THERMODYNAMICS: A 1.1 g sample of acetic acid (HC2H302) was burned in excess oxygen in a bomb calorimeter. The calorimeter, which alone had a heat capacity of 2.67 kJ/°C, contained 7 g of water. The temperature of the calorimeter and its contents increased from 24.7°C to 27.95°C. What is AH (in kJ) for the combustion per 1.00 mol of acetic acid? MW of acetic acid is 60 g/mol. (Round off the final answer to ONE decimal place. Do not include the unit.)

THERMODYNAMICS: A 1.1 g sample of acetic acid (HC2H302) was burned in excess oxygen in a bomb calorimeter. The calorimeter, which alone had a heat capacity of 2.67 kJ/°C, contained 7 g of water. The temperature of the calorimeter and its contents increased from 24.7°C to 27.95°C. What is AH (in kJ) for the combustion per 1.00 mol of acetic acid? MW of acetic acid is 60 g/mol. (Round off the final answer to ONE decimal place. Do not include the unit.)

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

A student transferred 50.0 ml 1.00 M HCl into a coffee-cup calorimeter, which had a temperature of 25.5 °C. He then added this to 50.0 ml 1.00 M NaOH which also had a temperature of 25.5 °C and stirred the mixture quickly. The resulting solution was found to have a temperature of 32.5 °C. The calorimeter constant for the coffee-cup calorimeter used was 15.0 J/°C. Calculate the heat of reaction. Please include the full solution.
1. The metabolism of one mole of glycerol trioleate, C5 H9306, a common fat, produces 3.022 x 10¹kJ of heat. How many grams of the fat must be burned to raise the temperature of 50 g of water from 25.0°C to 30.0°C? 2. A metal sample having a temperature of 100°C and a mass of 45.2 g was placed in 50 g of water with a temperature of 26°C. At equilibrium, the final temperature was 32.7°C a) How much heat flowed into the water? b) What is the specific heat of the metal?
In a laboratory investigation into the neutralization reaction; HNO3 (aq) + NaOH(s) → NaNO3 (aq) + H2O (l) a researcher adds 5.3 g of solid sodium hydroxide to 200.0 mL of 1.0 M nitric acid solution in a polystyrene calorimeter. The temperature changes from 21.0°C to 28.5°C. Calculate the molar enthalpy of neutralization of sodium hydroxide.
4. The reaction of 250.0 mL of a 1.00 M hydrochloric acid solution with 250.0 mL of a 1.00 M sodium hydroxide solution was carried out in a constant pressure calorimeter. The total heat capacity of the calorimeter plus solutions was 6.45 kJ/K. The temperature of the calorimeter and solutions increased by 2.11°C. What is AH (in kJ) for the neutralization of 1.00 mol HCl(aq) by NaOH(aq)? A) -54.4 B) -21.2 +12.6 +54.4 E) -12.6
A 1.595 g samples of a new organic material is combusted in a bomb calorimeter. The temperature of the calorimeter and its contents increase from 23.67 degrees Celsius to 29.44 degrees Celsius. The heat capacity (calorimeter constant) of the calorimeter is 30.29 kJ/degrees Celsius, what is the heat of combustion per gram of the material?
When 1.836 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?
When 1.366 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?
THERMODYNAMICS: A 1.96 g sample of acetic acid (HC;H3O2) was burned in excess oxygen in a bomb calorimeter. The calorimeter, which alone had a heat capacity of 2.67 kJ/°C, contained 776 g of water. The temperature of the calorimeter and its contents increased from 24.51°C to 27.95°C. What is AH (in kJ) for the combustion per 1.00 mol of acetic acid? MW of acetic acid is 60 g/mol. (Round off the final answer to ONE decimal place) Round your answer to 1 decimal place.
In a coffee-cup calorimeter, 110.0 mL of 1.3 M and 110.0 mL of 1.3 M are mixed. Both solutions were originally at 22.2°C. After the reaction, the final temperature is 30.9°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 in (kJ/mol). Assume that no heat is lost to the surroundings or to the calorimeter.
In an experiment, a 0.4481 g sample of 2-naphthylacetic acid ( C12H10 O2) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.290 10³ g of water. During the combustion the temperature increases from 28.40 to 30.68 °C. The heat capacity of water is × -1.°C-¹. 4.184 J The heat capacity of the calorimeter was determined in a previous experiment to be 928.7 J. C-¹. Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of 2-naphthylacetic acid based on these data. C12H10 O2 (s) + (27/2) O2(g) → 5H₂O(1) + 12CO2(g) + Energy kJ/mol e g Molar Heat of Combustion =
In a constant pressure coffee-cup calorimeter, 100.0 mL of 0. 050 M of Ag+ was mixed with 100.0 ml of 0.050 M of Cl‒. The temperature changed from 298.5 K to 299.4 K. Calculate the enthalpy of reaction, ΔH (kJ/mol). Assume that the solutions have a density of water (1 g/mL) and specific heat capacity of water (4.184 J/g °C). Ag+(aq) + Cl‒(aq) ⟶ AgCl(s)