) 51.8oC (B) 31.3oC (C) 30.2oC (D) 27.0oC
The complete combustion of 1.200 g of cinnamaldehyde (C9H8O), in a bomb calorimeter (Cbc = 3.640 kJ/oC) produces an increase in temperature of 12.79oC. What is the enthalpy, dH, for the combustion of one mole of cinnamaldehyde?(hint: q = ?, molar mass C9H8O = ?)
standard enthalpy of combustion for butan-1-ol is -2685 kJ/mol and is given bythe following reaction equation.CHaCH?CH2CH2OH(/) + 6 02(8) - 4 CO2(8) + 5 H20(/)The formation of carbon dioxide and liquid water are given by these equations.C(s) + 02(g) - CO2(g) AH° = -394 kJ/molH2(g) + 0.5 02(g) - H20(/) AH° = -286 kJ/molUsing these data, determine the standard enthalpy of fbrmation for butan-1-ol. Report your answer in kJ/mol with no decimal place in the answer.
The enthalpy of reaction for the combustion of C to CO2 is -393.5 kJ/mol C, and the enthalpy for the combustion of CO to CO2 is -283.0 kJ/mol CO:(1) C(s) + O2(g) -----> CO2(g) ΔH = -393.5 kJ(2) CO(g) + 1/2O2(g) -------> CO2(g) ΔH = -283.0 kJUsing these data, calculate the enthalpy for the combustion of C to CO:(3) C(s) + 1/2 O2(g) ------> CO(g) ΔH = ?
Under a constant pressure of 1.00 atm, at 25.00oC, the combustion of 1.136 g of C6H12O3(l) raises the temperature of 2.000 kg of water by 2.617 degrees Celsius. Combustion is the reaction of a substance with O2(g) to give CO2(g) and H2O(l). The specific heat capacity of water is 4.184 J K-1 g-1. Ignore the heat capacities of any containers.With the help of the data above, find the values of ΔH, ΔU, Q, and W for the combustion of 1.000 mol of C6H12O3(l) in a steel container of constant volume at 25.00oC.
When 0.659g of glucose (C6H12O6) undergoes combustion 8n a constant volume (bomb) calorimeter, the temperature rises from the initial temperature of 295.6K. If the deltaE rxn for the combustion of glucose is -2801kJ/mol, and the heat capacity of the bomb calorimeter is known to be 7.27kj/K, what is the final temperature of the calorimeter in K?
The heat of combustion of propan-2-ol at 298.15 K, determined in a bomb calorimeter, is -33.41kJ/g. For the combustion of one mole of propan-2-ol, determine ΔrH. Express your answer using four significant figures.
o-phthalic acid, C8H6O4, is sometimes used as a calorimetric standard. Its heat ofcombustion is - 3.224 × 103 kJ/mol C8H6O4. From the following data determine theheat capacity of a bomb calorimeter assembly (i.e., of the bomb, water, stirrer,thermometer, wires, etc.)mass of o-phthalic acid burned: 1.078 ginitial calorimeter temperature 24.96 °Cfinal calorimeter temperature 30.76 °C
A sample of methylhydrazine (rocket fuel) weighing 1.500 g was ignited in a bomb calorimeter initially at 25.0°C, producing a temperature rise of 10.215 K. Determine the internal energy (∆U) of combustion of methylhydrazine. a) To properly determine the internal energy of combustion methylhydrazine, the calorimeter was first calibrated. A 0.5000 g sample of sucrose (MW 342.296 g/mol)) was ignited under identical conditions and produced a temperature rise of 1.98 K. For sucrose, the internal energy combustion at constant volume, ∆U, is known to be –5616.64 kJ/mol. Calculate the calorimeter constant, in kJ/K. b) Using the calorimeter constant, determine ∆U, in kJ/mol, of combustion of the methylhydrazine (CH₆N₂, MW 46.10 g/mol).
A pellet of benzoic acid standard was combusted in a bomb calorimeter to determine the experimental calorimeter constant. After 6 mins of monitoring the temperature, the bomb was fired. The following data were obtained. mole of benzoic acid: 0.0049 mol mass of burnt fuse wire: 0.0117 g qwire,surr: 5858 J/g ΔHcombustion of benzoic acid: -3228.0 kJ/mol Δng (combustion of benzoic acid): -0.5 mol R: 8.314 J/mol•K r1: 0ºC/min r2: 0ºC/min Tf: 30.5ºC Ti: 28.4ºC Determine the calorimeter constant (in J/ºC). Report your answer in 2 decimal places.
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