A 1.107-g sample of benzoic acid (HC;H;O:) is burned in an excess of O:(g) in a bomb calorimeter, which is immersed in water. The reaction produces heat that causes the temperature of the water and bomb to increase from 24.96 to 29.20°C. (a) If the heat capacity of the calorimeter is 6.90 KJºC, how many kilojoules of heat are produced by the combustion of 1.107 g of benzoic acid? (b) Calculate the heat of combustion per gram of benzoic acid and the molar enthalpy of combustion of benzoic acid.

A 1.107-g sample of benzoic acid (HC;H;O:) is burned in an excess of O:(g) in a bomb calorimeter, which is immersed in water. The reaction produces heat that causes the temperature of the water and bomb to increase from 24.96 to 29.20°C. (a) If the heat capacity of the calorimeter is 6.90 KJºC, how many kilojoules of heat are produced by the combustion of 1.107 g of benzoic acid? (b) Calculate the heat of combustion per gram of benzoic acid and the molar enthalpy of combustion of benzoic acid.

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...

See similar textbooks

Similar questions

An 8.000 g sample of methane, CH4, was burned in a bomb calorimeter whose total heat capacity is 11.66 kJ/oC. The temperature of the calorimeter plus the contents increased from 22oC to 60oC. What is the heat of combustion per gram of methane? What is the molar heat of combustion of methane?
A 0.600 g sample of tristearin (C57H11O6), a common fat, is combusted in a bomb calorimeter containing 750.0 g of water. The heat capacity of the calorimeter is 326 J/K. The initial temperature is 19.5 °C. It is known that the heat of combustion of tristearin is -38.0 kJ/g. The specific heat capacity of water is 4.184 J/g.K.(a) How much heat (in kJ) is released by this reaction? (b) What is the final temperature (in °C)?
Methanol is an organic solvent that can be used as a fuel in some automobiles. 2 CH3OH() + 3 02(g) → 2 CO2(g) +4 H20 (/) AH = -1452.8 kJ/mol How much heat (kJ) is evolved when 35 mL of methanol (CH3OH) with a density of 0.792 g/mL heated in the presence of excess oxygen gas?
An experiment is carried out where 12.2g of NaOH is dissolved in 240.0g of water in a coffee cup calorimeter. Dissolution is not a chemical reaction, but is a chemical process. NaOH(s) → Na+(aq) + OH-(aq) The mixture can be assumed to have the same specific heat capacity as liquid water (4.18J/g.C) What is the massof the sorroundings where the temperature is being measured in this experiment?
A bomb calorimeter has a heat capacity of 2.47 kJ/?. When a 1.00 mol sample of a certain hydrocarbon was burned in this calorimeter, the temperature increased by 2.14?. Calculate the heat of combustion per mole of the hydrocarbon.
An experiment was performed to calculate the heat of solution for potassium fluoride. Use the following data to determine its heat of solution. Assume that the specific heat capacity of the solution produced is the same as that of water, 4.184 J⁄g·°C. Identity of Salt KF Mass of water in calorimeter (g) 52.42 Mass of salt sample (g) 7.32 Initial temperature of Calorimeter (°C) 20.8 Final temperature of Calorimeter (°C) 30.3 Report your answer in kJ/mol to 3 significant figures.
When 1.091 grams of sucrose (Molar mass 342.3 g/mol) is burned in a bomb calorimeter, the temperature of the calorimeter increases from 22.41°C to 26.63°C. If the heat capacity of the calorimeter is 4.900 kJ/°C, what is the heat of combustion of sucrose, in kJ/mol?
A) When 1.911 grams of sucrose (Molar mass 342.3 g/mol) is burned in a bomb calorimeter, the temperature of the calorimeter increases from 22.410 °C to 26.630 °C. If the heat capacity of the calorimeter is 4.900 kJ/ °C, what is the heat of combustion of sucrose, in kJ/mol? And B) A 90.0 g piece of metal, initially at 98.60 °C, is placed into 120.0 g of water initially at 24.30 °C. If the final temperature of the water is 34.00 °C, what is the specific heat of the metal? (The specific heat of water is 4.184 J/g･ °C).
A student runs two experiments with a constant-volume "bomb" calorimeter containing 1200.g of water First, a 5.500g tablet of benzoic acid C6H5CO2H is put into the "bomb" and burned completely in an excess of oxygen. (Benzoic acid is known to have a heat of combustion of 26.454kJ/g.) The temperature of the water is observed to rise from 16.00°C to 44.20°C over a time of 10.7 minutes. Next, 5.120g of ethanol C2H5OH are put into the "bomb" and similarly completely burned in an excess of oxygen. This time the temperature of the water rises from 16.00°C to 41.79°C. Use this information, to answer the questions below about this reaction: A "bomb" calorimeter. C2H5OH(l) + 3O2(g) → 2CO2(g) 3H2O(g) Be sure any of your answers that are calculated from measured data are rounded to the correct number of significant digits. Note for advanced students: it's possible the student did not do these experiments sufficiently carefully, and the values you calculate may not exactly…
In a constant‑pressure calorimeter, 55.0 mL of 0.340 M Ba(OH)2 was added to 55.0 mL of 0.680 HCl. The reaction caused the temperature of the solution to rise from 23.90 ∘C to 28.53 ∘C. If the solution has the same density and specific heat as water, what is heat absorbed by the solution? Assume that the total volume is the sum of the individual volumes. (And notice that the answer is in kJ).
When 1.151 grams of sucrose (Molar mass 342.3 g/mol) is burned in a bomb calorimeter, the temperature of the calorimeter increases from 22.41°C to 26.63°C. If the heat capacity of the calorimeter is 4.900 kJ/°C, what is the heat of combustion of sucrose, in kJ/mol?
An unknown sample of coal is burned in an apparatus with a calorimeter constant of 1.62 kJ/°C. When a 0.298-g sample is used, the temperature change is 8.72°C. What is the energy density of the sample in kJ/g?