wires heat sample Water Stirrer nud Sample buming Steel sample outside chamber In an experiment, a 0.5315 g sample of 1-naphthoic acid (Cu HaO₂) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.091 x 10³ g of water. During the combustion the temperature increases from 21.63 to 24.37 "C. The heat capacity of water is 4.184 J-g¹.0¹. The heat capacity of the calorimeter was determined in a previous experiment to be 983.1 J. "C Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of 1-naphthoic acid based on these data. C₁ H₂O₂(0)+120₂ (9) 4H₂O()+11C0₂(g) + Energy kJ/mol Molar Heat of Combustion -

wires heat sample Water Stirrer nud Sample buming Steel sample outside chamber In an experiment, a 0.5315 g sample of 1-naphthoic acid (Cu HaO₂) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.091 x 10³ g of water. During the combustion the temperature increases from 21.63 to 24.37 "C. The heat capacity of water is 4.184 J-g¹.0¹. The heat capacity of the calorimeter was determined in a previous experiment to be 983.1 J. "C Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of 1-naphthoic acid based on these data. C₁ H₂O₂(0)+120₂ (9) 4H₂O()+11C0₂(g) + Energy kJ/mol Molar Heat of Combustion -

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 138.9 g sample of an unknown metal at a temperature of 99.1 °C is added to 44.72 g of water at a temperature of 19.1 °C. The specific heat of water is 4.184 Jg-1 °C- 1. The final temperature of the system is 52.2°C. Calculate the specific heat of the unknown metal.
A 22.1g piece of aluminum (which has a molar capacity of 24.03 J/oC.mol) is heated to 82.4oC and dropped into a calorimeter containing water (specific heat capacity of water is 4.18J/goC) initially at 22.3oC. The final temperature of the water is 25.8oC. Ignoring significant figures, calculate the mass of the water in the calorimeter.
NW113AACE04-21 3. a hunk of metal-like substance was found in an archeological site. In an attempt to identify it, the metal was heated and placed in a calorimeter containing water and determined the specific heat of the metal. If the specific heat of the metal is 0.448 J/g °C, what is the approximate molar mass (atomic mass) and likely identity of the metal? (Hint: compare the molar mass (atomic mass) of metal that of metals in periodic table)
A 6.78 g sample of methanol was combusted in a bomb calorimeter. The temperature of the calorimeter increased by 12.7 °C. If the molar mass of methanol is 32.04 g/mol, and the heat capacity of the calorimeter is 5,104 J/°C, what is the molar AE for this reaction, in kJ/mol? Do not report units in your answer. Report your answer to one decimal place and include the correct sign.
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?
calculate the heat (in J) of the reaction if 50.0 mL of HCl is added to 50.0 mL of NaOH in a coffee-cup calorimeter. The initial temperature for both solutions is 23.2oC. At the end of the reaction after the data is graphed, the final temperature is determined to be 38.5oC.
10 A student heats 84.17 mL of water to 95.27°C using a hot plate. The heated water is added to a calorimeter containing 73.92 mL of cold water. The water temperature in the calorimeter rises from 2.15°C to 37.48°C. The specific heat capacity of water is 4.184 J and the density of water is g. °C 1.00 mL Assuming that heat was transferred from the hot water to the cold water and the calorimeter, determine the heat capacity of the calorimeter. J Heat capacity of calorimeter = °C
A 2.74 g sample of methanol, CH3OH, is combusted in a bomb calorimeter. The temperature of the calorimeter increases by 10.1°C. If the heat capacity of the bomb is 727.1 J/°C and it contains 1200 kg of water, what is the heat evolved in kJ/mol of methanol combusted? The specific heat capacity of water is 4.184 J/g°C and the molar mass of methanol is 32.04 g/mol. Show your answer in TWO (2) decimal places.
An unknown sample of coal is burned in an apparatus with a calorimeter constant of 0.8 kJ/°C. When a 0.443-g sample is used, the temperature change is 8.61°C. What is the energy density of the sample in kJ/g?
6, A 0.213 g sample of an organic compound with a molar mass of 386.0 g/mol was burned in the bomb calorimeter with a heat capacity of 2.54 kJ/K. The temperature in the calorimeter increased by 4.12 K. Calculate the energy of combustion of the compound in kJ/mol. A, –1.896 x103 B, –4.90 x102 C, 0.00937 D, –1.90 x104 E, -531
2. Consider the equation for the combustion of acetone (C₁H₂O), the main ingredient in nail polish remover. AHR -1790 kJ CHO (l)+4Oz (g) -> 3 CO, (g)+3H,O (g) If a bottle of nail polish remover contains 255 g of acetone, how much heat is released by its complete combustion?
A student has calibrated his/her calorimeter and finds the heat capacity to be 14.8 J/°C. S/he then determines the molar heat capacity of aluminum. The data are: 25.7 g Al at 100.0°C are put into the calorimeter, which contains 99.8 g H20 at 18.5°C. The final temperature comes to 22.6°C. Calculate the heat capacity of Al in J/mol-°C