A 5.500 g sample of liquid fuel (molar mass of 32 g/mole), was combusted in thepresence of excess oxygen in a bomb calorimeter containing 3000 g of water. Thetemperature of the water increased from 25.000 °C to 30.765 °C. The heatcapacity of the calorimeter was 2655 J/°C. The specific heat of water is 4.184J/g°C. Calculate the heat of combustion of the liquid fuel in kJ/mol.a. -510 kJ/molO b. -314 kJ/mol-69.5 kJ/molO d. -121 kJ/molO e. -716 kJ/mol

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Answered: A 5.500 g sample of liquid fuel (molar…

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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When a 4.31 g sample of liquid octane (C8H18) is burned in a bomb calorimeter, the temperature of the calorimeter rises by 27.3 °C. The heat capacity of the calorimeter, measured in a separate experiment, is 6.2 kJ/•C. The calorimeter also contains 3.00 kg of water, specific heat capacity of 4.18 J/g°C. Determine the heat of combustion of octane in units of kJ/mol octane. Enter your answer numerically and in terms of kJ/mol.
A 3.000 g sample of food was then burned in a calorimeter to determine its Calories per gram content. 50mL of water were used to determine ΔT of the reaction. Initial temperature of the water at the start of the combustion reaction was 20oC, final temperature was 99oC. Calorimeter constant for this calorimeter is 10.0J/oC. How much heat has been absorbed by the water sample?
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In a coffee-cup calorimeter, 120.0 mL of 1.4 M NaOH and 120.0 mL of 1.4 M HCL are mixed. Both solutions were originally at 20.6°C. After the reaction, the final temperature is 30.0°C. Assuming that all the solutions have a density of 1.0 and a specific heat capacity of 4.18 J/°C·g, calculate the enthalpy change for the neutralization of HCL by NaOH . Assume that no heat is lost to the surroundings or to the calorimeter. ΔH = kJ/mol
A gaseous fuel mixture contains 23.2% methane (CH4), 40.8% ethane (C₂H6) and the rest propane (C3H8) by volume. Part A When the fuel mixture contained in a 1.55 L tank, stored at 756 mmHg and 298 K, undergoes complete combustion, how much heat is emitted? (Assume that the water produced by the combustion is in the gaseous state.) Express your answer with the appropriate units. μA Value Units Review | Constants | Periodic Table ?
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25.00 mL of 0.200 M sulfuric acid was added to 25.00 mL of 0.200 M NAOH, in a constant volume calorimeter. The density of the resulting solution is 1.225 g/mL and its specific heat is 5.321 J/g-°C. As the reaction took place, the temperature of the solution rose from 22.0 °C to 31.3 °C. What is AH (in units of kJ/mol) for the reaction, per mole of water formed? This is a limiting reactant problem and your choice of limiting reactant must be justified through stoichiometric calculations. 21.
A 47.70 mL volume of 1.00 M HCl was mixed with 47.30 mL of 2.00 M NaOH in a coffee cup calorimeter (with calorimeter constant = 25.0 J/°C) at 21.71 °C. The final temperature of the aqueous solution after the reaction was 29.73 °C. Assuming that them heat capacity of the solution is 4.18 J/g/°C, calculate the following: The enthalpy change (∆H) for the neutralization in kJ/mol HCl ( this should be a negative number) in kJ/mol HCl
[References] The combustion of 0.1586 g benzoic acid increases the temperature of a bomb calorimeter by 2.50°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 0.2113-g sample of vanillin (C8H3 O3) is then burned in the same calorimeter, and the temperature increases by 3.29°C. What is the energy of combustion per gram of vanillin? Energy kJ/g Per mole of vanillin? Energy kJ/mol Submit Answer Try Another Version 3 item attempts remaining

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